The `P^(H)` of a solution is 3.602. Its `H^(+)` ion concentration is

Options

A. `4xx 10^(-14)`
B. `2.5xx10^(-11)`
C. `2.5xx10^(-4)`
D. `5.0xx10^(-4)`

Answer

To find the \( H^+ \) ion concentration from the given pH value, we can follow these steps:

### Step 1: Understand the relationship between pH and \( H^+ \) concentration.
The pH of a solution is defined as the negative logarithm (base 10) of the hydrogen ion concentration (\( H^+ \)):
\[ \text{pH} = -\log[H^+] \]

### Step 2: Rearrange the formula to find \( H^+ \) concentration.
To find the \( H^+ \) concentration, we can rearrange the formula:
\[ [H^+] = 10^{-\text{pH}} \]

### Step 3: Substitute the given pH value into the equation.
The given pH value is 3.602. Substituting this value into the equation gives:
\[ [H^+] = 10^{-3.602} \]

### Step 4: Calculate \( 10^{-3.602} \).
Using a calculator, we can compute:
\[ [H^+] \approx 2.51 \times 10^{-4} \, \text{mol/L} \]

### Step 5: Round the answer to two significant figures.
Rounding to two significant figures, we have:
\[ [H^+] \approx 2.5 \times 10^{-4} \, \text{mol/L} \]

### Final Answer:
The \( H^+ \) ion concentration is \( 2.5 \times 10^{-4} \, \text{mol/L} \).

---