Out of the following salts:
i. `NaH_(2)BO_(3)` ii. `NH_(2)CH_(2)COOH`
iii. `CH_(3)COONH_(4)` iv. `NaHS`
Salts (i) has concentration-depends `pH`.

Explanation

To determine whether the statement "Salts (i) has concentration-depends pH" is true or false, we will analyze the given salts one by one, focusing on the first salt, `NaH2BO3`.

### Step-by-Step Solution:

1. **Identify the Nature of the Salt**:
- The first salt is `NaH2BO3`, which is the sodium salt of boric acid (H3BO3).
- It is formed from a strong base (NaOH) and a weak acid (H3BO3).

2. **Understand the pH Dependence**:
- When a salt is derived from a strong base and a weak acid, it can hydrolyze in water. This hydrolysis affects the pH of the solution.
- The hydrolysis of `NaH2BO3` can be represented as:
\[ NaH_2BO_3 \rightarrow Na^+ + H_2BO_3^- \]
- The `H2BO3^-` ion can further react with water:
\[ H_2BO_3^- + H_2O \rightleftharpoons H_3BO_3 + OH^- \]
- This reaction produces hydroxide ions (OH^-), which increases the pH of the solution.

3. **Expression for pH**:
- The pH of a solution containing a salt that hydrolyzes can be expressed using the formula:
\[ pH = 14 + pK_a + \log C \]
- Here, \(C\) is the concentration of the salt, and \(pK_a\) is the dissociation constant of the weak acid (in this case, boric acid).

4. **Conclusion**:
- From the formula, it is clear that the pH of the solution depends on the concentration of the salt (`C`). Therefore, the statement that "salts (i) has concentration-depends pH" is **True**.

### Final Answer:
The statement is **True**.