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question_answer1)
The following equilibrium is established when \[HCl{{O}^{{}}}_{4}\]is dissolved in weak acid \[HF\]. \[HF+HCl{{O}_{4}}\rightleftharpoons Cl{{O}_{4}}^{-}+{{H}_{2}}{{F}^{+}}\] Which of the following is correct set of conjugate acid
A)
HF and \[HCl{{O}_{4}}\] done
clear
B)
HF and \[Cl{{O}_{4}}^{-}\] done
clear
C)
HF and \[{{H}_{2}}{{F}^{+}}\] done
clear
D)
\[HCl{{O}_{4}}\] and \[{{H}_{2}}{{F}^{+}}\] done
clear
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question_answer2)
Calculate pH of 0.002 N \[N{{H}_{4}}\]OH having 2% dissociation.
A)
7.6 done
clear
B)
8.6 done
clear
C)
9.6 done
clear
D)
10.6 done
clear
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question_answer3)
Four species are listed below:
(i) \[HC{{O}^{-}}_{3}\] |
(ii) \[{{H}_{3}}{{O}^{+}}\] |
(iii) \[HS{{O}^{-}}_{4}\] |
(iv) \[HS{{O}_{3}}F\] |
Which one of the following is the correct sequence of their acid strength? |
A)
iv <ii <iii <i done
clear
B)
ii <iii <i <iv done
clear
C)
i <iii <ii <iv done
clear
D)
iii <i <iv <ii done
clear
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question_answer4)
If \[p{{K}_{b}}\]A for fluoride ion at \[25{}^\circ C\]is 10.83, (he ionization constant of hydrofluoric acid in water at this temperature is
A)
\[1.74\times {{10}^{-5}}\] done
clear
B)
\[3.52\times {{10}^{-3}}\] done
clear
C)
\[6.75\times {{10}^{-4}}\] done
clear
D)
\[5.38\times {{10}^{-2}}\] done
clear
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question_answer5)
The pH of Ba \[{{(OH)}_{2}}\]solution is 13. The number millimoles of Ba\[{{(OH)}_{2}}\] present in 10 ml of solution would be
A)
1.00 done
clear
B)
0.50 done
clear
C)
10.00 done
clear
D)
15.00 done
clear
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question_answer6)
Equal volumes of three acid solutions of pH 3, 4 and 5 are mixed in a vessel. What will be the \[{{H}^{+}}\] ion concentration
A)
\[3.7\times {{10}^{-3}}M\] done
clear
B)
\[1.11\times {{10}^{-3}}M\] done
clear
C)
\[1.11\times {{10}^{-4}}M\] done
clear
D)
\[3.7\times {{10}^{-4}}M\] done
clear
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question_answer7)
The pH of a 0.01 M solution of a monobasic acid is four. Which one of the following statements about the acid is invorrect?
A)
When a little NaOH is added, it will form a buffer solution done
clear
B)
It is a weak acid done
clear
C)
Its sodium salt will be acidic done
clear
D)
Its sodium salt will be basic done
clear
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question_answer8)
pH for the solution of salt undergoing anionic hydrolysis (say \[C{{H}_{3}}COONa\]) is given by:
A)
\[pH=1/2\left[ p{{K}_{w}}+p{{K}_{a}}+\log C \right]\] done
clear
B)
\[pH=1/2\left[ p{{K}_{w}}+p{{K}_{a}}-\log C \right]\] done
clear
C)
\[pH=1/2\left[ p{{K}_{w}}+p{{K}_{b}}-\log C \right]\] done
clear
D)
None of these done
clear
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question_answer9)
From separate solutions of sodium salts, NaW, NaX, NaY and NaZ have pH7.0,9.010.0 and ll.O respectively. When each solution was 0.1 M, the strongest acid is:
A)
HW done
clear
B)
HX done
clear
C)
HY done
clear
D)
HZ done
clear
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question_answer10)
Silver nitrate solution is gradually added to an aqueous solution containing 0.01 M each of chloride, bromide and iodide ions. The correct sequence in which the halides will be preacipitated is:
A)
Bromide, chloride, iodide done
clear
B)
Iodide, chloride, bromide done
clear
C)
Iodide, bromide, chloride done
clear
D)
Bromide, chloride done
clear
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question_answer11)
The pH of a buffer is 6.745. When 0.01 mole of NaOH is added to 1 litre of it, the pH changes to 6.832. Its buffer capacity is
A)
0.187 done
clear
B)
0.115 done
clear
C)
0.076 done
clear
D)
0.896 done
clear
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question_answer12)
Calculate the amount of\[{{(N{{H}_{4}})}_{2}}S{{O}_{4}}\]in grams which must be added to 500 ml of 0.2 M \[N{{H}_{3}}\], to yield a solution of pH=9, \[{{K}_{b}}\]for \[N{{H}_{3}}=2\times {{10}^{-5}}\]
A)
3.248 g done
clear
B)
4.248 g done
clear
C)
1.320 g done
clear
D)
6.248 g done
clear
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question_answer13)
When 10 ml of 0.1 M acetic acid (\[p{{K}_{a}}\]. = 5.0) is titrated against 10ml of 0.l Mammonia solution (\[p{{K}_{b}}\]=5.0), the equivalence point occurs at pH
A)
5.0 done
clear
B)
6.0 done
clear
C)
7.0 done
clear
D)
9.0 done
clear
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question_answer14)
Which statement is not true?
