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question_answer1)
Silver ions are added to solution with \[[B{{r}^{-}}]=[C{{l}^{-}}]=[CO_{3}^{2-}]=[AsO_{4}^{3-}]=0.1\,M\]. Which compound will precipitate at lowest \[[A{{g}^{+}}]\]?
A)
\[AgBr({{K}_{sp}}=5\times {{10}^{-13}})\] done
clear
B)
\[AgCl({{K}_{sp}}=1.8\times {{10}^{-10}})\] done
clear
C)
\[A{{g}_{2}}C{{O}_{3}}({{K}_{sp}}=8\times {{10}^{-12}})\] done
clear
D)
\[A{{g}_{3}}As{{O}_{4}}({{K}_{sp}}={{10}^{-22}})\] done
clear
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question_answer2)
pH of 2M HCl solution at \[25{}^\circ \]
A)
Ph < 0 done
clear
B)
0 < pH > 1 done
clear
C)
0 done
clear
D)
1 done
clear
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question_answer3)
Taking \[Ba{{(OH)}_{2}}\] to be completely ionised. The pH of its 0.001 M solution is
A)
11.3 done
clear
B)
2.7 done
clear
C)
11 done
clear
D)
3 done
clear
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question_answer4)
The ionization constant of \[HCOOH\] is \[1.8\times {{10}^{-4}}\]. What is the percent ionization of a 0.001 M solution?
A)
66% done
clear
B)
42% done
clear
C)
34% done
clear
D)
58% done
clear
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question_answer5)
Which of the following statements is not correct?
A)
\[{{I}^{-}}\] is a weaker base than \[{{F}^{-}}\] done
clear
B)
\[H{{O}^{-}}\] is a stronger base than \[{{H}_{2}}{{N}^{-}}\] done
clear
C)
\[HON{{H}_{2}}\] is a weaker base than \[N{{H}_{3}}\] done
clear
D)
\[{{F}_{3}}{{C}^{-}}\] is a stronger base than \[C{{l}_{3}}{{C}^{-}}\] done
clear
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question_answer6)
The pH of solution, containing 0.1 N HCI and \[0.1\,N\,C{{H}_{3}}COOH\,({{K}_{a}}=2\times {{10}^{-5}})\] is
A)
1 done
clear
B)
0.7 done
clear
C)
3 done
clear
D)
1.3 done
clear
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question_answer7)
Equal volumes of two HCl solutions of \[pH=3\] and were mixed. What is the pH of the resulting solution?
A)
3.5 done
clear
B)
4.0 done
clear
C)
4.5 done
clear
D)
3.3 done
clear
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question_answer8)
Select the best indicator from the given table for titration of 20 mL of \[0.02\,M\,\,C{{H}_{3}}COOH\] with 0.02 M NaOH. Given \[p{{K}_{a}}\,(C{{H}_{3}}COOH)=4.74\]
| Indicator | pH Range |
(I) | Bromothy mol blue | 6.0-7.6 |
(II) | Thymolphthalein | 9.3-11.05 |
(III) | Malachite green | 11.4-13 |
(IV) | M-Cresol purple | 7.4-9.0 |
A)
I done
clear
B)
II done
clear
C)
III done
clear
D)
IV done
clear
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question_answer9)
Of the following acids |
I. Hypophosphorous acid |
II. Orthophosphorous acid |
III. Caro's acid |
IV. Glycine |
A)
I, II monobasic; III dibasic acid and IV amphoteric done
clear
B)
II monobasic; I, III dibasic acid and IV amphoteric done
clear
C)
I monobasic; II, III dibasic acid and IV amphoteric done
clear
D)
I, II, III dibasic acids and IV amphoteric done
clear
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question_answer10)
\[N{{H}_{4}}Cl\] is acidic, because:
A)
on hydrolysis, \[N{{H}_{4}}Cl\] gives weak base \[N{{H}_{4}}OH\] and strong acid \[HCl\] done
clear
B)
nitrogen donates a pair of electron done
clear
C)
it is a salt of weak acid and strong base done
clear
D)
on hydrolysis, \[N{{H}_{4}}Cl\] gives strong base and weak acid done
clear
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question_answer11)
pH of an aqueous solution of HCl is 5. if 1 c.c. of this solution is diluted to 1000 times. The pH will become
A)
8 done
clear
B)
5 done
clear
C)
6.9 done
clear
D)
None done
clear
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question_answer12)
In which case change in pH is maximum?
