A student uses a gravimetric acid titration to determine the purity of a solid sample containing \(\text{NaHCO}_3\) and an inert impurity. The mass of the sample is \(1.05\text{ g}\). The student adds a solution that is \(3.65\%\) \(\text{HCl}\) by mass until the endpoint is reached. The mass of the solution dispensed is \(10.0\text{ g}\). The reaction is represented by the following equation.

\[ \text{NaHCO}_3\text{(s)}+\text{HCl(aq)}\rightarrow\text{NaCl(aq)}+\text{CO}_2\text{(g)}+\text{H}_2\text{O(l)} \]

Assuming that only \(\text{NaHCO}_3\) reacts with the \(\text{HCl}\), what is the percent by mass of \(\text{NaHCO}_3\) in the sample?