JEE Main & Advanced Chemistry Equilibrium / साम्यावस्था Question Bank

done Self Evaluation Test - Equilibrium Total Questions - 100

• question_answer1)
  The equilibrium constant for the reaction \[W+X\rightleftharpoons Y+Z\] is 9.Ifone mole of each of w and x are mixed and there is no change in volume, the number of moles of y formed is
  A)
  0.10  done clear
  B)
  0.50  done clear
  C)
  0.75  done clear
  D)
  0.54 done clear
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• question_answer2)
  When heated, ammonium carbamate decomposes as follows: \[N{{H}_{4}}COON{{H}_{2}}(s)\rightleftharpoons 2N{{H}_{3}}(g)+C{{O}_{2}}(g)\]. At a certain temperature, the equilibrium pressure of the system is 0.318 atm. \[{{K}_{p}}\] for the reaction is:
  A)
  0.128                done clear
  B)
  0.426 done clear
  C)
  \[4.76\times {{10}^{-3}}\]        done clear
  D)
  None of these done clear
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• question_answer3)
  One mole of \[S{{O}_{3}}\] was placed in a one litre reaction flask at a given temperature when the reaction equilibrium was established in the reaction. \[2S{{O}_{3}}\rightleftharpoons 2S{{O}_{2}}+{{O}_{2}}\]. The vessel was found to contain 0.6 mole of\[S{{O}_{2}}\]. The value of the equilibrium constant is
  A)
  0.36                  done clear
  B)
  0.675 done clear
  C)
  0.45                  done clear
  D)
  0.54 done clear
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• question_answer4)
  For the equilibrium system \[2HX(g)\rightleftharpoons {{H}_{2}}(g)+{{X}_{2}}(g)\] the equilibrium constant is \[1.0\times {{10}^{-5}}\]. What is the concentration of HX if the equilibrium concentration of \[{{H}_{2}}\] and \[{{X}_{2}}\] are\[1.2\times {{10}^{-3}}M\], and \[1.2\times {{10}^{-4}}M\] respectively.
  A)
  \[12\times {{10}^{-4}}M\]         done clear
  B)
  \[12\times {{10}^{-3}}M\] done clear
  C)
  \[12\times {{10}^{-2}}M\]         done clear
  D)
  \[12\times {{10}^{-1}}M\] done clear
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• question_answer5)
  If \[{{K}_{1}}\] and \[{{K}_{2}}\] are respective equilibrium constants for the two reactions \[Xe{{F}_{6}}(g)+{{H}_{2}}O(g)\rightleftharpoons XeO{{F}_{4}}(g)+2HF(g)\] \[Xe{{O}_{4}}(g)+Xe{{F}_{6}}(g)\rightleftharpoons XeO{{F}_{4}}(g)+Xe{{O}_{3}}{{F}_{2}}(g)\] the equilibrium constant for the reaction \[Xe{{O}_{4}}(g)+2HF(g)\rightleftharpoons Xe{{O}_{3}}{{F}_{2}}(g)+{{H}_{2}}O(g)\] will be
  A)
  \[\frac{{{K}_{1}}}{K_{2}^{2}}\]                                 done clear
  B)
  \[{{K}_{1}}.{{K}_{2}}\] done clear
  C)
  \[\frac{{{K}_{1}}}{{{K}_{2}}}\]                                   done clear
  D)
  \[\frac{{{K}_{2}}}{{{K}_{1}}}\] done clear
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• question_answer6)
  If 1.0 mole of \[{{I}_{2}}\] is introduced into 1.0 litre flask at 1000 K, at quilibrium \[({{K}_{c}}={{10}^{-6}})\], which one is correct
  A)
  \[\left[ {{I}_{2}}(g) \right]>\left[ {{I}^{-}}\left( g \right) \right]\]   done clear
  B)
  \[\left[ {{I}_{2}}(g) \right]<\left[ {{I}^{-}}\left( g \right) \right]\] done clear
  C)
  \[\left[ {{I}_{2}}(g) \right]=\left[ {{I}^{-}}\left( g \right) \right]\]   done clear
  D)
  \[\left[ {{I}_{2}}(g) \right]=\frac{1}{2}\left[ {{I}^{-}}\left( g \right) \right]\] done clear
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• question_answer7)
  In a reaction\[A+B~\rightleftharpoons C+D\], the initial concentrations, of A and B were 0.9 mol. \[d{{m}^{-3}}\]each. At equilibrium the concentration of D was found to be 0.6 mol \[d{{m}^{-3}}\]. What is the value of equilibrium constant for the reaction
  A)
  8                      done clear
  B)
  4   done clear
  C)
  9                                  done clear
  D)
  3 done clear
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• question_answer8)
  The partial pressure of \[C{{H}_{3}}OH(g),CO(g)\] and \[{{H}_{2}}(g)\] in equilibrium mixture for the reaction, \[CO(g)+2{{H}_{2}}(g)\rightleftharpoons C{{H}_{3}}OH(g)\] are 2.0, 1.0 and 0.1 atm respectively at \[427{}^\circ C\]. The value of \[{{K}_{p}}\] for the decomposition of \[C{{H}_{3}}OH\] to CO and \[{{H}_{2}}\] is
  A)
  \[{{10}^{2}}atm\]                                done clear
  B)
  \[2\times {{10}^{2}}at{{m}^{-1}}\] done clear
  C)
  \[50\text{ }at{{m}^{2}}\]                     done clear
  D)
  \[5\times {{10}^{-3}}at{{m}^{2}}\] done clear
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• question_answer9)
  3.2 moles of hydrogen iodide were heated in a sealed bulb at \[444{}^\circ C\] till the equilibrium state was reached. Its degree of dissociation at this temperature was found to be 22% The number of moles of hydrogen iodide present at equilibrium are
  A)
  2.496                done clear
  B)
  1.87    done clear
  C)
  2                                  done clear
  D)
  4 done clear
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• question_answer10)
