Achemistry student weighs out 0.306 g of citric acid (h3c6h5o7), a triprotic acid, into a 250 ml volumetric flask and dilutes to the mark with distilled water. he plans to titrate the acid with 0.1000 m naoh solution. calculate the volume of naoh solution the student will need to add to reach the final equivalence point. be sure your answer has the correct number of significant digits.

The volume of NaOH solution is "47.8 mL".

Given values are:

Concentration of NaOH ,

Mass,

The equation,

→

Now,

→ The moles of will be:

=

=

=

→ Moles of NaOH will be:

=

=

=

hence,

→ The volume of NaOH will be:

=

=

=

or,

=

Thus the above response is right.

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Explanation:

For simplicity, let's write the formula of citric acid as H₃A.

1. Balanced chemical equation.

2. Moles of H₃A

3. Moles of NaOH.

4. Volume of NaOH