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A 0.704 g of a pure acid, HA, is dissolved in water and an acid-base indicator...

A 0.704 g of a pure acid, HA, is dissolved in water and an acid-base indicator added. The solution requires 33.78 mL of 0.256 M NaOH solution to reach the end point. What is the molar mass of the acid? HA(aq) + NaOH(aq) LaTeX: \longrightarrow⟶ NaA(aq) + H2O(aq)

Group of answer choices

81.4 g/mol

199 g/mol

145 g/mol

20.0 g/mol

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