Ionic Equilibrium Test 9

Total Questions:50 Total Time: 75 Min

Remaining:

 

Questions 1 of 50

Question:Which of the following is not a Lewis acid

Answers Choices:

CO

\(SiC{l_4}\)

\(S{O_3}\)

\(Z{n^{2 + }}\)

Questions 2 of 50

Question:The strength of an acid depends on its tendency to

Answers Choices:

Accept protons

Donate protons

Accept electrons

Donate electrons

Questions 3 of 50

Question:In the following reaction \(H{C_2}{O_4}^ - + P{O_4}^{ - - - }\) ? \(HP{O_4}^{ - - } + {C_2}{O_4}^{ - - }\) Which are the two Bronsted bases

Answers Choices:

\(0.1\,M\,HCN\) and \(P{O_4}^{ - - - }\)

\(HP{O_4}^{ - - }\) and \({C_2}{O_4}^{ - - }\)

\(N{H_4}Cl\) and \(P{O_4}^{ - - - }\)

\(P{O_4}^{ - - - }\) and \(pH\)

Questions 4 of 50

Question:Which one is not an acid salt

Answers Choices:

\(Na{H_2}P{O_2}\)

\(Na{H_2}P{O_3}\)

\(Na{H_2}P{O_4}\)

None

Questions 5 of 50

Question:Which one is the weakest acid

Answers Choices:

\(HN{O_3}\)

\(HCl{O_4}\)

\({H_2}S{O_4}\)

\(HBr\)

Questions 6 of 50

Question:The conjugate acid of \({S_2}O_8^{2 - }\) is

Answers Choices:

\({H_2}{S_2}{O_8}\)

\({H_2}S{O_4}\)

\(HSO_4^ - \)

\(H{S_2}O_8^ - \)

Questions 7 of 50

Question:In the reaction \(HCl + {H_2}O\)? \({H_3}{O^ + } + C{l^ - }\)

Answers Choices:

\({H_2}O\) is the conjugate base of \(HCl\) acid

\(C{l^ - }\)is the conjugate base of \(HCl\)acid

\(C{l^ - }\)is the conjugate acid of \({H_2}O\) base

\({H_3}{O^ + }\)is the conjugate base of \(HCl\)

Questions 8 of 50

Question:Ammonium ion is

Answers Choices:

Neither an acid nor base

Both an acid and a base

A conjugate acid

A conjugate base

Questions 9 of 50

Question:Ammonia gas dissolves in water to form \(N{H_4}OH\). In this reaction water acts as

Answers Choices:

A conjugate base

A non-polar solvent

An acid

A base

Questions 10 of 50

Question:The strongest Lewis base in the following

Answers Choices:

\(C{H_3}^ - \)

\({F^ - }\)

\(N{H_2}^ - \)

\(O{H^ - }\)

Questions 11 of 50

Question:Boron halides behave as Lewis acids, because of their

Answers Choices:

Ionic nature

Acidic nature

Covalent nature

Electron deficient nature

Questions 12 of 50

Question:Would gaseous HCl be considered as an Arrhenius acid

Answers Choices:

Yes

No

Not known

Gaseous HCl does not exist

Questions 13 of 50

Question:The solubility of \(Ca{F_2}\) is a moles/litre. Then its solubility product is …..

Answers Choices:

\({s^2}\)

\(4{s^3}\)

\(3{s^2}\)

\({s^3}\)

Questions 14 of 50

Question:On passing a current of \(HCl\) gas in a saturated solution of \(NaCl,\) the solubility of \(NaCl\)

Answers Choices:

Increases

Decreases

Remains unchanged

\(NaCl\)decomposes

Questions 15 of 50

Question:The correct representation for solubility product of \(Sn{S_2}\)is

Answers Choices:

\(3 \times {10^{ - 2}}\,M\)

\([S{n^{2 + }}]\,\,{[{S^{2 - }}]^2}\)

\([S{n^{2 + }}]\,\,[2{S^{2 - }}]\)

\([S{n^{4 + }}]\,\,{[2{S^{2 - }}]^2}\)

Questions 16 of 50

Question:A precipitate of calcium oxalate will not dissolve in

Answers Choices:

\(HCl\)

\(HN{O_3}\)

Aquaregia

\(C{H_3}COOH\)

Questions 17 of 50

Question:Which one is a mixed salt

Answers Choices:

\(NaHS{O_4}\)

\(NaKS{O_4}\)

\({K_4}Fe{(CN)_6}\)

\(Mg(OH)Cl\)

Questions 18 of 50

Question:If \({K_{sp}}\) for \(HgS{O_4}\) is \(6.4 \times {10^{ - 5}},\) then solubility of the salt is

Answers Choices:

\(8 \times {10^{ - 3}}\)

\(8 \times {10^{ - 6}}\)

\(6.4 \times {10^{ - 5}}\)