A)
1 mL of pH = 2 is diluted to 100 mL done
clear
B)
0.01 mol of \[NaOH\] is added to 100 mL of 0.01 M \[NaOH\] solution done
clear
C)
100 mL of \[{{H}_{2}}O\] is added to 900 mL of \[{{10}^{-6}}\] M \[HCl\] done
clear
D)
100 mL of pH = 2 solution is mixed with 100 mL of pH = 12 done
clear
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question_answer13)
Which relation is wrong
A)
\[{{10}^{-pH}}+{{10}^{-pOH}}={{10}^{-14}}\] done
clear
B)
\[pH\alpha \frac{1}{[{{H}^{+}}]}\] done
clear
C)
\[{{K}_{w}}\alpha \,T\] done
clear
D)
dissociation constant of water \[K=1.8\times {{10}^{-16}}\] done
clear
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question_answer14)
If acetic acid is 1.0% ionised in its decinormal solution, then pH of its seminormal solution will be
A)
3.4 done
clear
B)
4.8 done
clear
C)
1.6 done
clear
D)
2.6 done
clear
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question_answer15)
Which of the following species would be least likely to act as Lewis base?
A)
\[PC{{l}_{3}}\] done
clear
B)
\[C{{N}^{-}}\] done
clear
C)
\[SC{{l}_{2}}\] done
clear
D)
\[{{I}^{+}}\] done
clear
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question_answer16)
Which of the following cannot have a conjugate base?
A)
\[{{H}_{2}}PO_{2}^{-}\] done
clear
B)
\[HCO_{3}^{-}\] done
clear
C)
\[{{H}_{2}}{{O}_{2}}\] done
clear
D)
\[HSO_{4}^{-}\] done
clear
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question_answer17)
Choose the correct order of strength of following acids. |
(i) \[C{{H}_{3}}C{{H}_{2}}C{{H}_{2}}COOH\] |
(ii) \[~C{{H}_{3}}C{{H}_{2}}CH(Br)COOH\] |
(iii) \[C{{H}_{3}}CH(Br)C{{H}_{2}}COOH\] |
(IV) \[{{(C{{H}_{3}})}_{2}}CHCOOH\] |
A)
I < II < III < IV done
clear
B)
IV < I < III < II done
clear
C)
IV < III < I < II done
clear
D)
II < I < III < IV done
clear
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question_answer18)
Match List I with List II and select the correct answer using the code given below the lists
List I | List II |
[A] pH of 0.1 M HA \[(p{{K}_{a}}=5)\] and 0.01 M NaA | (p) 4 |
[B] pH of 0.1 M BOH \[(p{{K}_{b}}=6)\] and 0.1 M BCI | (q) 7 |
[C] pH of 0.1 M salt of HA \[(p{{K}_{a}}=5)\] and BOH \[(p{{K}_{b}}=7)\] | (r) 6 |
[D] pH of 500 litre of 0.2 M \[HN{{O}_{3}}\] and 500 litre 0.2 M NaOH | (s) 8 |
Codes:
A)
A\[\to \]p, B\[\to \]s, C\[\to \]r, D\[\to \]q done
clear
B)
A\[\to \]s, B\[\to \]p, C\[\to \]r, D\[\to \]q done
clear
C)
A\[\to \]p, B\[\to \]r, C\[\to \]s, D\[\to \]q done
clear
D)
A\[\to \]p, B\[\to \]s, C\[\to \]q, D\[\to \]r done
clear
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question_answer19)
A solution saturated in lime water has a pH of 12.4. Then the Ksp for \[Ca{{(OH)}_{2}}\] is:
A)
\[3.2\times {{10}^{-3}}\] done
clear
B)
\[7.8\times {{10}^{-6}}\] done
clear
C)
\[7.8\times {{10}^{-28}}\] done
clear
D)
\[3.2\times {{10}^{-4}}\] done
clear
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question_answer20)
Which will act as a buffer solution
A)
\[200\text{ }ml\text{ }N/10\text{ }NaOH\]\[+100\text{ }ml\text{ }N/20\text{ }HCl\] done
clear
B)
\[100\text{ }ml\text{ }0.1\text{ }N\text{ }NaOH\]\[+100\text{ }ml\text{ }0.1\text{ }N\text{ }HCl\] done
