# Ionic Equilibrium Test 4

Total Questions:50 Total Time: 75 Min

Remaining:

## Questions 1 of 50

Question:Which of the following is the strongest conjugate base

$$C{l^ - }$$

$$C{H_3}CO{O^ - }$$

$$S{O_4}^{ - - }$$

$$N{O_2}^ -$$

## Questions 2 of 50

Question:$$NaOH$$ is a strong base because

It gives $$O{H^ - }$$ion

It can be oxidized

It can be easily ionized

Both 1 and2

## Questions 3 of 50

Question:In the equilibrium HClO4+H2O $$\leftrightarrow$$ H2O++$$ClO_4^ -$$

$$HCl{O_4}$$ is the conjugate acid of $${H_2}O$$

$${H_2}O$$ is the conjugate acid of $${H_3}{O^ + }$$

$${H_3}{O^ + }$$is the conjugate base of $${H_2}O$$

$$ClO_4^ -$$ is the conjugate base of $$HCl{O_4}$$

## Questions 4 of 50

Question:Which of the following would be expected to form ionic solution in water

$$CC{l_4}$$

$${O_2}$$

$$NaBr$$

$$CHB{r_3}$$

## Questions 5 of 50

Question:The conjugate acid of $$HPO_3^{2 - }$$is

$${H_3}P{O_4}$$

$${H_3}P{O_3}$$

$${H_2}PO_3^ -$$

$$PO_4^{3 - }$$

## Questions 6 of 50

Question:Which of the following compounds are diprotic

$${H_2}P{O_5}$$

$${H_2}S$$

$$HCl{O_3}$$

$${H_3}P{O_3}$$

## Questions 7 of 50

Question:The salt that forms neutral solution in water is

$$N{H_4}Cl$$

$$NaCl$$

$$N{a_2}C{O_3}$$

$${K_3}B{O_3}$$

## Questions 8 of 50

Question:The aqueous solution of which one of the following is basic

$$HOCl$$

$$NaHS{O_4}$$

$$N{H_4}N{O_3}$$

$$NaOCl$$

## Questions 9 of 50

Question:An aqueous solution of aluminium sulphate would show

An acidic reaction

A neutral reaction

A basic reaction

Both acidic and basic reaction

## Questions 10 of 50

Question:The aqueous solution of $$AlC{l_3}$$ is acidic due to the hydrolysis of

Aluminium ion

Chloride ion

Both aluminium and chloride ion

None of these

## Questions 11 of 50

Question:The aqueous solution of ammonium chloride is

Neutral

Basic

Acidic

Amphoteric

## Questions 12 of 50

Question:Which of the following is not a Lewis acid

$$B{F_3}$$

$$AlC{l_3}$$

$$HCl$$

$$LiAl{H_4}$$

## Questions 13 of 50

Question:In a saturated solution of electrolyte, the ionic product of their concentration are constant at constant temperature and this constant for electrolyte is known as

Ionic product

Solubility product

Ionization constant

Dissociation constant

## Questions 14 of 50

Question:Some salts although containing two different metallic elements give test for only one of them in solution. Such salts are

Double salts

Normal salts

Complex salts

Basic salts

## Questions 15 of 50

Question:A white salt is readily soluble in water and gives a colourless solution with a $$pH$$of about 9. The salt would be

$$N{H_4}N{O_3}$$

$$C{H_3}COONa$$

$$C{H_3}COON{H_4}$$

$$CaC{O_3}$$

## Questions 16 of 50

Question:If the solubility of a sparingly soluble salt of the type $$B{A_2}$$ (giving three ions on dissociation of a molecule) is $$x$$ moles per litre, then its solubility product is given by

$${x^2}$$

$$2{x^3}$$

$$4{x^2}$$

$$4{x^3}$$

## Questions 17 of 50

Question:The solubility product of silver sulphide is $$3.2 \times {10^{ - 11}}.$$Its solubility at the experimental temperature is

$$2 \times {10^{ - 4}}$$moles per litre

$$6 \times {10^{ - 6}}$$moles per litre

$$1.2 \times {10^{ - 5}}$$moles per litre

$$8 \times {10^{ - 4}}$$moles per litre

## Questions 18 of 50

Question:At equilibrium, if to a saturated solution of $$NaCl,\,HCl$$ is passed, $$NaCl$$ gets precipitated because