\(6.4 \times {10^{ - 3}}\)

Questions 19 of 50

Question:Any precipitate is formed when

Answers Choices:

Solution becomes saturated

The value of ionic product is less that than the value of solubility product

The value of ionic product is equal than the value of solubility product

The value of ionic product is greater than the value of solubility product

Questions 20 of 50

Question:The solubility product of \(AgCl\) is \(4.0 \times {10^{ - 10}}\) at \(298\,\,K.\) The solubility of \(AgCl\)in \(0.04\,m\,\,CaC{l_2}\) will be

Answers Choices:

\(2.0 \times {10^{ - 5}}\,m\)

\(1.0 \times {10^{ - 4}}\,m\)

\(5.0 \times {10^{ - 9}}\,m\)

\(2.2 \times {10^{ - 4}}\,m\)

Questions 21 of 50

Question:The saturated solution of \(A{g_2}S{O_4}\) is \(2.5 \times {10^{ - 2}}\,M.\) Its solubility product \(({K_{sp}})\) is

Answers Choices:

\(62.5 \times {10^{ - 6}}\)

\(6.25 \times {10^{ - 4}}\)

\(15.625 \times {10^{ - 6}}\)

\(3.125 \times {10^{ - 6}}\)

Questions 22 of 50

Question:\({K_{sp}}\)for sodium chloride is \(36\,\,mo{l^2}/litr{e^2}.\) The solubility of sodium chloride is

Answers Choices:

\(\frac{1}{{36}}\)

\(\frac{1}{6}\)

6

3600

Questions 23 of 50

Question:According to the reaction \(PbC{l_2} = P{b^2} + 2C{l^ - },\)the solubility coefficient of \(NaOH + HCl\)is

Answers Choices:

\([P{b^{2 + }}]\,{[C{l^ - }]^2}\)

\([P{b^{2 + }}]\,[C{l^ - }]\)

\({[P{b^{2 + }}]^2}\,[C{l^ - }]\)

None of these

Questions 24 of 50

Question:\({K_{sp}}\) value of \(Al\,{(OH)_3}\) and \(Zn\,{(OH)_2}\) are \(8.5 \times {10^{ - 23}}\)and \(1.8 \times {10^{ - 14}}\) respectively. If \(N{H_4}OH\) is added in a solution of \(A{l^{3 + }}\)and \(Z{n^{2 + }},\) which will precipitate earlier

Answers Choices:

\(Al\,{(OH)_3}\)

\(Zn\,{(OH)_2}\)

Both together

None

Questions 25 of 50

Question:The compound insoluble in acetic acid is

Answers Choices:

Calcium oxide

Calcium carbonate

Calcium oxalate

Calcium hydroxide

Questions 26 of 50

Question:A saturated solution of \(A{g_2}S{O_4}\)is \(2.5 \times {10^{ - 2}}\)M; The value of its solubility product is

Answers Choices:

\(62.5 \times {10^{ - 6}}\)

\(6.25 \times {10^{ - 4}}\)

\(15.625 \times {10^{ - 6}}\)

\(3.125 \times {10^{ - 6}}\)

Questions 27 of 50

Question:An example for a strong electrolyte is

Answers Choices:

Urea

Ammonium hydroxide

Sugar

Sodium acetate

Questions 28 of 50

Question:Which one is strongest electrolyte in the following

Answers Choices:

\(NaCl\)

\(C{H_3}COOH\)

\(N{H_4}OH\)

\({C_6}{H_{12}}{O_6}\)

Questions 29 of 50

Question:Which will not affect the degree of ionization

Answers Choices:

Temperature

Concentration

Type of solvent

Current

Questions 30 of 50

Question:The addition of a polar solvent to a solid electrolyte results in

Answers Choices:

Polarization

Association

Ionization

Electron transfer

Questions 31 of 50

Question:0.1 mole of CH3NH2 (Kb = 5 ´ 10-4) is mixed with 0.08 mole of HCl and diluted to one litre. What will be the H+ concentration in the solution?

Answers Choices:

8 ´ 10\(^{ - 2}\) M

8 ´ 10\(^{ - {\rm{11}}}\)M

1.6 ´ 10\(^{ - {\rm{11}}}\) M

8 ´ 10\(^{ - 5}\) M

Questions 32 of 50

Question:What will be the sum of \(pH\)and \(pOH\) in an aqueous solution ?