  \[{{K}_{c}}\] for \[PC{{l}_{5}}(g)\rightleftharpoons PC{{l}_{3}}(g)+C{{l}_{2}}(g)\] is 0.04 at \[250{}^\circ C\]. How many moles of \[PC{{l}_{5}}\] must be added to a 3 L flask to obtain a \[C{{l}_{2}}\] concentration of 0.15M
  A)
  4.2 moles done clear
  B)
  2.1 moles done clear
  C)
  5.5 moles           done clear
  D)
  6.3 moles done clear
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• question_answer11)
  Gaseous \[{{N}_{2}}{{O}_{4}}\] dissociates into gaseous \[N{{O}_{2}}\]according to the reaction    \[[{{N}_{2}}{{O}_{4}}(g)\rightleftharpoons 2N{{O}_{2}}(g)]\] At 300 K and 1 atm pressure, the degree of dissociation of \[{{N}_{2}}{{O}_{4}}\] is 0.2. If one mole of \[{{N}_{2}}{{O}_{4}}\] gas is contained in a vessel, then the density of the equilibrium mixture is:
  A)
  1.56 g/L           done clear
  B)
  6.22 g/L done clear
  C)
  3.11g/L             done clear
  D)
  4.56 g/L done clear
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• question_answer12)
  The value of \[{{K}_{p}}\] for the equilibrium reaction \[{{N}_{2}}{{O}_{4}}(g)\rightleftharpoons 2N{{O}_{2}}(g)\] is 2.  The percentage dissociation of \[{{N}_{2}}{{O}_{4}}(g)\] at a pressure of 0.5 atm is
  A)
  25                     done clear
  B)
  88     done clear
  C)
  50                     done clear
  D)
  71 done clear
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• question_answer13)
  If  \[CuS{{O}_{4}}.5{{H}_{2}}O(s)\rightleftharpoons \] \[CuS{{O}_{4}}.3{{H}_{2}}O\left( s \right)+2{{H}_{2}}O\left( g \right)\] \[{{K}_{p}}=1.086\times {{10}^{-4}}at{{m}^{2}}\] at \[25{}^\circ C\]. The efflorescent nature of \[CuS{{O}_{4}}.5{{H}_{2}}O\] can be noticed when the vapour pressure of \[{{H}_{2}}O\] in atmosphere is
  A)
  >9.72mm          done clear
  B)
  <7.92mm done clear
  C)
  >7.92mm          done clear
  D)
  < 11.92mm done clear
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• question_answer14)
  \[28g\,{{N}_{2}}\] and 6.0 g of \[{{H}_{2}}\] are heated over catalyst in a closed one litre flask of\[450{}^\circ C\]. The entire equilibrium mixture required 500 mL of 1.0 M \[{{H}_{2}}S{{O}_{4}}\] for neutralisation. The value of \[{{K}_{c}}\] for the reaction \[{{N}_{2}}(g)+3{{H}_{2}}(g)\rightleftharpoons 2N{{H}_{3}}(g)\] is
  A)
  \[0.06\text{ }mo{{l}^{-2}}{{L}^{2}}\]            done clear
  B)
  \[0.59\text{ }mo{{l}^{-2}}{{L}^{2}}\] done clear
  C)
  \[1.69\text{ }mo{{l}^{2}}{{L}^{-2}}\]            done clear
  D)
  \[0.03\text{ }mo{{l}^{2}}{{L}^{-2}}\] done clear
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• question_answer15)
  A gaseous compound of molecular mass 82.1 dissociates on heating to 400 K as \[{{X}_{2}}{{Y}_{4}}(g)\rightleftharpoons {{X}_{2}}(g)+2{{Y}_{2}}(g)\] The density of the equilibrium mixture at a pressure of 1 atm and temperature of 400K is\[2.0g{{L}^{-1}}\]. The percentage dissociation of the compound is  
  A)
  12.5%               done clear
  B)
  48.5% done clear
  C)
  90.1%               done clear
  D)
  25.0% done clear
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• question_answer16)
  At \[527{}^\circ C\], the reaction given below has \[{{K}_{c}}=4\] \[N{{H}_{3}}(g)\rightleftharpoons \frac{1}{2}{{N}_{2}}(g)+\frac{3}{2}{{H}_{2}}(g)\] What is the \[{{K}_{p}}\] for the reaction? \[{{N}_{2}}(g)+3{{H}_{2}}(g)\rightleftharpoons 2N{{H}_{3}}(g)\]
  A)
  \[16\times {{(800R)}^{2}}\]                   done clear
  B)
  \[{{\left( \frac{800R}{4} \right)}^{-2}}\] done clear
  C)
  \[{{\left( \frac{1}{4\times 800R} \right)}^{2}}\]               done clear
  D)
  None of these done clear
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• question_answer17)
  At a certain temperature, only 50% HI is dissociated into \[{{H}_{2}}\] and \[{{I}_{2}}\] at equilibrium. The equilibrium constant is:
  A)
  1.0                    done clear
  B)
  3.0     done clear
  C)
  0.5                    done clear
  D)
  0.25 done clear
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• question_answer18)
  Some inert gas is added at constant volume to the following reaction at equilibrium \[N{{H}_{4}}HS(s)\rightleftharpoons N{{H}_{3}}(g)+{{H}_{2}}S(g)\] Predict the effect of adding the inert gas:
  A)
  The equilibrium shifts in the forward direction done clear
  B)
  The equilibrium shifts in the backward direction done clear
  C)
  The equilibrium remains unaffected done clear
  D)
  The value of \[{{K}_{p}}\]is increased done clear
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• question_answer19)
  The standard state Gibb's free energy change for the isomerisation reaction \[cis-2-pentene\rightleftharpoons trans-2-pentene\]is \[-3.67\text{ }kJ\text{ }mo{{l}^{-1}}\] at 400 K. If more trans-2-pentene is added to the reaction vessel
  A)
  more cis-2-pentene is formed done clear
  B)
  equilibrium shifts in the forward direction done clear
  C)
  equilibrium remains unaltered done clear
  D)
  more trans-2-pentene is produced done clear
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• question_answer20)

