Find the concentration of `H^(o+), HCO_(3)^(Θ)`, and `CO_(3)^(-2)` in a `0.01M` solution of carbonic acid if the `pH` of solution is `4.18`.
`K_(1) = 4.45 xx 10^(-7),K_(2) = 4.69 xx 10^(-11)`

Explanation

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

### Step 1: Calculate the concentration of \( H^+ \) ions

The pH of a solution is defined as:

\[
\text{pH} = -\log[H^+]
...