Choose the correct set of True/Fasle for following statements:
(i) Silver chloride is more soluble in very concentrated sodium chloride solution than in pure water.
(ii) The pH of a buffer solution does not change on addition of small amount of an acid or a base.
(iii) Addition of `NH_(4)Cl` does not affect the pH of a solution of `NH_(4)OH`
(iv) Degree of hydrolysis of ammonium acetate does not depend upon the concentration of ammonium acetate solution.
(v) A mixture of acetic acid and sodium acetate can act as buffer solution.

Options

A. TTFTT
B. FTTTF
C. TFTFT
D. FTTTT

Answer

To determine the truth value of each statement, we will analyze them one by one.

### Step-by-Step Solution:

1. **Statement (i)**: Silver chloride is more soluble in very concentrated sodium chloride solution than in pure water.
- **Analysis**: Silver chloride (AgCl) dissociates into Ag⁺ and Cl⁻ ions. In a concentrated sodium chloride (NaCl) solution, there is an abundance of Cl⁻ ions. According to the common ion effect, the presence of a common ion (Cl⁻) will shift the equilibrium to the left, thus decreasing the solubility of AgCl. Therefore, this statement is **False**.

2. **Statement (ii)**: The pH of a buffer solution does not change on addition of a small amount of an acid or a base.
- **Analysis**: Buffer solutions are designed to resist changes in pH when small amounts of acid or base are added. They maintain a relatively constant pH. Thus, this statement is **True**.

3. **Statement (iii)**: Addition of NH₄Cl does not affect the pH of a solution of NH₄OH.
- **Analysis**: NH₄Cl dissociates into NH₄⁺ and Cl⁻. NH₄OH is a weak base. The addition of NH₄Cl introduces NH₄⁺, which can react with OH⁻ ions, forming NH₄OH. This reaction does not significantly change the pH of the solution, as it forms a buffer system. Therefore, this statement is **True**.

4. **Statement (iv)**: Degree of hydrolysis of ammonium acetate does not depend upon the concentration of ammonium acetate solution.
- **Analysis**: The degree of hydrolysis does depend on the concentration of the solution. As the concentration increases, the degree of hydrolysis typically decreases due to Le Chatelier's principle. Therefore, this statement is **False**.

5. **Statement (v)**: A mixture of acetic acid and sodium acetate can act as a buffer solution.
- **Analysis**: Acetic acid (a weak acid) and sodium acetate (the salt of the weak acid) can indeed form a buffer solution. This combination allows the solution to resist changes in pH upon the addition of small amounts of acid or base. Therefore, this statement is **True**.

### Summary of Truth Values:
- (i) False
- (ii) True
- (iii) True
- (iv) False
- (v) True

### Final Answer:
The correct set of True/False for the statements is:
- (i) F
- (ii) T
- (iii) T
- (iv) F
- (v) T