Find the concentration of `H^+, HCO_3^- and CO_3^(2-)` in a 0.01 M solution of carbonic acid if the pH of this is 4.18, `K_a (H_2CO_3)=4.45 xx 10^(-7), K_(a)=(HCO_(3)^(-))=4.69 xx 10^(-11)`.

Explanation

To find the concentrations of \( H^+ \), \( HCO_3^- \), and \( CO_3^{2-} \) in a 0.01 M solution of carbonic acid (\( H_2CO_3 \)) with a pH of 4.18, we will follow these steps:

### Step 1: Calculate the concentration of \( H^+ \) ions from the pH
The concentration of hydrogen ions can be calculated using the formula:
\[ [H^+] = 10^{-\text{pH}} \]
Substituting the given pH value:
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