Salt of Strong Acid and Weak Base

Q. What is the $\left[O{H}^{-}\right]$ in the final solution prepared by mixing $20.0mL\text{of}0.050M$ $HCl$ with $30.0mL\text{of}0.10MBa(OH{)}_2$?

1. 0.005 M
   
2. 0.12 M
3. 0.10 M
   
4. 0.40 M

Q. 2.5 mL of $\frac{2}{5}M$ weak monoacidic base ($K_b=1\times {10}^{-12}$) at ${25}^{o}C$ is titrated with $\frac{2}{15}M$ HCl in water at ${25}^{o}C.$ The concentration of $H^{+}$ at equivalence point is $(K_w=1\times {10}^{-14}at{25}^{o}C)$

1. $3.7\times {10}^{-13}M$
2. $3.2\times {10}^{-7}M$
3. $3.2\times {10}^{-2}M$
4. $2.7\times {10}^{-2}M$

Q. The ionization constant of Ammonium hydroxide is $1.77\times {10}^{-5}$ at 298 K. It is hydrolysis constant is

1. 
2. 
3. 
4. 

Q.

Give examples of Basic salt, Complex Salt and Normal Salt.

Q. 40 ml of 0.1 M ammonia solution is mixed with 20 mL of 0.1 M HCl. What is the pH of a mixture? ($p{K}_b$ of ammonia solution is 4.74)

1. 9.26
   
2. 2.26
   
3. 4.74
   
4. 5

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

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

Q. Calculate amount of $N{H}_{4}Cl$ required to be dissolved in $500mL$ water to have $pH=5.[K_{b}N{H}_{4}OH=1.8\times {10}^{-5}].$
(Molar mass of $N{H}_{4}Cl=53.5gmo{l}^{-1}$)

1. 1.855 g
2. 2.543 g
3. 4.815 g
4. 6.066 g

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. Enthalpy of neutralization of acetic acid and sodium hydroxide is -55.4 kJ/mol. The enthalpy of ionization of acetic acid is

1. - 5.54 kJ/mol
2. + 5.54 kJ/mol
3. - 1.7 kJ/mol
4. + 1.7 kJ/mol

Q.

The pH of a 0.001M $NaOH$ will be

1. 3

2. 11

3. 2

4. 12

Q. Calculate pH of mixture of $(400mL,\frac{1}{200}MBa(OH{)}_2)+(400mL,\frac{1}{50}MHCl)+(200\text{mL of water})$
$log2=0.3010$

1. 2.4
2. 7
3. more than 7
4. 4.5

Q.

What is the normality of 2.5 M sulphuric acid?

Q.

The compound whose $0.1\mathrm{M}$ solution is basic?

1. ${\mathrm{NH}}_4\mathrm{Cl}$

2. ${\mathrm{CH}}_3\mathrm{COONa}$

3. ${\mathrm{Na}}_2{\mathrm{SO}}_4$

4. ${\mathrm{CH}}_3{\mathrm{COONH}}_4$

Q.

Does $\mathrm{NaCl}$ undergo hydrolysis?

Q.

Hydrolysis constant of a salt $NaX$ is ${10}^{‑8}$ The pH of 0.01 M solution of the weak acid $HX$ is

1. 12

2. 6

3. 8

4. 4

Q.

Give two examples of mineral acid.

Q. Calculate the pH of 0.1 M $N{H}_{4}Cl$ solution in water :
$K_b\left(N{H}_{4}OH\right)=1.8\times {10}^{-5}$

1. 4.5
2. 7.63
3. 5.13
4. 6.53

Q. 100 mL solution of $HCl$ having concentration of $0.06M$ is mixed with an another 400 mL solution of $NaOH$ having a concentration of $0.01M$. The resultant pH of the mixture is :

1. 1.5
2. 9.6
3. 2.4
4. 11.5

Q. Aniline behaves as a weak base. When $0.1M,50mL$ solution of aniline was mixed with $0.1M,25mL$ solution of $HCl$ the $pH$ of resulting solution was 8. The $pH$ of $0.01M$ solution of anilinium chloride will be:

1. $5$
2. $4.5$
3. $6$
4. $6.5$

Q.

A solution of $CuS{O}_4$ is

1. Acidic in nature

2. Alkaline in nature

3. Neutral in nature

4. Amphoteric in nature

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

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

Q. The hydrolysis constant of $N{H}_{4}Cl$ is $5.6\times {10}^{-6}$. Find the $pH$ of 0.1 molar solution of $N{H}_{4}Cl$ at equilibrium. When $log1.79=0.253$.

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

Q. Calculate the pH of 0.1 M $N{H}_{4}Cl$ solution in water :
$K_b\left(N{H}_{4}OH\right)=1.8\times {10}^{-5}$

1. 4.5
2. 7.63
3. 6.53
4. 5.13

Q.

A white substance having alkaline nature in solution is

1. NaNO₃

2. Na₂CO₃

3. NH₄Cl

4. Fe₂O₃

Q. The basic ionisation constant for hydrazine, $N_2{H}_4$ is $9.6\times {10}^{-7}$. What would be the percentage hydrolysis of $0.1M{N}_2{H}_{5}Cl$ ?
$(Given:\sqrt{10.4}\approx 3.2and\sqrt{1.04}=1.013)$

1. $0.01\%$
2. $3.2\%$
3. $1.013\%$
4. $0.032\%$

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. A $50mL$ of $0.02MN{H}_{4}OH$ solution is titrated with $0.02MHCl$. Find the $pH$ of the solution when $50.1mL$ of $HCl$ is added.
Given: $K_b\left(N{H}_{4}OH\right)=1.8\times {10}^{-5}$

1. 2.65
2. 4.65
3. 10.35
4. 9.35

Q. The treatment of alkyl chlorides with aqueous $KOH$ leads to the formation of alcohols but in the presence of alcoholic $KOH$, alkenes are major products. Explain.

Q. The pH of a solution obtained by mixing 100 ml of 0.2 M ${CH}_{3}COOH$ with 100 ml of 0.1 M $NaOH$ will be: ($p{K}_a$ for ${CH}_{3}COOH$ = 4.74 )

1. 4.74
2. 9.1
3. 8.87
4. 8.57

Q. If the hydrolysis constant of $N{H}_{4}Cl$ is $2\times {10}^{-5}$ at $298K$. Find the $pH$ of $0.5M$ solution of $N{H}_{4}Cl$ at equilibrium.
Given : $\log 5=0.7$

1. 8.22
2. 2.5
3. 7.34
4. 4.85