  (1) \[{{N}_{2}}(g)+3{{H}_{2}}(g)\rightleftharpoons 2N{{H}_{3}}(g),{{K}_{1}}\]

  (2) \[{{N}_{2}}(g)+{{O}_{2}}(g)\rightleftharpoons 2NO(g),{{K}_{2}}\]

  (3) \[{{H}_{2}}(g)+\frac{1}{2}{{O}_{2}}(g)\rightleftharpoons {{H}_{2}}O(g),{{K}_{3}}\]

  The equation for the equilibrium constant of the reaction

  \[2N{{H}_{3}}(g)+\frac{5}{2}{{O}_{2}}(g)\rightleftharpoons 2NO(g)+3{{H}_{2}}O(g),\]

  \[({{K}_{4}})\] in terms of \[{{K}_{1}},{{K}_{2}}\] and\[~{{K}_{3}}\] is:

  A)
  \[\frac{{{K}_{1}}.{{K}_{2}}}{{{K}_{3}}}\] done clear
  B)
  \[\frac{{{K}_{1}}.K_{3}^{2}}{{{K}_{2}}}\] done clear
  C)
  \[{{K}_{1}}{{K}_{2}}{{K}_{3}}\]                    done clear
  D)
  \[\frac{{{K}_{2}}.K_{3}^{3}}{{{K}_{1}}}\] done clear
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• question_answer21)
  On the basis of Le-Chatelier's principle, predict which of the following conditions would be unfavourable for the formation of 803? Given that \[2S{{O}_{2}}+O\rightleftharpoons 2S{{O}_{3}};\Delta H=-42kcal\]
  A)
  Low pressure and low temperature done clear
  B)
  High pressure and low temperature done clear
  C)
  High temperature and low pressure done clear
  D)
  High concentration of \[S{{O}_{2}}\] done clear
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• question_answer22)
  The reaction, \[S{{O}_{2}}+C{{l}_{2}}\xrightarrow{{}}S{{O}_{2}}C{{l}_{2}}\] is exothermic and reversible. A mixture of\[SO{{  }_{2}}(g)\], \[C{{l}_{2}}(g)\] and \[S{{O}_{2}}C{{l}_{2}}(l)\] is at equilibrium in a closed container. Now a certain quantity of extra \[S{{O}_{2}}\]is introduced into the container, the volume remaining the same. Which of the following is/ are true?
  A)
  The pressure inside the container will not change. done clear
  B)
  The temperature will not change. done clear
  C)
  The temperature will increase. done clear
  D)
  The temperature will decrease. done clear
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• question_answer23)
  In reaction \[A+2B\rightleftharpoons 2C+D\], initial concentration of B was 1.5 times of [A], but at equilibrium the concentrations of A and B became equal. The equilibrium constant for the reaction is:
  A)
  8                      done clear
  B)
  4 done clear
  C)
  12                     done clear
  D)
  6 done clear
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• question_answer24)
  For the reaction: \[2Ba{{O}_{2}}(s)\rightleftharpoons 2BaO(s)+{{O}_{2}}(g);\] \[\Delta H=+ve.\] In equilibrium condition, pressure of \[{{O}_{2}}\] is dependent on
  A)
  mass of \[Ba{{O}_{2}}\] done clear
  B)
  mass of \[BaO\] done clear
  C)
  temperature of equilibrium done clear
  D)
  mass of \[Ba{{O}_{2}}\] and \[BaO\]both done clear
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• question_answer25)
  For the reaction \[N{{H}_{4}}HS(g)\rightleftharpoons N{{H}_{3}}(g)+{{H}_{2}}S(g)\] in a closed flask, the equilibrium pressure is P atm. The standard free energy of the reaction would be:
  A)
  \[-RT\] ln p         done clear
  B)
  \[-RT\] (ln p - ln 2) done clear
  C)
  \[-2RT\] ln p                    done clear
  D)
  \[-2RT\] (ln p - ln 2) done clear
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• question_answer26)
  For the reaction \[{{H}_{2}}(g)+{{I}_{2}}(g)\rightleftharpoons 2HI(g)\] at 721 K, the value of equilibrium constant is 50, when equilibrium concentration of both is 5M. Value of \[{{K}_{p}}\] under the same conditions will be
  A)
  0.02                  done clear
  B)
  0.2    done clear
  C)
  50                                 done clear
  D)
  50 RT done clear
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• question_answer27)
  For a reversible gaseous reaction \[{{N}_{2}}+3{{H}_{2}}\rightleftharpoons 2N{{H}_{3}}\] at equilibrium, if some moles of \[{{H}_{2}}\] are replaced by same number of moles of \[{{T}_{2}}\](T is tritium, isotope of H and assume isotopes do not have different chemical properties) without affecting other parameter, then:
  A)
  the sample of ammonia obtained after sometime will be radioactive. done clear
  B)
  moles of \[{{N}_{2}}\] after the change will be different as compared to moles of \[{{N}_{2}}\] present before the change done clear
  C)
  the value of \[{{K}_{p}}\] or \[{{K}_{c}}\]will change done clear
  D)
  the average molecular mass of new equilibrium will be same as that of old equilibrium done clear
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• question_answer28)
  The ratio\[\frac{{{K}_{p}}}{{{K}_{c}}}\] for the reaction \[CO(g)+\frac{1}{2}{{O}_{2}}(g)\rightleftharpoons C{{O}_{2}}(g)\]is:
  A)
  \[\frac{1}{\sqrt{RT}}\]                done clear
  B)
  \[{{(RT)}^{1/2}}\] done clear
  C)
  RT                                done clear
  D)
  1 done clear
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• question_answer29)
  Which of the following is true at chemical equilibrium?
  A)
  \[{{(\Delta G)}_{T,P}}\] is minimum and \[{{(\Delta S)}_{U,V}}\] is also minimum done clear
  B)
  \[{{(\Delta G)}_{T,V}}\]is minimum and \[{{(\Delta S)}_{U,V}}\] is maximum done clear
  C)
  \[{{(\Delta G)}_{T,V}}\] is maximum and \[{{(\Delta S)}_{U,V}}\]is zero done clear
  D)
  \[{{(\Delta G)}_{T,P}}\] is zero and \[{{(\Delta S)}_{U,V}}\] is also zero done clear
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• question_answer30)
  \[{{K}_{1}},{{K}_{2}}\] and \[{{K}_{3}}\] are the equilibrium constants of the following reactions (I), (II) and (III) respectively:

  (I) \[{{N}_{2}}+2{{O}_{2}}\rightleftharpoons 2N{{O}_{2}}\]

  (II) \[2N{{O}_{2}}\rightleftharpoons {{N}_{2}}+2{{O}_{2}}\]

  (III) \[N{{O}_{2}}\rightleftharpoons \frac{1}{2}{{N}_{2}}+{{O}_{2}}\]

