A standard solution of 0.243 M NaOH was used to determine the concentration of a hydrochloric acid solution. If 46.33 mL of NaOH is needed to neutralize 10.00 mL of the acid, what is the molar concentration of the acid?

Question

Quizplus · Accepted Answer

First, we need to use the balanced chemical equation for the neutralization reaction:

HCl + NaOH → NaCl + H2O

We can see that the mole ratio between NaOH and HCl is 1:1, which means that the moles of NaOH used will be equal to the moles of HCl present in the solution.

Using the concentration and volume of NaOH used, we can calculate the moles of NaOH used:

mol NaOH = concentration × volume = 0.243 M × 0.04633 L = 0.01124 mol

Since the mole ratio is 1:1, the moles of HCl present in the solution will also be 0.01124 mol. We can calculate the molar concentration of the acid solution as follows:

concentration = moles ÷ volume = 0.01124 mol ÷ 0.01000 L = 1.13 M

Therefore, the correct answer is C.

A Standard Solution of 0