Answers Choices:

7

\(p{k_w}\)

Zero

1

Questions 33 of 50

Question:The \(pH\) of a \({10^{ - 9}}M\) solution of \(HCl\) in water is

Answers Choices:

8

8

Between 7 and 8

Between 6 and 7

Questions 34 of 50

Question:\(pH + pOH\)equal to

Answers Choices:

Zero

Fourteen

A negative number

Infinity

Questions 35 of 50

Question:The pH value of \(1.0 \times {10^{ - 8}}M\,HCl\) solution is less than 8 because \(HCl\) is completely ionised at this concentration

Answers Choices:

The ionization of water is negligible

The ionization of water cannot be assumed to be negligible in comparison with this low concentration of \(HCl\)

The pH cannot be calculated at such a low concentration of \(HCl\)

\(HCl\) is completely ionised at this concentration

Questions 36 of 50

Question:What is the pH for a neutral solutions at the normal temperature of the human body

Answers Choices:

7.2

14

6.8

6

Questions 37 of 50

Question:Highest pH 14 is given by

Answers Choices:

\(0.1\,M\,{H_2}S{O_4}\)

\(0.1\,M\,NaOH\)

\(1N\,NaOH\)

\(1N\,HCl\)

Questions 38 of 50

Question:What will be the \(pH\)of a \({10^{ - 8}}\,M\,HCl\) solution

Answers Choices:

8

7

6.98

14

Questions 39 of 50

Question:To obtain a buffer which should be suitable for maintaining a \(pH\)of about \(4 - 5,\) we need to have in solution, a mixture of

Answers Choices:

A strong base + its salt with a weak acid

A weak base + its salt with a strong acid

A strong acid + its salt with a weak base

A weak acid + its salt with a strong base

Questions 40 of 50

Question:The concentration of \(NaOH\) solution is\({10^{ - 8}}\,M.\) Find out the \((O{H^ - })\) concentration

Answers Choices:

\({10^{ - 8}}\)

Greater than \({10^{ - 6}}\)

\({10^{ - 6}}\)

Lies between \({10^{ - 6}}\)and \({10^{ - 7}}\)

Questions 41 of 50

Question:In a solution of acetic acid, sodium acetate is added, then its pH value

Answers Choices:

Decreases

Increases

Remains unchanged

both 1,2 are correct

Questions 42 of 50

Question:If pOH of a solution is 6.0, then its pH will be

Answers Choices:

6

10

8

14

Questions 43 of 50

Question:The \(pH\) of a buffer solution containing \(25\,ml\)of \(1\,M\,C{H_3}COONa\) and \(25\,\,ml\) of \(1\,\,M\,\,C{H_3}COOH\) will be appreciably affected by \(5\,\,ml\) of

Answers Choices:

\(1\,\,M\,\,C{H_3}COOH\)

\(5\,\,M\,\,C{H_3}COOH\)

\(5\,\,M\,\,HCl\)

\(1\,\,M\,\,N{H_4}OH\)

Questions 44 of 50

Question:The \(pH\)value of decinormal solution of \(N{H_4}OH\) which is 20% ionised, is

Answers Choices:

13.3

14.7

12.3

12.95

Questions 45 of 50

Question:If \(0.4\,gm\,\,NaOH\) is present in 1 litre solution, then its \(pH\) will be

Answers Choices:

2

10

11

12

Questions 46 of 50

Question:Assuming complete ionisation, the \(pH\) of \(0.1\,M\,\,HCl\)is 1. The molarity of \({H_2}S{O_4}\) with the same \(pH\) is

Answers Choices:

0.2

0.1

2

0.05

Questions 47 of 50

Question:Out of the following, which pair of solutions is not a buffer solution

Answers Choices:

\(N{H_4}Cl + N{H_4}OH\)

\(NaCl + NaOH\)

\(N{a_2}HP{O_4} + N{a_3}P{O_4}\)

\(C{H_3}COOH + C{H_3}COONa\)

Questions 48 of 50

Question:Which solution has the highest pH value

Answers Choices:

\(1\,M\,KOH\)

\(1\,M\,{H_2}S{O_4}\)

Chlorine water

Water containing carbon dioxide

Questions 49 of 50

Question:The hydrogen ion concentration of 0.001 \(M\,\,NaOH\) solution is

Answers Choices:

\(1 \times {10^{ - 2}}mole/litre\)

\(1 \times {10^{ - 11}}mole/litre\)

\(1 \times {10^{ - 14}}mole/litre\)

\(1 \times {10^{ - 12}}mole/litre\)

Questions 50 of 50

Question:The rapid change of pH near the stoichiometric point of an acid-base titration is the basis of indicator detection. pH of the solution is related to ratio of the concentrations of the conjugate acid (HIn) and base \((I{n^ - })\)forms of the indicator by the expression

Answers Choices:

\(\log \frac{{[HIn]}}{{[I{n^ - }]}} = pH - p{K_{In}}\)

\(\log \frac{{[I{n^ - }]}}{{[HIn]}} = pH - p{K_{In}}\)

\(\log \frac{{[I{n^ - }]}}{{[HIn]}} = p{K_{In}} - pH\)

\(\log \frac{{[HIn]}}{{[I{n^ - }]}} = p{K_{In}} - pH\)