Equilibrium - Part 2 - Live Session

The pH of 0.1 M solution of the following slats increases in the order
1. NaCl < NH $_{4}$ Cl < NaCN < HCl
2. HCl < NH $_{4}$ Cl < NaCl < NaCN
3. NaCN < NH $_{4}$ Cl < NaCl <HCl
4. HCl < NaCl < NaCN < NH $_{4}$ Cl

The degree of hydrolysis in hydrolytic equilibrum $A^{-} + H_{2} O ⇌ H A + O H^{-}$
at salt concentration of 0.001 M is ( $K_{a} = 1 \times 10^{- 5})$
1. 1 $\times$ 10 $^{- 3}$
2. 1 $\times$ 10 $^{- 4}$
3. 5 $\times$ 10 $^{- 4}$
4. 1 $\times$ 10 $^{- 6}$

Henderson's equation is pH = pK $_{a}$ + log $\frac{[S a l t]}{a c i d}$ .
If the acid gets half neutralized the value of pH will be : (pK $_{a}$ =4.30)
1. 4.3
2. 2.15
3. 8.60
4. 7

The solubility product of CuS, Ag $_{2}$ S. HgS are 10 $^{- 37}, 10^{- 44}$ and 10 $^{- 54}$ respectively. The solubilities of these sulphides are in the order of:
1. Ag $_{2}$ S > CuS > HgS
2. Ag $_{2}$ S > HgS > CuS
3. HgS > Ag $_{2}$ S > CuS
4. CuS > Ag $_{2}$ S > HgS

The solubility product constant K $_{s p}$ of Mg (OH) $_{2}$ is 9.0 $\times$ 10 $^{- 12}$ . If a solution is 0.010 M with respect to Mg $^{2 +}$ ions, what is the maximum hydroxide ion concentration which
could be present without causing the precipitation of Mg(OH) $_{2}$
1. 1.5 $\times$ 10 $^{- 7}$ M
2. 3.0 $\times$ 10 $^{- 7}$ M
3. 1.5 $\times$ 10 $^{- 5}$ M
4. 3.0 $\times$ 10 $^{- 5}$ M

The pH of a 0.01 M solutions of acetic acid having degree of dissociation 12.5% is
1. 5.623
2. 2.903
3. 3.723
4. 4.509

Whcih of the following solutions will have pH closed to 1.0
1. 100 ml of $\frac{M}{10}$ HCl + 100 ml of $\frac{M}{10}$ NaOH
2. 55 ml of $\frac{M}{10}$ HCl = 45 ml of $\frac{M}{10}$ NaOH
3. 10 ml of $\frac{M}{10}$ HCl + 90 ml of $\frac{M}{10}$ NaOH
4. 75 ml of $\frac{M}{10}$ HCl + 25 ml of $\frac{M}{10}$ NaOH

In which of the following solvents will AgBr have the highest solubility
1. 10 $^{- 3}$ M NaBr
2. 10 $^{- 3}$ M NH4OH
3. Pure water
4. 10 $^{- 3}$ M HBr

How many grams of Ca $C_{2} O_{4}$ (molecular weight= 128) on dissolving in distilled water
will give a saturated solution
$[K_{s p} (C a C_{2} O_{4}) = 2.5 \times 10^{- 9} m o l^{2 / l - 2}]$
1. 0.0064 g
2. 0.1280 g
3. 0.0128 g
4.1. 2800 g

10.

Which may be added to one litre of water to act as a buffer
1. One mole of $H C_{2} H_{3} O_{2}$ and 0.5 mole of NaOH
2. One mole of NH $_{4}$ C1 and one mole of HC1
3. One mole of NH $_{4}$ OH and one mole of NaOH
4. One mole of $H C_{2} H_{3} O_{2}$ and one mole of NaOH

11.

A solution of weak acid HA containing 0.01 moles of acid per litre of solutions has pH=4. The percentage degree of ionisation of the acid and the ionisation constant of acid are respectively-
1. 1%, 10^-6
2. 0.01%, 10^-4
3. 1% 10^-4
4. 0.01%, 10^-6

12.

40 mg of pure sodium hydroxide is dissolved in 10 litres of distilled water. The pH of the
solution is
1. 9.0
2. 10
3. 11
4. 12

13.

A monoprotic acid in a 0.1 M solution ionizes to 0.001%.Its ionisation constant is
1. $1.0 \times 10^{- 3}$
2. $1.0 \times 10^{- 6}$
3. $1.0 \times 10^{- 8}$
4. $1.0 \times 10^{- 11}$

14.

With increase in temperature, ionic product of water
1. decreases
2. increases
3. remains same
4. may increase or decrease

15.

pH of pure water at 25 $°$ C is 7 . If water is heated to 60 $°$ C, the
1. pH will decrease
2. pH will increase
3. pH will remain constant
4. H $^{+}$ ions and OH $^{-}$ ions concentrations will become unequal.

16.

If $S_{1}, S_{3}, S_{3}$ and S $_{4}$ are the solubilities of Ag Cl in water, ion 0.01 M CaCl $_{2}$ , in M NaCl and in 0.05 M agNO $_{3}$ respectively at a certain temperature, the correct order of solubilities is
1. S $_{1}$ >S $_{2}$ >S $_{3}$ >S $_{4}$
2. S $_{1}$ >S $_{3}$ >S $_{2}$ >S $_{4}$
3. S $_{1}$ >S $_{2}$ >S $_{3}$ >S $_{4}$
4. none of these

17.

Which salt is maximum hydolysed?
1. NH $_{4}$ C1
2. CuSO $_{4}$
3. A1C1 $_{3}$
4. All have same extent of hydrogen

18.

Which mixture acts as buffer?
1.50 ml M CH $_{3}$ COOH + 100 ml 1 M NaOH
2. 50 ml M CH $_{3}$ COOH + 25 ml 1 M NaOH
3. 50 ml NH $_{4}$ OH+ 100 ml 1 M HC1
4. 50 ml NH $_{4}$ OH+ 25 ml 1 M NaOH

19.

pH of Ba(OH) $_{2}$ solution is 12. Its solubility product is
1. 10 $^{- 6} M^{3}$
2. 4 $\times$ 10 $^{- 6} M^{3}$
3. 5 $\times$ 10 $^{- 7} M^{3}$
4. 5 $\times$ 10 $^{- 6} M^{3}$

20.

When a solution of acetic acid was titrated with NaOH, the pH of the solution when half of the acid, neutralised was 4.74 Dissociation constant of the acid is
1. 1.8 $\times$ 10 $^{- 5}$
2. 3.2 $\times$ 10 $^{- 5}$
3. 8.7 $\times$ 10 $^{- 5}$
4. 6.42 $\times$ 10 $^{- 5}$

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