A)
pH of \[1\times {{10}^{8}}M\,\,HCl\] is 8 done
clear
B)
96500 coulomb deposits 1 g equivalent of copper done
clear
C)
Conjugate base of \[{{H}_{2}}P{{O}^{-}}_{4}\] is\[HP{{O}^{2-}}_{4}\]. done
clear
D)
\[pH+pOH=14\]for all aqueous solution done
clear
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question_answer15)
In a saturated solution of the sparingly soluble strong electrolyte \[AgI{{O}_{3}}\] (molecular mass = 283) the equilibrium which sets in is \[AgI{{O}_{3}}(s)\rightleftharpoons A{{g}^{+}}(aq)+I{{O}^{-}}_{3}(aq)\] 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)
\[28.3\times {{10}^{-2}}g\] done
clear
B)
\[28.3\times {{10}^{-3}}g\] done
clear
C)
\[1.0\times {{10}^{-7}}g\] done
clear
D)
\[1.0\times {{10}^{-4}}g\] done
clear
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question_answer16)
The first and second dissociation constant 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)
\[5.0\times {{10}^{-5}}\] done
clear
B)
\[5.0\times {{10}^{15}}\] done
clear
C)
\[5.0\times {{10}^{-15}}\] done
clear
D)
\[0.2\times {{10}^{5}}\] done
clear
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question_answer17)
Solubility product of silver bromide is \[5.0\times {{10}^{-13}}\]. The quantity of potassium bromid (molar mass taken as 120 g \[mo{{l}^{-1}}\]) to be added to 1 L of 0.05 M solution of silver nitrate to start the precipitatin of AgBr is
A)
\[1.2\times {{10}^{-10}}g\] done
clear
B)
\[1.2\times {{10}^{-9}}g\] done
clear
C)
\[6.2\times {{10}^{-5}}g\] done
clear
D)
\[5.0\times {{10}^{-8}}g\] done
clear
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question_answer18)
The best indicator for detection of end point in titration of a Weak acid and a strong base is
A)
Methy1 orange (3 to 4) done
clear
B)
Methy1 red (5 to 6) done
clear
C)
Bromothymol blue (6 to 7.5) done
clear
D)
Phenolphthalein (8 to 9.6) done
clear
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question_answer19)
When equal volumes of the following solutions are mixed, precipitation of AgCl (\[{{K}_{sp}}\] = \[1.8\times {{10}^{-10}}\]) will occur only with
A)
\[{{10}^{-4}}M(A{{g}^{+}})\,and\,{{10}^{-4}}M(C{{l}^{-}})\] done
clear
B)
\[{{10}^{-5}}M(A{{g}^{+}})\,and\,{{10}^{-5}}M(C{{l}^{-}})\] done
clear
C)
\[{{10}^{-16}}M(A{{g}^{+}})\,and\,{{10}^{-6}}M(C{{l}^{-}})\] done
clear
D)
\[{{10}^{-10}}M(A{{g}^{+}})\,and\,{{10}^{-10}}M(C{{l}^{-}})\] done
clear
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question_answer20)
The degree of dissociation of water at \[25{}^\circ C\] is \[1.9\times {{10}^{-7}}\] % and density is 1.0 g \[c{{m}^{-3}}\]. The ionic constant for water is
A)
\[1.0\times {{10}^{-10}}\] done
clear
B)
\[1.0\times {{10}^{-14}}\] done
clear
C)
\[1.0\times {{10}^{-16}}\] done
clear
D)
\[1.0\times {{10}^{-8}}\] done
clear
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question_answer21)
How much water in (in terms of \[{{10}^{2}}\]) ml must be added to 300 ml of 0.2 M solution or \[C{{H}_{3}}COOH\]\[({{K}_{a}}=1.8\times {{10}^{-5}})\]for the degree of ionisation of the acid to double?
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question_answer22)
The acid ionization (hydrolysis) constant of \[Z{{n}^{2+}}\]is \[1.0\times {{10}^{-9}}\].What is the pH of 0.001 M solution of \[ZnC{{l}_{2}}\]?
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question_answer23)
If 50 ml of 0.2 M NaCN is mixed with 50 ml of 0.2 M HCl, then \[({{K}_{b}}\,for\,C{{N}^{-}}=2\times {{10}^{-5}})\]calculate concentration of [\[{{H}_{3}}{{O}^{+}}\]] in terms of molarity \[\times {{10}^{-6}}\].
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question_answer24)
Amongst the following, the total number of compounds whose aqueous solution turns red litmus paper blue is
\[KCN\]
|
\[{{K}_{2}}S{{O}_{4}}\]
|
|
\[{{(N{{H}_{4}})}_{2}}{{C}_{2}}{{O}_{4}}\]
|
\[NaCl\]
|
\[Zn{{(N{{O}_{3}})}_{2}}\]
|
\[FeC{{l}_{3}}\]
|
\[{{K}_{2}}C{{O}_{3}}\]
|
|
\[N{{H}_{4}}N{{O}_{3}}\]
|
\[LiCN\]
|
|
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question_answer25)
The total number of diprotic acids among the following is
\[{{H}_{3}}P{{O}_{4}}\]
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\[{{H}_{2}}S{{O}_{4}}\]
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\[{{H}_{3}}P{{O}_{3}}\]
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\[{{H}_{2}}C{{O}_{3}}\]
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\[{{H}_{2}}{{S}_{2}}{{O}_{7}}\]
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\[{{H}_{3}}B{{O}_{3}}\]
|
\[{{H}_{3}}P{{O}_{2}}\]
|
\[{{H}_{2}}Cr{{O}_{4}}\]
|
\[{{H}_{2}}S{{O}_{3}}\]
|
|
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