Number of `H^(+)` ions present in 10 mL of solution of `pH=3` are:

Options

A. `10^(13)`
B. `6.02xx10^(18)`
C. `6.02xx10^(13)`
D. `6.002xx10^(10)`

Explanation

To find the number of \( H^+ \) ions present in 10 mL of a solution with a pH of 3, we can follow these steps:

### Step 1: Calculate the concentration of \( H^+ \) ions
The concentration of \( H^+ \) ions can be calculated using the formula:
\[ [H^+] = 10^{-\text{pH}} \]
Given that the pH is 3, we can substitute this value into the formula:
\[ [H^+] = 10^{-3} \, \text{mol/L} \]

### Step 2: Convert the volume of the solution to liters
Since we have the volume in milliliters, we need to convert it to liters:
\[ \text{Volume} = 10 \, \text{mL} = 10 \times 10^{-3} \, \text{L} = 0.01 \, \text{L} \]

### Step 3: Calculate the number of moles of \( H^+ \) ions
Using the concentration and the volume, we can find the number of moles of \( H^+ \) ions:
\[ \text{Moles of } H^+ = [H^+] \times \text{Volume} = 10^{-3} \, \text{mol/L} \times 0.01 \, \text{L} = 10^{-5} \, \text{mol} \]

### Step 4: Convert moles to the number of ions
To find the total number of \( H^+ \) ions, we multiply the number of moles by Avogadro's number (\( 6.02 \times 10^{23} \) ions/mol):
\[ \text{Number of } H^+ \text{ ions} = \text{Moles of } H^+ \times \text{Avogadro's number} = 10^{-5} \, \text{mol} \times 6.02 \times 10^{23} \, \text{ions/mol} \]
\[ = 6.02 \times 10^{18} \, \text{ions} \]

### Final Answer
The number of \( H^+ \) ions present in 10 mL of a solution with a pH of 3 is \( 6.02 \times 10^{18} \) ions.

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