Calculate the hydrolysis constant and degree of hydrolysis of `NH_(4) Cl" in " 0.1` M solution .
`K_(b) = 1.8 xx 10^(-5)`. Calculate the concentration of `H^(+)` ions in the solution .

Explanation

To solve the problem of calculating the hydrolysis constant and degree of hydrolysis of `NH₄Cl` in a `0.1 M` solution, as well as the concentration of `H⁺` ions, we can follow these steps:

### Step 1: Understanding Hydrolysis of `NH₄Cl`
`NH₄Cl` is a salt formed from a weak base (`NH₃`) and a strong acid (`HCl`). When dissolved in water, it undergoes hydrolysis:
\[ NH₄^+ + H₂O \rightleftharpoons NH₃ + H₃O^+ \]

### Step 2: Calculate the Hydrolysis Constant (`K_h`)
The hydrolysis constant can be calculated using the relationship:
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