A 50.0-mL sample of a 1.50 M NaOH solution is titrated with a 2.90 M HCl solution. What will be the final volume (sample + titrant) of solution when the NaOH has been completely neutralized by the HCl?

Question

Chemistry

London Robinson

27 September, 07:02

A 50.0-mL sample of a 1.50 M NaOH solution is titrated with a 2.90 M HCl solution. What will be the final volume (sample + titrant) of solution when the NaOH has been completely neutralized by the HCl?

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Answers (1)

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Deangelo Bright · Answer 1

In order to proceed calculations for a titration process, it is important that we know the reaction involved. For this case, it would be:

HCl + NaOH = NaCl + H2O

To determine the final volume of the sample and the titrant added, we need to know how much of the titrant or the HCl solution was added into the sample. To do this, we use the given values in the problem and the reaction to relate the substances. We do as follows:

1.50 M NaOH (.05 L solution) (1 mol HCl / 1 mol NaOH) = 0.075 mol HCl

0.075 mol HCl / 2.90 M HCl = 0.0259 L HCl solution or 25.9 mL of the HCl solution was added

Therefore, the total volume of the sample and the titrant would be 50.0 + 25.90 = 75.90 mL.