clear
C)
\[100\,\,ml\,\,0.1\,\,N\,NaOH\]\[+50\,\,ml\,\,0.2N\,C{{H}_{3}}OOH\] done
clear
D)
\[100\text{ }ml\text{ }0.1\text{ }N\text{ }NaOH\]\[+150\text{ }ml\text{ }0.1\text{ }N\text{ }HCN\] done
clear
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question_answer21)
100 mL of 1 M \[HCl\] is mixed with 50 mL of 2 M \[HCl\]. Hence, \[\left[ {{H}_{3}}{{O}^{+}} \right]\] is:
A)
1.00 M done
clear
B)
1.50 M done
clear
C)
1.33 M done
clear
D)
3.00 M done
clear
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question_answer22)
The solubility product of \[Mg{{(OH)}_{2}}\] is \[{{10}^{-14}}\]. The solubility of \[Mg{{(OH)}_{2}}\] in a buffer solution of \[pH=8\] is
A)
\[{{10}^{-8}}\] done
clear
B)
\[{{10}^{-6}}\] done
clear
C)
\[{{10}^{-2}}\] done
clear
D)
\[{{10}^{-4}}\] done
clear
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question_answer23)
At \[30{}^\circ C\] the solubility of \[A{{g}_{2}}C{{O}_{3}}\] \[({{K}_{SP}}=8\times {{10}^{-12}})\] would be greatest in one litre of:
A)
\[0.05M\,\,N{{a}_{2}}C{{O}_{3}}\] done
clear
B)
\[0.05M\,AgN{{O}_{3}}\] done
clear
C)
Pure water done
clear
D)
\[0.05M\,{{K}_{2}}C{{O}_{3}}\] done
clear
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question_answer24)
A mixture of weak acid is \[0.1\text{ }M\] in \[HCOOH\] \[({{K}_{a}}=1.8\times {{10}^{-4}})\] and \[0.1\text{ }M\] in \[HOCN\,\,({{K}_{a}}=3.1\times {{10}^{-4}})\] Hence, \[[{{H}_{3}}{{O}^{\oplus }}]\] is
A)
\[7.0\times {{10}^{-3}}M\] done
clear
B)
\[4.1\times {{10}^{-4}}M\] done
clear
C)
\[0.20M\] done
clear
D)
\[4.1\times {{10}^{-3}}M\] done
clear
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question_answer25)
The solubility of \[AgCl\] in water at \[25{}^\circ C\] is \[1.79\times {{10}^{-3}}g/L\]. The \[{{K}_{sp}}\] of \[AgCl\] at \[25{}^\circ C\] is
A)
\[1.68\times {{10}^{-12}}\] done
clear
B)
\[1.55\times {{10}^{-10}}\] done
clear
C)
\[12.4\times {{10}^{-8}}\] done
clear
D)
\[1.73\times {{10}^{-14}}\] done
clear
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question_answer26)
Solubility of \[PbC{{l}_{2}}\] in 0.5 M NaCl is \[{{S}_{1}}\] and that in 0.5 M \[Pb{{(N{{O}_{3}})}_{2}}\] is \[{{S}_{2}}\] then which of 5 the following is correct:
A)
\[\frac{{{S}_{1}}}{{{S}_{2}}}=1\] done
clear
B)
\[{{S}_{1}}-{{S}_{2}}>0\] done
clear
C)
\[{{S}_{1}}-{{S}_{2}}<0\] done
clear
D)
\[\frac{{{S}_{1}}}{{{S}_{2}}}>1\] done
clear
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question_answer27)
Arrange the following in increasing order of \[pH\,\,KN{{O}_{3}}(aq),\,C{{H}_{3}}COON(aq),\]\[N{{H}_{4}}Cl(aq),\,{{C}_{6}}{{H}_{5}}COON{{H}_{4}}(aq)\]
A)
\[C{{H}_{3}}COONa<{{C}_{6}}{{H}_{5}}COON{{H}_{4}}\]\[<N{{H}_{4}}Cl<KN{{O}_{3}}\] done
clear
B)
\[KN{{O}_{3}}<N{{H}_{4}}C<C{{H}_{3}}COONa\]\[<{{C}_{6}}{{H}_{5}}COONa\] done
clear
C)
\[N{{H}_{4}}Cl<KN{{O}_{3}}<C{{H}_{3}}COONa\]\[<{{C}_{6}}{{H}_{5}}COON{{H}_{4}}\] done
clear
D)
\[N{{H}_{4}}Cl<KN{{O}_{3}}<{{C}_{6}}{{H}_{5}}COON{{H}_{4}}\]\[<C{{H}_{3}}COONa\] done
clear
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question_answer28)
Blue litmus turns red in which of the following mixture of acid and base?
