What volume of 5.00 × 10^-3 M HNO₃ is needed to titrate 20.00 mL of 5.00 × 10^-3 M Ca(OH)₂ to the equivalence point? A) 2.50 mL B) 10.0 mL C) 20.0 mL D) 40.0 mL E) 180. mL

Question

Quizplus · Accepted Answer

The reaction between $ HNO_3 $ and $ Ca(OH)_2 $ can be represented by the balanced chemical equation: $ 2HNO_3 + Ca(OH)_2 \rightarrow Ca(NO_3)_2 + 2H_2O $. This shows that 2 moles of $ HNO_3 $ are needed to neutralize 1 mole of $ Ca(OH)_2 $. Given both solutions have the same molarity ( $ 5.00 \times 10^{-3} $ M), and we have 20.00 mL of $ Ca(OH)_2 $, we need twice the volume of $ HNO_3 $ to reach the equivalence point, hence 40.0 mL.

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