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
View Answer play_arrow
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
View Answer play_arrow
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
View Answer play_arrow
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
View Answer play_arrow
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
View Answer play_arrow
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
View Answer play_arrow
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
View Answer play_arrow
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
View Answer play_arrow
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
View Answer play_arrow
\[N{{H}_{4}}Cl\] 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
View Answer play_arrow
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
View Answer play_arrow
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
View Answer play_arrow
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
View Answer play_arrow
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
View Answer play_arrow
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
View Answer play_arrow
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
View Answer play_arrow
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
View Answer play_arrow
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
View Answer play_arrow
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
View Answer play_arrow
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
View Answer play_arrow
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
View Answer play_arrow
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
View Answer play_arrow
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
View Answer play_arrow
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
View Answer play_arrow
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
View Answer play_arrow
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
View Answer play_arrow
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
View Answer play_arrow
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
View Answer play_arrow
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
View Answer play_arrow
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
View Answer play_arrow
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
View Answer play_arrow
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
View Answer play_arrow
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
View Answer play_arrow
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
View Answer play_arrow
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
View Answer play_arrow