AP Chemistry
4.6 Introduction to Titration
4.5 Stoichiometry
A student titrates a \(25.0 \text{ mL}\) sample of an unknown diprotic acid, \(\text{H}_2\text{A(aq)}\), with a standardized \(0.200 \text{ M } \text{NaOH(aq)}\) solution according to the balanced equation below:
\[\text{H}_2\text{A(aq)} + 2\,\text{NaOH(aq)} \rightarrow \text{Na}_2\text{A(aq)} + 2\,\text{H}_2\text{O(l)}\]
The student reaches the second equivalence point after adding exactly \(30.0 \text{ mL}\) of the \(\text{NaOH(aq)}\) titrant. What is the molar concentration of the \(\text{H}_2\text{A(aq)}\) solution?
\[\text{H}_2\text{A(aq)} + 2\,\text{NaOH(aq)} \rightarrow \text{Na}_2\text{A(aq)} + 2\,\text{H}_2\text{O(l)}\]
The student reaches the second equivalence point after adding exactly \(30.0 \text{ mL}\) of the \(\text{NaOH(aq)}\) titrant. What is the molar concentration of the \(\text{H}_2\text{A(aq)}\) solution?
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