$$HCl$$ is a strong acid

Solubility of $$NaCl$$ decreases

Ionic product of $$NaCl$$ becomes greater than its $${K_{sp}}$$

$$HCl$$ is a weak acid

## Questions 19 of 50

Question:Which one of the following compounds is a Lewis acid

$$PC{l_3}$$

$$BC{l_3}$$

$$NC{l_3}$$

$$CHC{l_3}$$

## Questions 20 of 50

Question:In hydrolysis of a salt of weak acid and strong base, $${A^ - } + {H_2}O$$ $$\leftrightarrow$$ $$HA + O{H^ - },$$ the hydrolysis constant $$({K_h})$$ is equal to.…

$$\frac{{{K_w}}}{{{K_a}}}$$

$$\frac{{{K_w}}}{{{K_b}}}$$

$$\sqrt {\frac{{{K_a}}}{C}}$$

$$\frac{{{K_w}}}{{{K_a} \times {K_b}}}$$

## Questions 21 of 50

Question:At infinite dilution, the percentage ionisation for both strong and weak electrolytes is

1%

20%

50%

100%

## Questions 22 of 50

Question:The degree of ionization of a compound depends on

Size of solute molecules

Nature of solute molecules

Nature of vessel used

Quantity of electricity passed

## Questions 23 of 50

Question:The best conductor of electricity is a 1.0 M solution of

Boric acid

Acetic acid

Sulphuric acid

Phosphoric acid

## Questions 24 of 50

Question:The colour of an electrolyte solution depends on

The nature of the anion

The nature of the cation

The nature of both the ions

The nature of the solvent

## Questions 25 of 50

Question:At 25$$^\circ$$C, the dissociation constant of a base BOH is $$1.0 \times {10^{ - 12}}$$. The concentration of Hydroxyl ions in 0.01 M aqueous solution of the base would be

$$2.0 \times {10^{ - 6}}mol\,{L^{ - 1}}$$

$$1.0 \times {10^{ - 5}}mol\;{L^{ - 1}}$$

$$1.0 \times {10^{ - 6}}mol\,{L^{ - 1}}$$

$$1.0 \times {10^{ - 7}}mol\;{L^{ - 1}}$$

## Questions 26 of 50

Question:Aqueous solution of $$HCl$$ has the $$pH = 4$$. Its molarity would be

4 M

0.4 M

0.0001 M

10 M

## Questions 27 of 50

Question:The compound whose 0.1 M solution is basic is

Ammonium acetate

Calcium carbonate

Ammonium sulphate

Sodium acetate

## Questions 28 of 50

Question:The following reaction is known to occur in the body $$C{O_2} + {H_2}O$$ $$\leftrightarrow$$ $${H_2}C{O_3}$$ $$\leftrightarrow$$ $${H^ + } + HCO_3^ - .$$ If $$C{O_2}$$escapes from the system

$$pH$$ will decrease

Hydrogen ion concentration will decrease

$${H_2}C{O_3}$$ concentration will be unaltered

The forward reaction will be promoted

## Questions 29 of 50

Question:The pH of the solution containing $$10\,ml$$ of a $$0.1\,N\,NaOH$$ and $$10\,ml$$ of $$0.05\,N$$ $${H_2}S{O_4}$$ would be

1

0

7

> 7

## Questions 30 of 50

Question:The $$pH$$ of $${10^{ - 7}}M\,NaOH$$ is

7.01

Between 7 and 8

Between 9 and 10

Greater than 10

## Questions 31 of 50

Question:$$20ml$$ of $$0.5N\,HCl$$ and $$35\,ml$$ of $$0.1N\,NaOH$$ are mixed. The resulting solution will