  The correct relation from the following is

  A)
  \[{{K}_{1}}=\frac{1}{{{K}_{2}}}=\frac{1}{{{K}_{3}}}\]         done clear
  B)
  \[{{K}_{1}}=\frac{1}{{{K}_{2}}}=\frac{1}{{{({{K}_{3}})}^{2}}}\] done clear
  C)
  \[{{K}_{1}}=\sqrt{{{K}_{2}}}={{K}_{3}}\]     done clear
  D)
  \[{{K}_{1}}=\frac{1}{{{K}_{2}}}={{K}_{3}}\] done clear
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• question_answer31)
  lf \[{{K}_{sp}}\]of \[Ca{{F}_{2}}\] at \[25{}^\circ C\] is\[1.7\times {{10}^{-10}}\], the combination amongst the following which gives a precipitate of \[Ca{{F}_{2}}\] is   
  A)
  \[1\times {{10}^{-2}}MC{{a}^{2+}}\] and \[1\times {{10}^{-3}}M{{F}^{-}}\] done clear
  B)
  \[1\times {{10}^{-4}}MC{{a}^{2+}}\] and \[1\times {{10}^{-4}}M{{F}^{-}}\] done clear
  C)
  \[1\times {{10}^{-2}}MC{{a}^{2+}}\] and \[1\times {{10}^{-5}}M{{F}^{-}}\] done clear
  D)
  \[1\times {{10}^{-3}}MC{{a}^{2+}}\] and \[1\times {{10}^{-5}}M{{F}^{-}}\] done clear
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• question_answer32)
  The solubility of \[Pb{{I}_{2}}\] at \[25{}^\circ C\] is\[0.7\text{ }g\text{ }{{L}^{-1}}\]. The solubility product of \[Pb{{I}_{2}}\] at this temperature is (molar mass of\[Pb{{I}_{2}}=461.2gmo{{l}^{-1}}\])
  A)
  \[1.40\times {{10}^{-9}}\]         done clear
  B)
  \[0.14\times {{10}^{-9}}\] done clear
  C)
  \[140\times {{10}^{-9}}\]          done clear
  D)
  \[14.0\times {{10}^{-9}}\] done clear
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• question_answer33)
  Consider the expression \[\Delta G=-\,RT\,\ln {{K}_{p}}+RT\,\ln {{Q}_{p}}\]  and indicate the correct statement at equilibrium
  A)
  \[\Delta G=0,\text{ }{{Q}_{p}}>{{K}_{p}}\] the equilibrium reaction will shift from left to right done clear
  B)
  \[\Delta G=0,\text{ }{{Q}_{p}}={{K}_{p}}\] the equilibrium reaction will shift from left to right done clear
  C)
  \[\Delta G=\infty ,\text{ }{{Q}_{p}}<{{K}_{p}}\] the equilibrium reaction will shift from right to left done clear
  D)
  \[\Delta G<0,\text{ }{{Q}_{p}}>{{K}_{p}}\] the equilibrium reaction will shift from right to left where \[{{Q}_{p}}\] and \[{{K}_{p}}\] term refer to reaction quotient and equilibrium constant at constant pressure respectively. done clear
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• question_answer34)
  If the synthesis of ammonia from Haber's process is carried out with exactly the same starting conditions (of partial pressure and temperature) but using \[{{D}_{\text{2}}}\](deuterium) in place of\[{{H}_{2}}\]. Then
  A)
  the equilibrium will be disturbed done clear
  B)
  the composition of reaction mixture will remain same at equilibrium. done clear
  C)
  Use of isotope in reaction will not produce ammonia. done clear
  D)
  At equilibrium rate of forward reaction will be greater than the rate of reverse reaction done clear
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• question_answer35)
  A solution of \[0.1\text{ }M\text{ }NaZ\] has \[pH=8.90.\]The \[{{K}_{a}}\] of HZ is
  A)
  \[6.3\times {{10}^{-11}}\]        done clear
  B)
  \[6.3\times {{10}^{-10}}\] done clear
  C)
  \[1.6\times {{10}^{-5}}\]          done clear
  D)
  \[1.6\times {{10}^{-6}}\] done clear
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• question_answer36)
  The following equilibrium is established when hydrogen chloride is dissolved in acetic acid. \[HCl+C{{H}_{3}}COOH\rightleftharpoons C{{l}^{-}}+C{{H}_{3}}COOH_{2}^{+}\] The set that characterises the conjugate acid- base pairs is
  A)
  \[(HCl,C{{H}_{3}}COOH)and(C{{H}_{3}}COOH_{2}^{+},C{{l}^{-}})\] done clear
  B)
  \[(HCl,C{{H}_{3}}COOH_{2}^{+})and(C{{H}_{3}}COOH,C{{l}^{-}})\] done clear
  C)
  \[(C{{H}_{3}}COOH_{2}^{+},HCl)and(C{{l}^{-}},C{{H}_{3}}COOH)\] done clear
  D)
  \[(HCl,C{{l}^{-}})and(C{{H}_{3}}COOH_{2}^{+},C{{H}_{3}}COOH)\] done clear
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• question_answer37)
  A solution contains 10 mL 0.1 N \[NaOH\] and 10 mL 0.05 N \[{{H}_{2}}S{{O}_{4}}\], pH of this solution is:
  A)
  less than 7        done clear
  B)
  7 done clear
  C)
  zero                               done clear
  D)
  greater than 7 done clear
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• question_answer38)
  8 mol of \[A{{B}_{3}}(g)\]are introduced into a \[1.0\text{ }d{{m}^{3}}\]vessel. If it dissociates as \[2A{{B}_{3}}(g)\rightleftharpoons {{A}_{2}}(g)+3{{B}_{2}}(g)\]. At equilibrium, 2 mol of \[{{A}_{2}}\] are found to be present. The equilibrium. constant of this reaction is
  A)
  2                      done clear
  B)
  3      done clear
  C)
  27                     done clear
  D)
  36 done clear
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• question_answer39)
  Assuming that the degree of hydrolysis is small, the pH of 0.1 M solution of sodium acetate \[({{K}_{a}}=1.0\times {{10}^{-5}})\] will be:
  A)
  5.0                    done clear
  B)
  6.0     done clear
  C)
  8.0                    done clear
  D)
  9.0 done clear
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• question_answer40)
  The hydrogen ion concentration of 0.2 N \[C{{H}_{3}}COOH\] which is 40% dissociated is
  A)
  0.08 N               done clear
  B)
  0.12 N done clear
  C)
  0.80 N               done clear
  D)
  1.2N done clear
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• question_answer41)
  Which one of the following is the correct statement?
  A)
  \[HC{{O}_{3}}^{-}\] is the conjugate base of\[C{{O}_{3}}^{2-}\]. done clear
  B)
  \[N{{H}_{2}}^{-}\]is the conjugate acid of \[N{{H}_{3}}\]. done clear
  C)
  \[{{H}_{2}}S{{O}_{4}}\] is the conjugate acid of\[HS{{O}_{4}}^{-}\]. done clear
  D)
  \[N{{H}_{3}}\]is the conjugate base of\[N{{H}_{2}}^{-}\]. done clear
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• question_answer42)
  Which equilibrium can be described as an acid- base reaction using the Lewis acid-base definition but not using the Bronsted-Lowry definition?
  A)
  \[2N{{H}_{3}}+{{H}_{2}}S{{O}_{4}}\rightleftharpoons 2N{{H}_{4}}^{+}+S{{O}_{4}}^{2-}\] done clear
  B)
  \[N{{H}_{3}}+C{{H}_{3}}COOH\rightleftharpoons N{{H}_{4}}^{+}+C{{H}_{3}}CO{{O}^{-}}\] done clear
  C)
  \[{{H}_{2}}O+C{{H}_{3}}COOH\rightleftharpoons {{H}_{3}}{{O}^{+}}+C{{H}_{3}}CO{{O}^{-}}\] done clear
  D)
  \[{{[Cu{{({{H}_{2}}O)}_{4}}]}^{2+}}+4N{{H}_{3}}\rightleftharpoons {{[Cu{{(N{{H}_{3}})}_{4}}]}^{2+}}+4{{H}_{2}}O\] done clear
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• question_answer43)
  At a certain temperature the dissociation constants of formic acid and acetic acid are \[1.8\times {{10}^{-4}}\] and \[1.8\times {{10}^{-6}}\] respectively. The concentration of acetic acid solution in which the hydrogen ion has the same concentration as in 0.001 M formic acid solution is equal to
  A)
  0.001 M           done clear
  B)
  0.01 M done clear
  C)
  0.1M                             done clear
  D)
  0.0001 M done clear
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• question_answer44)
  One mole of \[{{O}_{2}}(g)\] and two moles of \[S{{O}_{2}}(g)\] were heated in a closed vessel of one-litre capacity at 1098 K. At equilibrium 1.6 moles of \[S{{O}_{3}}\left( g \right)\] were found. The equilibrium constant \[{{K}_{c}}\] of the reaction would be         
  A)
  30                     done clear
  B)
  40     done clear
  C)
  80                                 done clear
  D)
  60 done clear
  View Solution play_arrow

• question_answer45)
  The increase of pressure on ice \[\rightleftharpoons \] water system at constant temperature will lead to
  A)
  a decrease in the entropy of the system done clear
  B)
  an increase in the Gibb's energy of the system done clear
  C)
  no effect on the equilibrium done clear
  D)
  a shift of the equilibrium in the forward direction done clear
  View Solution play_arrow

• question_answer46)
  What is the decreasing order of basic strengths of \[O{{H}^{-}},N{{H}_{2}}^{-},H-C\equiv {{C}^{-}}\] and \[C{{H}_{3}}-C{{H}_{2}}^{-}\]
  A)
  \[C{{H}_{3}}-CH_{2}^{-}>NH_{2}^{-}>H-C\equiv {{C}^{-}}>O{{H}^{-}}\] done clear
  B)
  \[H-C\equiv {{C}^{-}}>C{{H}_{3}}C{{H}_{2}}^{-}>NH_{2}^{-}>O{{H}^{-}}\] done clear
  C)
  \[O{{H}^{-}}>N{{H}_{2}}^{-}>H-C\equiv {{C}^{-}}>C{{H}_{3}}-CH_{2}^{-}\] done clear
  D)
  \[N{{H}_{2}}^{-}>H-C\equiv {{C}^{-}}>O{{H}^{-}}>C{{H}_{3}}-CH_{2}^{-}\] done clear
  View Solution play_arrow

• question_answer47)
  When \[C{{O}_{2}}\] dissolves in water, the following equilibrium is established \[C{{O}_{2}}+2{{H}_{2}}O\rightleftharpoons {{H}_{3}}{{O}^{+}}+HC{{O}_{3}}^{-}\] for which the equilibrium constant is \[3.8\times {{10}^{-7}}\] and pH = 6.0. The ratio of \[\left[ HC{{O}_{3}}^{-} \right]\] to \[[C{{O}_{2}}]\] would be
  A)
  \[3.8\times {{10}^{-13}}\]        done clear
  B)
  \[3.8\times {{10}^{-1}}\] done clear
  C)
   6.0                               done clear
  D)
  13.4 done clear
  View Solution play_arrow

• question_answer48)
  The first and second dissociation constants of an acid \[{{H}_{2}}A\] are \[1.0\times {{10}^{-5}}\] and \[5.0\times {{10}^{-10}}\] respectively. The overall dissociation constant of the acid will be
  A)
  \[0.2\times {{10}^{5}}\]           done clear
  B)
  \[5.0\times {{10}^{-5}}\] done clear
  C)
  \[5.0\times {{10}^{15}}\]          done clear
  D)
  \[5.0\times {{10}^{-15}}\] done clear
  View Solution play_arrow

• question_answer49)
  Values of dissociation constant, \[{{K}_{a}}\] are given as follows:

  Acid	\[{{K}_{a}}\]
  HCN	\[6.2\times {{10}^{-10}}\]
  HF	\[7.2\times {{10}^{-4}}\]
  HNCX	\[4.0\times {{10}^{-4}}\]

  Correct order of increasing base strength of the base \[C{{N}^{-}}\text{, }{{F}^{-}}\]and \[NO_{2}^{-}\] will be:
  A)
  \[{{F}^{-}}<C{{N}^{-}}<NO_{_{2}}^{-}\] done clear
  B)
  \[NO_{_{2}}^{-}<C{{N}^{-}}<{{F}^{-}}\] done clear
  C)
  \[{{F}^{-}}<NO_{2}^{-}<C{{N}^{-}}\] done clear
  D)
  \[NO_{2}^{-}<{{F}^{-}}<C{{N}^{-}}\] done clear
  View Solution play_arrow

• question_answer50)
  Given

  (i) \[HCN(aq)+{{H}_{2}}O(l)\rightleftharpoons \]

  \[{{H}_{3}}{{O}^{+}}(aq)+C{{N}^{-}}(aq){{K}_{a}}=6.2\times {{10}^{-10}}\]

  (ii) \[C{{N}^{-}}(aq)+{{H}_{2}}O(l)\rightleftharpoons \]

  \[HCN(aq)+O{{H}^{-}}(aq){{K}_{b}}=1.6\times {{10}^{-5}}.\]

  These equilibria show the following order of the relative base strength,

  A)
  \[O{{H}^{-}}>{{H}_{2}}O>C{{N}^{-}}\] done clear
  B)
  \[O{{H}^{-}}>C{{N}^{-}}>{{H}_{2}}O\] done clear
  C)
  \[{{H}_{2}}O>C{{N}^{-}}>O{{H}^{-}}\]     done clear
  D)
  \[C{{N}^{-}}>{{H}_{2}}O>O{{H}^{-}}\] done clear
  View Solution play_arrow

• question_answer51)
  Which of the following statements about pH and \[{{H}^{+}}\] ion concentration is incorrect?
  A)
  Addition of one drop of concentrated \[HCl\] in \[N{{H}_{4}}OH\] solution decreases pH of the solution. done clear
  B)
  A solution of the mixture of one equivalent of each of \[C{{H}_{3}}COOH\] and \[NaOH\] has a pH of 7 done clear
  C)
  pH of pure neutral water is not zero done clear
  D)
  A cold and concentrated \[{{H}_{2}}S{{O}_{4}}\] has lower \[{{H}^{+}}\] ion concentration than a dilute solution of\[{{H}_{2}}S{{O}_{4}}\] done clear
  View Solution play_arrow

• question_answer52)
  Assuming that the buffer in the blood is \[C{{O}_{2}}-HCO_{3}^{-}\]. Calculate the ratio of conjugate base to acid necessary to maintain blood at its proper pH of 7.4. \[{{K}_{1}}({{H}_{2}}CO{{  }_{3}})=4.5\times {{10}^{-7}}\]
  A)
  11                     done clear
  B)
  8      done clear
  C)
  6                                  done clear
  D)
  14 done clear
  View Solution play_arrow

• question_answer53)
  If the reaction between \[C{{O}_{2}}\] and \[{{H}_{2}}O\]is  \[C{{O}_{2}}+{{H}_{2}}O\rightleftharpoons {{H}_{2}}C{{O}_{3}}\rightleftharpoons {{H}^{+}}+HCO_{3}^{-}\] If \[C{{O}_{2}}\] escapes from the system
  A)
  pH will decrease done clear
  B)
  \[{{H}^{+}}\] concentration will decrease done clear
  C)
  \[{{H}_{2}}C{{O}_{3}}\] concentration will be altered done clear
  D)
  The forward reaction is promoted done clear
  View Solution play_arrow

• question_answer54)
  Calculate the pH of a solution containing 0.1 M

  \[HCO_{3}^{-}\] and \[0.2\,M\,CO_{3}^{2-}\]

  \[[{{K}_{1}}({{H}_{2}}CO_{3}^{-})=4.2\times {{10}^{-7}}\times 10\]and

  \[{{K}_{2}}(HCO_{3}^{-})=4.8\times {{10}^{-11}}].\]

  A)
  3.18                  done clear
  B)
  10.62 done clear
  C)
  6.62                  done clear
  D)
  9.31 done clear
  View Solution play_arrow

• question_answer55)
  What is the pH of a \[{{10}^{-4}}M\,O{{H}^{-}}\] solution at 330K, if \[{{K}_{w}}\] at 330K is \[{{10}^{-13.6}}\]?
  A)
  4                      done clear
  B)
  9.0    done clear
  C)
  10                     done clear
  D)
  9.6 done clear
  View Solution play_arrow

• question_answer56)
  What happens when an inert gas is added to an equilibrium keeping volume unchanged?
  A)
  More product will form done clear
  B)
  Less product will form done clear
  C)
  More reactant will form done clear
  D)
  Equilibrium will remain unchanged done clear
  View Solution play_arrow

• question_answer57)
  The degree of dissociation of 0.1 M weak acid HA is 0.5%. If 2 mL of 1.0 M HA solution is diluted to 32 mL the degree of dissociation of acid and \[{{H}_{3}}{{O}^{+}}\] ion concentration in the resulting solution will be respectively
  A)
  0.02 and \[3.125\times {{10}^{-4}}\] done clear
  B)
  \[1.25\times {{10}^{-3}}\] and 0.02 done clear
  C)
  0.02 and \[1.25\times {{10}^{-3}}\] done clear
  D)
  0.02 and \[8.0\times {{10}^{-12}}\] done clear
  View Solution play_arrow

• question_answer58)
  20 mL of 0.2 M \[NaOH\] are added to 50 mL of 0.2 M \[C{{H}_{2}}COOH\]\[({{K}_{a}}=1.8\times 10{{~}^{-5}})\] the pH of the solution is
  A)
  4.56                  done clear
  B)
  4.73   done clear
  C)
  9.45                  done clear
  D)
  6.78 done clear
  View Solution play_arrow

• question_answer59)
  Why only \[A{{s}^{3+}}\] gets precipitated as \[A{{s}_{2}}{{S}_{3}}\] and not \[Z{{n}^{2+}}\]as ZnS when \[{{H}_{2}}S\] is passed through an acidic solution containing \[A{{s}^{3+}}\] and\[Z{{n}^{2+}}\]?
  A)
  Solubility product of \[A{{s}_{2}}{{S}_{3}}\] is less than that of ZnS done clear
  B)
  Enough \[A{{s}^{3+}}\]are present in acidic medium done clear
  C)
  Zinc salt does not ionise in acidic medium done clear
  D)
  Solubility product changes in presence of an acid done clear
  View Solution play_arrow

• question_answer60)
  The conjugate base of hydrazoic acid is:
  A)
  \[{{N}^{-3}}\]                         done clear
  B)
  \[N_{3}^{-}\]   done clear
  C)
  \[N_{2}^{-}\]                           done clear
  D)
  \[HN_{3}^{-}\] done clear
  View Solution play_arrow

• question_answer61)
  \[NaOH\] is a strong base. What will be pH of \[5.0\times {{10}^{-2}}M\,NaOH\] solution? \[\left( log2=0.3 \right)\]
  A)
  14.00                done clear
  B)
  13.70 done clear
  C)
  13.00                done clear
  D)
  12.70 done clear
  View Solution play_arrow