A)
\[100\,mL\] of \[1\times {{10}^{-2}}M\,{{H}_{2}}S{{O}_{4}}\]\[+\,100\,mL\] of \[1\times {{10}^{-2}}M\,Ca{{\left( OH \right)}_{2}}\] done
clear
B)
\[100\,mL\] of \[1\times {{10}^{-2}}M\,HCl\]+ \[100\,mL\] of \[1\times {{10}^{-2}}M\,Ba{{\left( OH \right)}_{2}}\] done
clear
C)
\[100\,mL\] of \[1\times {{10}^{-2}}M\,{{H}_{2}}S{{O}_{4}}\]\[+\,10\,mL\] of \[1\times {{10}^{-2}}M\,NaOH\] done
clear
D)
\[100\,mL\] of \[1\times {{10}^{-2}}M\,HCl\]\[+\,100\,mL\] of \[1\times {{10}^{-2}}M\,NaOH\] done
clear
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question_answer29)
The degree of ionization of a compound depends on
A)
size of solute done
clear
B)
nature of solute done
clear
C)
nature of vessel done
clear
D)
quantity of electricity passed done
clear
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question_answer30)
What is the minimum pH when \[Fe{{(OH)}_{3}},\] starts precipitating from a solution containing \[0.1M\text{ }FeC{{l}_{3}}\]? \[{{k}_{sp}}\] of \[Fe{{(OH)}_{3}}=8\times {{10}^{-13}}{{M}^{3}}(\log \text{ }2\text{ }=\text{ }0.3)\]
A)
3.7 done
clear
B)
5.7 done
clear
C)
10.3 done
clear
D)
8.3 done
clear
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question_answer31)
The number of moles of \[N{{H}_{3}}\] that must be added to 1 L of 0.1 M \[AgN{{O}_{3}}\] to reduce \[A{{g}^{+}}\] concentration to \[2\times {{10}^{-7}}M\] are Given, \[{{K}_{dis}}{{[Ag{{(N{{H}_{3}})}_{2}}]}^{+}}=6.8\times {{10}^{-8}}\]
A)
0.184 M done
clear
B)
0.384 M done
clear
C)
0.293 M done
clear
D)
0.0539 M done
clear
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question_answer32)
10 mL, of a strong acid solution of \[pH=2.000\] are mixed with 990 mL of another strong acid solution of \[pH=4.000\]. The pH of the resulting solution will be:
A)
4.002 done
clear
B)
4.000 done
clear
C)
4.200 done
clear
D)
3.7 done
clear
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question_answer33)
Conjugate base of \[NH_{4}^{+}\] is
A)
\[N{{H}_{3}}\] done
clear
B)
\[NH_{2}^{-}\] done
clear
C)
\[N{{H}_{4}}OH\] done
clear
D)
\[C{{l}^{-}}\] done
clear
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question_answer34)
The correct order of acidic strength is:
A)
\[C{{l}_{2}}{{O}_{7}}>S{{O}_{2}}>{{P}_{4}}{{O}_{10}}\] done
clear
B)
\[C{{O}_{2}}>{{N}_{2}}{{O}_{5}}>S{{O}_{3}}\] done
clear
C)
\[N{{a}_{2}}O>MgO>A{{l}_{2}}{{O}_{3}}\] done
clear
D)
\[{{K}_{2}}O>CaO>MgO\] done
clear
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question_answer35)
Match list I (Solutions of salts of...) with list II (pH of the solution is given by) and select the correct answer using the codes given below the lists:
List I | List II |
Weak acid and strong base | (p) \[\frac{1}{2}p{{K}_{w}}\] |
Strong acid and weak base | (q) \[\frac{1}{2}(p{{K}_{w}}-p{{K}_{b}}+p{{K}_{a}})\] |
Weak acid and weak base | (r) \[\frac{1}{2}(p{{K}_{w}}-p{{K}_{b}}-\log \,\,C)\] |
Strong acid and strong base | (s) \[\frac{1}{2}(p{{K}_{w}}+p{{K}_{a}}+\log \,\,C)\] |
Codes:
A)
A\[\to \]p, B\[\to \]q, C\[\to \]r, D\[\to \]s done
clear
B)
A\[\to \]s, B\[\to \]r, C\[\to \]q, D\[\to \]p done
clear
C)
A\[\to \]s, B\[\to \]r, C\[\to \]p, D\[\to \]q done
clear
D)
A\[\to \]r, B\[\to \]s, C\[\to \]q, D\[\to \]p done
clear
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