# 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

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

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

$$0.1\,M\,HCN$$ 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

$$Na{H_2}P{O_2}$$

$$Na{H_2}P{O_3}$$

$$Na{H_2}P{O_4}$$

None

## Questions 5 of 50

Question:Which one is the weakest acid

$$HN{O_3}$$

$$HCl{O_4}$$

$${H_2}S{O_4}$$

$$HBr$$

## Questions 6 of 50

Question:The conjugate acid of $${S_2}O_8^{2 - }$$ is

$${H_2}{S_2}{O_8}$$

$${H_2}S{O_4}$$

$$HSO_4^ -$$

$$H{S_2}O_8^ -$$

## Questions 7 of 50

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

$${H_2}O$$ 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

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

A conjugate base

A non-polar solvent

An acid

A base

## Questions 10 of 50

Question:The strongest Lewis base in the following

$$C{H_3}^ -$$

$${F^ - }$$

$$N{H_2}^ -$$

$$O{H^ - }$$

## Questions 11 of 50

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

Ionic nature

Acidic nature

Covalent nature

Electron deficient nature

## Questions 12 of 50

Question:Would gaseous HCl be considered as an Arrhenius acid

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 …..

$${s^2}$$

$$4{s^3}$$

$$3{s^2}$$

$${s^3}$$

## Questions 14 of 50

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

Increases

Decreases

Remains unchanged

$$NaCl$$decomposes

## Questions 15 of 50

Question:The correct representation for solubility product of $$Sn{S_2}$$is

$$3 \times {10^{ - 2}}\,M$$

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

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

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

## Questions 16 of 50

Question:A precipitate of calcium oxalate will not dissolve in

$$HCl$$

$$HN{O_3}$$

Aquaregia

$$C{H_3}COOH$$

## Questions 17 of 50

Question:Which one is a mixed salt

$$NaHS{O_4}$$

$$NaKS{O_4}$$

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

$$Mg(OH)Cl$$

## Questions 18 of 50

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

$$8 \times {10^{ - 3}}$$

$$8 \times {10^{ - 6}}$$

$$6.4 \times {10^{ - 5}}$$

$$6.4 \times {10^{ - 3}}$$

## Questions 19 of 50

Question:Any precipitate is formed when

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

$$2.0 \times {10^{ - 5}}\,m$$

$$1.0 \times {10^{ - 4}}\,m$$

$$5.0 \times {10^{ - 9}}\,m$$

$$2.2 \times {10^{ - 4}}\,m$$

## 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

$$62.5 \times {10^{ - 6}}$$

$$6.25 \times {10^{ - 4}}$$

$$15.625 \times {10^{ - 6}}$$

$$3.125 \times {10^{ - 6}}$$

## Questions 22 of 50

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

$$\frac{1}{{36}}$$

$$\frac{1}{6}$$

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

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

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

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

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

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

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

Both together

None

## Questions 25 of 50

Question:The compound insoluble in acetic acid is

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

$$62.5 \times {10^{ - 6}}$$

$$6.25 \times {10^{ - 4}}$$

$$15.625 \times {10^{ - 6}}$$

$$3.125 \times {10^{ - 6}}$$

## Questions 27 of 50

Question:An example for a strong electrolyte is

Urea

Ammonium hydroxide

Sugar

Sodium acetate

## Questions 28 of 50

Question:Which one is strongest electrolyte in the following

$$NaCl$$

$$C{H_3}COOH$$

$$N{H_4}OH$$

$${C_6}{H_{12}}{O_6}$$

## Questions 29 of 50

Question:Which will not affect the degree of ionization

Temperature

Concentration

Type of solvent

Current

## Questions 30 of 50

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

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?

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 ?

7

$$p{k_w}$$

Zero

1

## Questions 33 of 50

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

8

8

Between 7 and 8

Between 6 and 7

## Questions 34 of 50

Question:$$pH + pOH$$equal to

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

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

7.2

14

6.8

6

## Questions 37 of 50

Question:Highest pH 14 is given by

$$0.1\,M\,{H_2}S{O_4}$$

$$0.1\,M\,NaOH$$

$$1N\,NaOH$$

$$1N\,HCl$$

## Questions 38 of 50

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

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

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

$${10^{ - 8}}$$

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

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

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

$$1\,\,M\,\,C{H_3}COOH$$

$$5\,\,M\,\,C{H_3}COOH$$

$$5\,\,M\,\,HCl$$

$$1\,\,M\,\,N{H_4}OH$$

## Questions 44 of 50

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

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

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

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

$$N{H_4}Cl + N{H_4}OH$$

$$NaCl + NaOH$$

$$N{a_2}HP{O_4} + N{a_3}P{O_4}$$

$$C{H_3}COOH + C{H_3}COONa$$

## Questions 48 of 50

Question:Which solution has the highest pH value

$$1\,M\,KOH$$

$$1\,M\,{H_2}S{O_4}$$

Chlorine water

Water containing carbon dioxide

## Questions 49 of 50

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

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

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

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

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

## 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

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