• question_answer62)
  The solubility product of \[A{{g}_{2}}Cr{{O}_{4}}\] is \[32\times {{10}^{-12}}\]. What is the concentration of \[CrO_{4}^{2-}\] ions in that solution (in g\[{{L}^{-1}}\])
  A)
  \[2\times {{10}^{-4}}\]                         done clear
  B)
  \[8\times {{10}^{-4}}\] done clear
  C)
  \[8\times {{10}^{-8}}\]                         done clear
  D)
  \[16\times {{10}^{-4}}\] done clear
  View Solution play_arrow

• question_answer63)
  What is the minimum concentration of \[S{{O}_{4}}^{2-}\]required to precipitate \[BaS{{O}_{4}}\] in a solution containing \[1.0\times {{10}^{-4}}\] mole of\[B{{a}^{2+}}\]? \[{{K}_{sp}}\] for \[BaS{{O}_{4}}=4\times {{10}^{-10}}\]
  A)
  \[4\times {{10}^{-10}}M\]         done clear
  B)
  \[2\times {{10}^{-7}}M\] done clear
  C)
  \[4\times {{10}^{-6}}M\]          done clear
  D)
  \[2\times {{10}^{-3}}M\] done clear
  View Solution play_arrow

• question_answer64)
  Equimolar solutions of the following compounds are prepared separately in water. Which will have the lowest pH value?
  A)
  \[BeC{{l}_{2}}\]                       done clear
  B)
  \[SrC{{l}_{2}}\] done clear
  C)
  \[CaC{{l}_{2}}\]                       done clear
  D)
  \[MgC{{l}_{2}}\] done clear
  View Solution play_arrow

• question_answer65)
  Addition of which chemical will decrease the hydrogen ion concentration of an acetic acid solution
  A)
  \[N{{H}_{4}}Cl\]                      done clear
  B)
  \[A{{l}_{2}}{{\left( S{{O}_{4}} \right)}_{3}}\] done clear
  C)
  \[AgN{{O}_{3}}\]                      done clear
  D)
  \[NaCN\] done clear
  View Solution play_arrow

• question_answer66)
  What is the percentage hydrolysis of NaCN in N/80 solution when the dissociation constant for \[HCN\] is \[1.3\times {{10}^{-9}}\]and \[{{K}_{w}}=1.0\times {{10}^{-14}}\]
  A)
  2.48                  done clear
  B)
  5.26  done clear
  C)
  8.2                    done clear
  D)
  9.6 done clear
  View Solution play_arrow

• question_answer67)
  The dissociation constant of 0.1 M acetic acid solution is\[1.8\times {{10}^{-5}}\]. If 1 L of this solution is mixed with 0.05 mole of\[HCl\], what will be pH of mixture? \[\left[ log5=0.7 \right]\]
  A)
  1.3                    done clear
  B)
  2.6    done clear
  C)
  1.9                    done clear
  D)
  3.4 done clear
  View Solution play_arrow

• question_answer68)
  For preparing a buffer solution of pH 6 by mixing sodium acetate and acetic acid, the ratio of the concentration of salt and acid should be \[({{K}_{a}}={{10}^{-5}})\]
  A)
  1:10                  done clear
  B)
  10:1 done clear
  C)
  100:1                done clear
  D)
  1:100 done clear
  View Solution play_arrow

• question_answer69)
  In a saturated solution of the sparingly soluble strong electrolyte \[AgI{{O}_{3}}\](molecular mass = 283) the equilibrium which sets is \[AgI{{O}_{3}}(s)\rightleftharpoons A{{g}^{+}}(aq)+IO_{3}^{-}(aq).\] If the solubility product constant \[{{K}_{sp}}\] of \[AgI{{O}_{3}}\] at a given temperature is \[1.0\times {{10}^{-8}}\], what is the mass of \[AgI{{O}_{3}}\] contained in 100 mL of its saturated solution?
  A)
  \[1.0\times {{10}^{-4}}\]g     done clear
  B)
  \[28.3\times {{10}^{-2}}g\] done clear
  C)
  \[2.83\times {{10}^{-3}}g\]       done clear
  D)
  \[1.0\times {{10}^{-7}}g.\] done clear
  View Solution play_arrow

• question_answer70)
  At \[25{}^\circ C\], the dissociation constant of a base, BOH, is \[1.0\times {{10}^{-12}}\]. The concentration of hydroxyl ions in 0.01 M aqueous solution of the base would be
  A)
  \[1.0\times {{10}^{-5}}mol\,{{L}^{-1}}\]         done clear
  B)
  \[1.0\times {{10}^{-6}}mol\,{{L}^{-1}}\] done clear
  C)
  \[2.0\times {{10}^{-6}}mol\text{ }{{L}^{-1}}\] done clear
  D)
  \[1.0\times {{10}^{-7}}mol\text{ }{{L}^{-1}}\] done clear
  View Solution play_arrow

• question_answer71)
  What would be the pH of a solution obtained by mixing 5g of acetic acid and 7.5g of sodium acetate and making the volume equal to 500 mL? \[({{K}_{a}}=1.75\times {{10}^{-5}},p{{K}_{a}}=4.76)\]
  A)
  \[pH=4.70\] done clear
  B)
  pH < 4.70 done clear
  C)
  pH of solution will be equal to pH of acetic acid done clear
  D)
  4.76 < pH < 5.0 done clear
  View Solution play_arrow

• question_answer72)
  In some solutions, the concentration of \[{{H}_{2}}{{O}^{+}}\]remains constant even when small amounts of strong acid or strong base are added to them. These solutions are known as:
  A)
  Ideal solutions    done clear
  B)
  Colloidal solutions done clear
  C)
  True solutions    done clear
  D)
  Buffer solutions done clear
  View Solution play_arrow

• question_answer73)
  If degree of dissociation of pure water at\[100{}^\circ C\] is\[1.8\times {{10}^{-8}}\], then the dissociation constant of water will be (density of\[{{H}_{2}}O=1g/cc\])
  A)
  \[1\times {{10}^{-12}}\]           done clear
  B)
  \[1\times {{10}^{-14}}\] done clear
  C)
  \[1.8\times {{10}^{-12}}\]         done clear
  D)
  \[1.8\times {{10}^{-14}}\] done clear
  View Solution play_arrow

• question_answer74)
  The dissociation constant of two acids \[H{{A}_{1}}\] and \[H{{A}_{2}}\] are \[3.14\times {{10}^{-4}}\] and \[1.96\times {{10}^{-5}}\]respectively The relative strength of the acids will be approximately
  A)
  1:4                                done clear
  B)
  4:1   done clear
  C)
  1:16                              done clear
  D)
  16:1 done clear
  View Solution play_arrow

• question_answer75)
  At 298K a 0.1 M \[C{{H}_{2}}COOH\]solution is 1.34 % ionized. The ionization constant \[{{K}_{a}}\]for acetic acid will be
  A)
  \[1.82\times {{10}^{-5}}\]         done clear
  B)
  \[18.2\times {{10}^{-5}}\] done clear
  C)
  \[0.182\times {{10}^{-5}}\]      done clear
  D)
  None of these done clear
  View Solution play_arrow

• question_answer76)
  A buffer solution is prepared by mixing 10 mL of  \[1.0M\,C{{H}_{3}}COOH\] and 20 mL of 0.5 M \[C{{H}_{3}}COONa\] and then diluted to 100 mL with distilled water. If \[p{{K}_{a}}\]of \[C{{H}_{3}}COOH\] is 4.76, what is the pH of the buffer solution?
  A)
  5.8                    done clear
  B)
  4.34   done clear
  C)
  5.21                  done clear
  D)
  4.76 done clear
  View Solution play_arrow