Be neutral

Be basic

Turn phenolphthalein solution pink

Turn methyl orange red

## Questions 32 of 50

Question:The $$pH$$ of a 0.02 M solution of hydrochloric acid is

2

1.7

0.3

2.2

## Questions 33 of 50

Question:Amongst the following solutions, the buffer solution is

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

$$N{H_4}Cl + NaOH$$solution

$$N{H_4}OH + HCl$$solution

$$NaOH + HCl$$solution

## Questions 34 of 50

Question:The $$pH$$ of solution having $$[O{H^ - }] = {10^{ - 7}}$$ is

7

14

Zero

$$- 7$$

## Questions 35 of 50

Question:At $${80^o}C,$$ distilled water has $$[{H_3}{O^ + }]$$ concentration equal to $$1 \times {10^{ - 6}}\,\,mole/litre.$$ The value of $${K_w}$$at this temperature will be

$$1 \times {10^{ - 6}}$$

$$1 \times {10^{ - 9}}$$

$$1 \times {10^{ - 12}}$$

$${K_{SP}}$$

## Questions 36 of 50

Question:The $$pH$$ value of $$0.1\,\,M\,\,NaOH$$ solution is (when there is a given reaction $$[{H^ + }]\,[O{H^ - }] = {10^{ - 15}}$$)

13

12

11

2

## Questions 37 of 50

Question:The $$pH$$ of a solution obtained by mixing $$50\,\,ml$$ of $$0.4\,\,N\,\,HCl$$ and $$50\,\,ml$$ of $$0.2\,\,N\,\,NaOH$$is

$$- \log 2$$

$$- \log 0.2$$

1

2

## Questions 38 of 50

Question:Which of the following is a buffer

$$NaOH + C{H_3}COONa$$

$$NaOH + N{a_2}S{O_4}$$

$$1 \times {10^{ - 4}}$$

$$N{H_4}OH + C{H_3}COON{H_4}$$

## Questions 39 of 50

Question:The concentration of hydronium $$({H_3}{O^ + })$$ ion in water is

Zero

$$1 \times {10^7}\,gm\,\,ion/litre$$

$$1 \times {10^{ - 14}}\,gm\,\,ion/litre$$

$$1 \times {10^{ - 7}}\,gm\,\,ion/litre$$

## Questions 40 of 50

Question:A solution whose pH value is less than 7 will be

Basic

Acidic

Neutral

Buffer

## Questions 41 of 50

Question:The $$pH$$ of a $${10^{ - 10}}$$ molar $$HCl$$ solution is approximately

10

7

1

14

## Questions 42 of 50

Question:The $${H^ + }$$ion concentration is $$1.0 \times {10^{ - 6}}$$ mole/litre in a solution. Its pH value will be

12

6

18

24

## Questions 43 of 50

Question:Which buffer solution out of the following will have $$pH > 7$$

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

$$HCOOH + HCOOK$$

$$C{H_3}COON{H_4}$$

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

## Questions 44 of 50

Question:The $$p{K_a}$$ of equimolecular sodium acetate and acetic acid mixture is 4.74. If $$pH$$ is

7

9.2

4.74

14

## Questions 45 of 50

Question:The gastric juice in our stomach contains enough $$HCl$$ to make the hydrogen ion concentration about $$0.01\,\,mole/litre.$$ The $$pH$$of gastric juice is

0.01

1

2

14

## Questions 46 of 50

Question:Addition of which chemical will decrease the hydrogen ion concentration of an acetic acid solution

$$N{H_4}Cl$$

$$A{l_2}{(S{O_4})_3}$$

$$AgN{O_3}$$

$$HCN$$

## Questions 47 of 50

Question:$$Ka$$of $${H_2}{O_2}$$is of the order of

$${10^{ - 12}}$$

$${10^{ - 14}}$$

$${10^{ - 16}}$$

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

## Questions 48 of 50

Question:Equivalent weight of an acid

Depends on the reaction involved

Depends upon the number of oxygen atoms present

Is always same

None of the above

## Questions 49 of 50

Question:The $$pH$$value of $$0.1\,\,M\,\,HCl$$is approximately 1. What will be the approximate $$pH$$value of 0.05 $$M\,\,{H_2}S{O_4}$$

0.05

0.5

1

2

## Questions 50 of 50

Question:The $${K_{sp}}$$ of $$Mg{(OH)_2}$$ is $$1 \times {10^{ - 12}},\,0.01M\,Mg{(OH)_2}$$ will precipitate at the limiting pH