AP Chemistry
4.6 Introduction to Titration
4.5 Stoichiometry
A student titrates a 20.0 mL sample of a diprotic acid solution, \(\text{H}_2\text{A(aq)}\), with a standardized \(0.100 \text{ M NaOH(aq)}\) solution using phenolphthalein as an indicator. The net ionic equation for the reaction that occurs during the titration is shown below.
\[\text{H}_2\text{A(aq)} + 2\text{OH}^-\text{(aq)} \rightarrow \text{A}^{2-}\text{(aq)} + 2\text{H}_2\text{O(l)}\]
The initial buret reading of \(0.100 \text{ M NaOH(aq)}\) is 5.00 mL. At the pale pink endpoint, the final buret reading is 45.00 mL. What is the molarity of the \(\text{H}_2\text{A(aq)}\) sample?
\[\text{H}_2\text{A(aq)} + 2\text{OH}^-\text{(aq)} \rightarrow \text{A}^{2-}\text{(aq)} + 2\text{H}_2\text{O(l)}\]
The initial buret reading of \(0.100 \text{ M NaOH(aq)}\) is 5.00 mL. At the pale pink endpoint, the final buret reading is 45.00 mL. What is the molarity of the \(\text{H}_2\text{A(aq)}\) sample?
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