• question_answer77)
  Which one of the following arrangements represents the correct order of the proton affinity of the given species:
  A)
  \[{{I}^{-}}<{{F}^{-}}<H{{S}^{-}}<NH_{2}^{-}\] done clear
  B)
  \[H{{S}^{-}}<NH_{2}^{-}<{{F}^{-}}<{{I}^{-}}\] done clear
  C)
  \[{{F}^{-}}<{{I}^{-}}<\text{ }NH_{2}^{-}<H{{S}^{-}}\] done clear
  D)
  \[NH_{2}^{-}<H{{S}^{-}}<{{I}^{-}}<{{F}^{-}}\] done clear
  View Solution play_arrow

• question_answer78)
  Consider the following equilibrium \[AgCl\downarrow +2N{{H}_{3}}\rightleftharpoons {{\left[ Ag{{(N{{H}_{3}})}_{2}} \right]}^{+}}+C{{l}^{-}}\] White precipitate of \[AgCl\] appears on adding which of the following?
  A)
  \[N{{H}_{3}}\]                         done clear
  B)
  aqueous \[NaCl\] done clear
  C)
  aqueous\[HN{{O}_{3}}\]   done clear
  D)
  aqueous \[N{{H}_{4}}Cl\] done clear
  View Solution play_arrow

• question_answer79)
  The degree of hydrolysis in hydrolytic equilibrium \[{{A}^{-}}~+{{H}_{2}}O\rightleftharpoons HA+O{{H}^{-}}\] at salt concentration of 0.001 M is : \[({{K}_{a}}=1\times {{10}^{-5}})\]
  A)
  \[1\times {{10}^{-3}}\]                         done clear
  B)
  \[1\times {{10}^{-4}}\] done clear
  C)
  \[5\times {{10}^{-4}}\]                         done clear
  D)
  \[1\times {{10}^{-6}}\] done clear
  View Solution play_arrow

• question_answer80)
  A litre of solution is saturated with\[AgCl\]. To this solution if \[1.0\times {{10}^{-4}}\] mole of solid \[NaCl\] is added, what will be the\[\left[ A{{g}^{+}} \right]\], assuming no volume change?
  A)
  More                 done clear
  B)
  Less done clear
  C)
  Equal                done clear
  D)
  Zero done clear
  View Solution play_arrow

• question_answer81)
  If the equilibrium constant of the reaction of weak acid HA with strong base is\[{{10}^{-7}}\], then pOH of the aqueous solution of \[0.1M\text{ }NaA\] is
  A)
  8                      done clear
  B)
  10 done clear
  C)
  4                                  done clear
  D)
  5 done clear
  View Solution play_arrow

• question_answer82)
  How many gms of \[Ca{{C}_{2}}{{O}_{4}}\] will dissolve in one litre of saturated solution. \[{{K}_{sp}}\] of \[Ca{{C}_{2}}{{O}_{4}}\] is \[2.5\times {{10}^{-19}}\,mo{{l}^{2}}li{{t}^{-2}}\]
  A)
  0.0064 g            done clear
  B)
  0.0128 g done clear
  C)
  0.0032 g            done clear
  D)
  None of these done clear
  View Solution play_arrow

• question_answer83)
  Zirconium phosphate \[[Z{{r}_{3}}{{\left( P{{O}_{4}} \right)}_{4}}]\] dissociates into three zirconium cations of charge + 4 and four phosphate anions of charge \[-3\]. If molar solubility of zirconium phosphate is denoted by S and its solubility product by K then which of the following relationship between S and  \[{{K}_{sp}}\] is correct?                    
  A)
  \[S=\{{{K}_{sp}}/{{(6912)}^{1/7}}\}\] done clear
  B)
  \[S={{\{{{K}_{sp}}/144\}}^{1/7}}\] done clear
  C)
  \[S={{\{{{K}_{sp}}/6912\}}^{1/7}}\]  done clear
  D)
  \[S={{\{{{K}_{sp}}/6912\}}^{7}}\] done clear
  View Solution play_arrow

• question_answer84)
  Solid \[Ba{{(N{{O}_{3}})}_{2}}\] is gradually dissolved in a  \[1.0\times {{10}^{-4}}M\,N{{a}_{2}}C{{O}_{3}}\] solution. At which concentration of \[B{{a}^{2+}}\] precipitate of \[BaC{{O}_{3}}\] begins to form? (\[{{K}_{sp}}\] for \[BaC{{O}_{3}}=5.1\times {{10}^{-9}}\])
  A)
  \[5.1\times {{10}^{-5}}M\]        done clear
  B)
  \[7.1\times {{10}^{-8}}M\] done clear
  C)
  \[4.1\times {{10}^{-5}}M\]        done clear
  D)
  \[8.1\times {{10}^{-7}}M\] done clear
  View Solution play_arrow

• question_answer85)
  A solution of \[N{{H}_{4}}Cl\] and \[N{{H}_{3}}\] has pH = 8.0. Which of the following hydroxides may be precipitated when this solution is mixed with equal volume of 0.2 M of metal ion.
  A)
  \[Ba{{\left( OH \right)}_{2}}\left( {{K}_{sp}}=1.1\times {{10}^{-4}} \right)\] done clear
  B)
  \[Mg{{\left( OH \right)}_{2}}\left( {{K}_{sp}}=3.5\times {{10}^{-4}} \right)\] done clear
  C)
  \[Fe{{(OH)}_{2}}\left( {{K}_{sp}}=8.1\times {{10}^{-16}} \right)\] done clear
  D)
  \[Ca{{\left( OH \right)}_{2}}\left( {{K}_{sp}}=2.1\times {{10}^{-5}} \right).\] done clear
  View Solution play_arrow

• question_answer86)
  On addition of increasing amount of \[AgN{{O}_{3}}\] to 0.1 M each of \[NaCl\] and \[NaBr\] in a solution, what % of \[B{{r}^{-}}\] ion get precipitated when \[C{{l}^{-}}\]ion starts precipitating.\[{{K}_{sp}}\left( AgCl \right)=1.0\times {{10}^{-10}}\], \[{{K}_{sp}}(AgBr)=1\times {{10}^{-13}}\]
  A)
  0.11                  done clear
  B)
  99.9  done clear
  C)
  0.01                  done clear
  D)
  9.99 done clear
  View Solution play_arrow

• question_answer87)
  The percentage hydrolysis of 0.15 M solution of ammonium acetate, \[{{K}_{a}}\] for \[C{{H}_{3}}COOH\]is \[1.8\times {{10}^{-5}}\] and \[{{K}_{b}}\] for \[N{{H}_{3}}\] is \[1.8\times {{10}^{-5}}\]
  A)
  0.55 done clear
  B)
  4.72  done clear
  C)
  9.38                  done clear
  D)
  5.56 done clear
  View Solution play_arrow

• question_answer88)
  Which one of the following arrangements represents the correct order of solubilities of sparingly soluble salts \[H{{g}_{2}}C{{l}_{2}},\,\,C{{r}_{2}}{{(S{{O}_{4}})}_{3}},\] \[BaS{{O}_{4}}\] and \[CrC{{l}_{3}}\] respectively?
  A)
  \[BaS{{O}_{4}}>H{{g}_{2}}C{{l}_{2}}>Cr{{(S{{O}_{4}})}_{3}}>CrC{{l}_{3}}\] done clear
  B)
  \[BaS{{O}_{4}}>H{{g}_{2}}C{{l}_{2}}>CrC{{l}_{3}}>C{{r}_{2}}{{(S{{O}_{4}})}_{3}}\] done clear
  C)
  \[BaS{{O}_{4}}>CrC{{l}_{3}}>H{{g}_{2}}C{{l}_{2}}>C{{r}_{2}}{{(S{{O}_{4}})}_{3}}\] done clear
  D)
  \[H{{g}_{2}}C{{l}_{2}}>BaS{{O}_{4}}>CrC{{l}_{3}}>C{{r}_{2}}{{(S{{O}_{4}})}_{3}}\] done clear
  View Solution play_arrow

