Salt of Strong Acid and Weak Base

Q.

Is CO₂ Acidic or Basic?

Q. Aqueous solution of ammonium chloride $\left(N{H}_{4}Cl\right)$ is :

1. Acidic due to cationic hydrolysis.
2. Basic due to anionic hydrolysis.
3. Neutral.
4. Hydrolysis of both cation and anion occur.

Q. What is pH of 50 ml 0.1 (M) $N{H}_{4}OH$ and 50 ml 0.05 (M) HCI?
$p{K}_b=4.73$

1. 9.27
2. 9.37
3. 8.37
4. 9.47

Q. The hydrolysis constant of $N{H}_{4}Cl$ is $4\times {10}^{-10}$. Find the $pH$ of 0.1 molar solution of $N{H}_{4}Cl$ at equilibrium at ${25}^{\circ }C$.

1. 3.13
2. 7
3. 5.24
4. 8.95

Q.

The percentage of hydrolysis in $0.003M$ aqueous solution of $NaOCN$ is:

($Ka$ for $HOCN$ = $3.33\times {10}^{-4}M$)

1. 0.01 %

2. 0.1%

3. 0.001%

4. 0.0001%

Q. A solution contains $N{a}_{2}C{O}_3$ and $NaHC{O}_3$. $10\text{mL}$ of this solution required $2.5\text{mL}$ of $0.1\text{M}{H}_{2}S{O}_4$ for neutralization using phenolphthalein as an indicator. Methyl orange is then added when a further $2.5\text{mL}$ of $0.2\text{M}{H}_{2}S{O}_4$ was required. The amount of $N{a}_{2}C{O}_3$ and $NaHC{O}_3$ respectively, in 1 litre of solution is:

1. $5.3\text{g and 4.2 g}$
2. $\text{3.3 g and 6.2 g}$
3. $\text{4.2 g and 5.3 g}$
4. $\text{6.2 g and 3.3 g}$

Q. The base dissociation constant for hydrazine $N_2{H}_4$ is $9.6\times {10}^{-7}$. What would be the percent hydrolysis of $0.1M{N}_2{H}_{5}Cl$, a salt containing the acid ion conjugate to hydrazine base at ${25}^{\circ }C$?

1. $2.667\times {10}^{-3}$
2. $1.525\times {10}^{-4}$
3. $4.557\times {10}^{-6}$
4. $3.225\times {10}^{-2}$

Q.

Mixing of 0.1 mol of NaOH and 0.1 mol of acetic acid in one litre of water results into

1. an alkaline solution

2. a neutral solution

3. an acidic solution

4. a solution with no free ions

Q.

Distinguish between acidic and basic salts giving examples.

Q. A $25mL$ solution of $0.2MN{H}_{4}OH$ is titrated against $0.2MHCl$. Find the $pH$ of the solution when $25mL$ of $HCl$ is added.
$p{K}_b\left(N{H}_{4}OH\right)=4.74$

1. 8.37
2. 5.13
3. 4.74
4. 3.55

Q.

Mixing of 0.1 mol of NaOH and 0.1 mol of acetic acid in one litre of water results into

1. an acidic solution

2. an alkaline solution

3. a neutral solution

4. a solution with no free ${OH}^{-}$ ions

Q. A $20mL$ sollution of $0.02MN{H}_{4}OH$ is titrated with $0.4MHCl$. Find the $pH$ of the solution when $80mL$ of $HCl$ is added.
Given $p{K}_b\left(N{H}_{4}OH\right)=4.74$

1. 0.5
2. 2.5
3. 7
4. 4.4

Q.

Which of the following is acidic in nature?

1. $B(OH{)}_3$

2. $Mg(OH{)}_2$

3. $Al(OH{)}_3$

4. $B(OH{)}_3$