\[{H_2}S{O_4}\] is a stronger acid than {H_2}S{O_3} .A. TrueB. False

To determine if \(\text{H}_2\text{SO}_4\) (sulfuric acid) is a stronger acid than \(\text{H}_2\text{SO}_3\) (sulfurous acid), we need to look at their acid strengths.

**Sulfuric Acid (\(\text{H}_2\text{SO}_4\)):**

1. **Sulfuric acid** is a strong acid that dissociates completely in water. The dissociation is:
\[\text{H}_2\text{SO}_4 \rightarrow \text{H}^+ + \text{HSO}_4^-\]
\[\text{HSO}_4^- \rightarrow \text{H}^+ + \text{SO}_4^{2-}\]

Sulfuric acid is classified as a strong acid because it dissociates almost completely in water, releasing a high concentration of hydrogen ions (\(\text{H}^+\)).

**Sulfurous Acid (\(\text{H}_2\text{SO}_3\)):**

1. **Sulfurous acid** is a weaker acid compared to sulfuric acid. It dissociates in water as follows:
\[\text{H}_2\text{SO}_3 \rightarrow \text{H}^+ + \text{HSO}_3^-\]

\[\text{HSO}_3^- \rightarrow \text{H}^+ + \text{SO}_3^{2-}\]

Sulfurous acid is a weak acid because it does not dissociate completely in water. The equilibrium lies more to the left compared to sulfuric acid, meaning fewer hydrogen ions are released into the solution.

**Comparison:**

- **Sulfuric acid** is a stronger acid than **sulfurous acid** because it dissociates more completely and releases more hydrogen ions into the solution.

Therefore, the statement "\(\text{H}_2\text{SO}_4\) is a stronger acid than \(\text{H}_2\text{SO}_3\)" is **True**.

So, the correct answer is **A. True**.