• question_answer89)
  What will be the \[{{H}^{+}}\] ion concentration in a solution prepared by mixing 50 mL of 0.20 \[M\,\,NaCl\] 25mL of \[0.10M\,NaOH\] and 25mL of 0.30\[NHCl\]?
  A)
  0.5 M                done clear
  B)
  0.05 M done clear
  C)
  0.02M                           done clear
  D)
  0.10M done clear
  View Solution play_arrow

• question_answer90)
  The concentration of hydroxyl ion in a solution left after mixing 100mL of 0.1M \[MgC{{l}_{2}}\] and 100mL of 0.2M \[NaOH\] \[({{K}_{sp}} of \,Mg{{(OH)}_{2}}=1.2\times {{10}^{-11}})\] is
  A)
  \[2.8\times {{10}^{-4}}\]          done clear
  B)
  \[2.8\times {{10}^{-3}}\] done clear
  C)
  \[2.8\times {{10}^{-2}}\]          done clear
  D)
  \[2.8\times {{10}^{-5}}\] done clear
  View Solution play_arrow

• question_answer91)
  The 0.001M solution of \[Mg{{(N{{O}_{3}})}_{2}}\] is adjusted to pH 9, \[{{K}_{sp}}\] of \[Mg{{(OH)}_{2}}\] is \[8.9\times {{10}^{-12}}\]. At this pH
  A)
  \[Mg{{(OH)}_{2}}\] will be precipitated done clear
  B)
  \[Mg{{(OH)}_{2}}\] is not precipitated done clear
  C)
  \[Mg{{\left( OH \right)}_{3}}\] will be precipitated done clear
  D)
  \[Mg{{\left( OH \right)}_{3}}\] is not precipitated done clear
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• question_answer92)
  The solubility (in \[mol\text{ }{{L}^{-1}}\]) of \[AgCl\] \[({{K}_{sp}}=1.0\times {{10}^{-10}})\] in a 0.1 M \[KCl\] solution will be
  A)
  \[1.0\times {{10}^{-9}}\]          done clear
  B)
  \[1.0\times {{10}^{-10}}\] done clear
  C)
  \[1.0\times {{10}^{-5}}\]          done clear
  D)
  \[1.0\times {{10}^{-11}}\] done clear
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• question_answer93)
  A solution is saturated with respect to \[SrC{{O}_{2}}\] and \[Sr{{F}_{2}}\] The \[\left[ C{{O}_{3}}^{2-} \right]\] was found to be \[1.2\times {{10}^{-3}}M.\] The concentration of \[{{F}^{-}}\] in the solution would be Given\[{{K}_{sp}}\,of\,SrC{{O}_{3}}=7.0\times {{10}^{-10}}{{M}^{2}}\], \[{{K}_{sp}}\]of \[Sr{{F}_{2}}=7.9\times {{10}^{-10}}{{M}^{3}}\]
  A)
  \[1.3\times {{10}^{-3}}M\]        done clear
  B)
  \[2.6\times {{10}^{-2}}M\] done clear
  C)
  \[3.7\times {{10}^{-2}}M\]        done clear
  D)
  \[5.8\times {{10}^{-7}}M\] done clear
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• question_answer94)
  If \[p{{K}_{b}}\] for fluoride ion at \[25{}^\circ C\] is 10.83, the ionisation constant of hydrofluoric acid in water at this temperature is
  A)
  \[3.52\times {{10}^{-3}}\]         done clear
  B)
  \[6.75\times {{10}^{-4}}\] done clear
  C)
  \[5.38\times {{10}^{-2}}\]         done clear
  D)
  \[1.74\times {{10}^{-5}}\] done clear
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• question_answer95)
  If \[{{K}_{sp}}(PbS{{O}_{4}})=1.8\times {{10}^{-8}}\] and \[{{K}_{a}}(HSO_{4}^{-})=1.0\times {{10}^{-2}}\] the equilibrium constant for the reaction.  \[PbS{{O}_{4}}(s)+{{H}^{+}}(aq)\rightleftharpoons HSO_{4}^{-}(aq)+P{{b}^{2+}}(aq)\] is
  A)
  \[1.8\times {{10}^{-6}}\]         done clear
  B)
  \[1.8\times {{10}^{-10}}\] done clear
  C)
  \[2.8\times {{10}^{-10}}\]        done clear
  D)
  \[1.0\times {{10}^{-2}}\] done clear
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• question_answer96)
  The dissociation constants of a weak acid HA and weak base BOH are \[2\times {{10}^{-5}}\] and \[5\times {{10}^{-6}}\] respectively. The equilibrium constant for the neutralisation reaction of the two is
  A)
  \[1.0\times {{10}^{4}}\]           done clear
  B)
  \[1.0\times {{10}^{-4}}\] done clear
  C)
  \[1.0\times {{10}^{-10}}\]         done clear
  D)
  \[2.5\times {{10}^{-1}}\] done clear
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• question_answer97)
  Solid \[AgN{{O}_{3}}\] is slowly added to a solution containing each of 0.01M \[NaCl\] and 0.001 M \[NaBr.\] What will be the concentration of \[{{C}^{-}}\] ions in solution when \[AgBr\] will just start to precipitate? \[{{K}_{sp}}(AgBr)=3.6\times {{10}^{-13}},{{K}_{sp}}(AgCl)=1.8\times {{10}^{-10}}.\]
  A)
  \[1.8\times {{10}^{-7}}\]          done clear
  B)
  \[3.6\times {{10}^{-10}}\] done clear
  C)
  0.01                              done clear
  D)
  \[2\times {{10}^{-4}}\] done clear
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• question_answer98)
  What is the unit of \[{{K}_{p}}\] for the reaction? \[C{{S}_{2}}(g)+4{{H}_{2}}(g)\rightleftharpoons C{{H}_{4}}(g)+2{{H}_{2}}S(g)\]
  A)
  atm                   done clear
  B)
  \[at{{m}^{-2}}\] done clear
  C)
  \[at{{m}^{2}}\]                       done clear
  D)
  \[at{{m}^{-1}}\] done clear
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• question_answer99)
  In the dissociation of \[PC{{l}_{5}}\] as \[PC{{l}_{5}}(g)\rightleftharpoons PC{{l}_{3}}(g)+C{{l}_{2}}(g)\] if the degree of dissociation is a at equilibrium pressure P, then the equilibrium constant for the reaction is
  A)
  \[{{K}_{P}}=\frac{{{\alpha }^{2}}}{1+{{\alpha }^{2}}P}\]   done clear
  B)
  \[{{K}_{P}}=\frac{{{\alpha }^{2}}{{P}^{2}}}{1-{{\alpha }^{2}}}\] done clear
  C)
  \[{{K}_{P}}=\frac{{{P}^{2}}}{1-{{\alpha }^{2}}}\] done clear
  D)
  \[{{K}_{P}}=\frac{{{\alpha }^{2}}P}{1-{{\alpha }^{2}}}\] done clear
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• question_answer100)
  The equilibrium constant for a reaction is K, and the reaction quotient is Q. For a particular reaction mixture, the ratio \[\frac{K}{Q}\]. is 0.33. This means that:
  A)
  The reaction mixture will equilibrate to form more reactant species done clear
  B)
  the reaction mixture will equilibrate to form more product species done clear
  C)
  the equilibrium ratio of reactant to product concentrations will be 3 done clear
  D)
  the equilibrium ratio of reactant to product concentrations will be 0.33 done clear
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