question_answer 1)
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_answer 2)
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_answer 3)
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_answer 4)
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_answer 5)
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_answer 6)
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_answer 7)
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_answer 8)
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_answer 9)
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_answer 10)
\[{{K}_{c}}\] 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_answer 11)
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_answer 12)
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_answer 13)
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_answer 14)
\[28g\,{{N}_{2}}\] 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_answer 15)
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_answer 16)
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_answer 17)
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_answer 18)
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_answer 19)
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_answer 20)
(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_answer 21)
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_answer 22)
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_answer 23)
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_answer 24)
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_answer 25)
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_answer 26)
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_answer 27)
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_answer 28)
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_answer 29)
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_answer 30)
\[{{K}_{1}},{{K}_{2}}\] 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_answer 31)
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_answer 32)
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_answer 33)
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_answer 34)
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_answer 35)
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_answer 36)
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_answer 37)
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_answer 38)
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_answer 39)
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_answer 40)
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_answer 41)
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_answer 42)
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_answer 43)
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_answer 44)
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
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question_answer 45)
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
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question_answer 46)
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_answer 47)
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_answer 48)
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_answer 49)
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_answer 50)
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_answer 51)
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
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question_answer 52)
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_answer 53)
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_answer 54)
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_answer 55)
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_answer 56)
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_answer 57)
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_answer 58)
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_answer 59)
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_answer 60)
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_answer 61)
\[NaOH\] 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_answer 62)
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_answer 63)
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_answer 64)
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_answer 65)
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_answer 66)
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_answer 67)
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_answer 68)
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_answer 69)
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_answer 70)
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_answer 71)
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_answer 72)
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_answer 73)
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_answer 74)
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_answer 75)
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_answer 76)
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_answer 77)
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_answer 78)
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_answer 79)
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_answer 80)
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_answer 81)
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_answer 82)
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_answer 83)
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_answer 84)
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_answer 85)
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_answer 86)
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_answer 87)
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_answer 88)
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
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question_answer 89)
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_answer 90)
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_answer 91)
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
View Solution play_arrow
question_answer 92)
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
View Solution play_arrow
question_answer 93)
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
View Solution play_arrow
question_answer 94)
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
View Solution play_arrow
question_answer 95)
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
View Solution play_arrow
question_answer 96)
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_answer 97)
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_answer 98)
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_answer 99)
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_answer 100)
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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