Salt of Weak Acid and Strong Base

Q. Calculate the degree of hydrolysis ($h$) of a $0.1M$ sodium acetate solution at $298K$.
Given: $K_a=1.8\times {10}^{-5}$

1. $8.42\times {10}^{-5}$
2. $7.42\times {10}^{-6}$
3. $7.42\times {10}^{-5}$
4. $8.42\times {10}^{-6}$

Q.

Physical and chemical Properties of acids, bases and salts. (5-10 properties for each)

Q. Which of the following is correct for a salt of weak acid and strong base?
Here C is the concentration of the salt.

1. $pH=7+\frac{1}{2}(p{K}_a+logC)$
2. $pH=7+\frac{1}{2}(p{K}_b+logC)$
3. $K_h=\frac{K_w}{K_a}$
4. $K_h\times K_w=K_a$

Q. The pH of 1 M $C{H}_{3}COONa$ solution in water will be nearly: $(p{K}_{a}forC{H}_{3}COOH=4.74)$

1. 12.37
2. 11.37
3. 7.37
4. 9.37

Q.

Define the term basicity of an acid. Give the basicity of nitric acid, sulphuric acid, and phosphoric acid.

Q.

The pH of a sample of vinegar is 3.76. Calculate the concentration of hydrogen ion in it.

Q.

What is the pH of baking soda?

Q.

The increasing order of reducing the power of the halogen acids is

1. $\mathrm{HF}<\mathrm{HCI}<\mathrm{HBr}<\mathrm{HI}$

2. $\mathrm{HI}<\mathrm{HBr}<\mathrm{HCI}<\mathrm{HF}$

3. $\mathrm{HBr}<\mathrm{HCI}<\mathrm{HF}<\mathrm{HI}$

4. HCI < HBr < HF < HI

Q.

The ionization constant of nitrous acid is $4.5\times {10}^{-4}$. Calculate the pH of 0.04 M sodium nitrite solution and also its degree of hydrolysis.

Q. Amongst the following, the total number of compounds whose aqueous solution turns red litmus paper blue is ___

KCN $K_{2}S{O}_4$ $(N{H}_4{)}_2{C}_2{O}_4$ $NaCl$ $Zn(N{O}_3{)}_2$ $FeC{l}_3$ $K_{2}C{O}_3$ $N{H}_{4}N{O}_3$
$LiCN$

Q. What is the pH when 25.0 mL of 0.2 M of $C{H}_{3}COOH$ has been titrated with 35.0 mL of 0.1 M $NaOH$ ?
$p{K}_a\left(C{H}_{3}COOH\right)=4.752$
$log2.333=0.368$

1. 7
2. 3.45
3. 5.12
4. 6.52

Q.

The solubility product of a sparingly soluble salt $A_{2}B$ is $3.2\times {10}^{-11}$. Its solubility in $mol{L}^{-1}$ is:

1. $4\times {10}^{-4}$
2. $2\times {10}^{-4}$
3. $6\times {10}^{-4}$
4. $3\times {10}^{-4}$

Q.

Predict if the solutions of the following salts are neutral, acidic or basic:
$NaCl,KBr,NaCN,N{H}_{4}N{O}_3,NaN{O}_2$ and KF

Q. A $50mL$ solution of $0.2MC{H}_{3}COOH$ is titrated against $0.2MNaOH$. Find the $pH$ of the solution when $50mL$ of $NaOH$ is added.
$p{K}_a\left(C{H}_{3}COOH\right)=4.74$

1. 5.66
2. 10.52
3. 8.87
4. 9.44

Q. On dissolving 1 mole of each of the following acid in 1lit. water, the acid which does not give a solution of strength 1N is

1. $HN{O}_3$
2. HCl
3. Perchloric acid
4. Phosphoric acid

Q. Which of the following substances gives a flame colouration different from the other?

1. Caustic potash
2. Nitre
3. Table salt
4. Potassium chloride

Q. When 50 mL of 0.1 M NaOH is added to 50 mL of 0.1 M $C{H}_{3}COOH$ solution, the pH will be:
(use :$(p{K}_a{)}_{aceticacid}=5,log2=0.3,log3=0.5,log5=0.7)$

1. 4.75
2. 9.75
3. 4.25
4. 8.85

Q. The pH of ammonium acetate can be calculated by using the expression:

1. 
   
   
2. 
3. 
4. 

Q. The pH of 1 M $C{H}_{3}COONa$ solution in water will be nearly: $(p{K}_{a}forC{H}_{3}COOH=4.74)$

1. 12.37
2. 7.37
3. 11.37
4. 9.37

Q. Calculate the pH of solution obtained by mixing 10ml of 0.2M HCL and 40ml of 0.1M H2SO4.

Q. Which of the following statement(s) is/are correct for an equimolar aqueous solution of $HCl$ and $N{H}_{4}OH$?

1. $N{H}_4^{+}$ ions will undergo hydrolysis to form $N{H}_{4}OH$
2. Solution will be basic in nature.
3. Solution will be acidic in nature.
4. Hydrolysis does not occur

Q. What is pH of 50 ml 0.05 (M) NaOH and 50 ml 0.1 (N)
​$C{H}_{3}COOH$
$p{K}_a=4.73$

1. 4.73
2. 4.63
3. 3.73
4. 4.83

Q. pH of 0.01 M solution of HA is 4. Find the value of pKa of HA at ${25}^{\circ }C$

Q. Choose the correct statements for an aqueous solution of $KOCl$

1. The solution will be basic in nature
2. The solution will be acidic in nature.
3. Cationic $\left(K^{+}\right)$ hydrolysis occurs.
4. Anionic $\left(OC{l}^{-}\right)$ hydrolysis occurs

Q. For sodium acetate solution in water, the given equilibrium reaction occur:
$C{H}_{3}CO{O}^{-}\left(aq\right)+H_{2}O\left(l\right)\stackrel{hydrolysis}{\rightleftharpoons }C{H}_{3}COOH\left(aq\right)+O{H}^{-}\left(aq\right)$
Which of the following describes the correct relation ?
(where $h$ is the degree of hydrolysis of salt)

1. $h=\sqrt{\frac{K_w\cdot C}{K_a}}$
2. $h=\sqrt{\frac{K_w}{K_a\cdot C}}$
3. $h=\sqrt{\frac{K_a\cdot C}{K_w}}$
4. $h=\sqrt{\frac{K_a}{K_w\cdot C}}$

Q.

The pH of an aqueous solution at ${25}^{\circ }C$ having 0.1 M NaOH and 0.3 M to acetic acid ($p{K}_a$ = 4.76) would be nearly

1. 4.25

2. 4.45

3. 4.75

4. 5.05

Q.

Which of the following solutions has the maximum pH value?

1. 0.2 M

2. 0.2 M

3. 0.2 M

4. 0.2 M HCl

Q. what is the quantity of NaOH present in 250cc of the solution , so that it gives a pH=1

Q. $50mL$ of a $0.1MC{H}_{3}COONa\left(aq\right)$ is titrated against a $0.1MHCl\left(aq\right)$. Calculate the $pH$ of solution when $50mLHCl$ was added.
Given: $p{K}_a\left(C{H}_{3}COOH\right)=4.74at{25}^{o}C$

1. 4.74
2. 3.02
3. 5.25
4. 4.24

Q. A $20mL$ of $0.02MC{H}_{3}COOH$ is titrated with $0.2MNaOH$. Find the $pH$ of the solution when $80mL$ of $NaOH$ has been added.
Given $p{K}_a\left(C{H}_{3}COOH\right)=4.74$

1. 13.2
2. 12.2
3. 0.8
4. 1.8