Question

Following the procedure for this experiment, a student titrated 20.0 mL of grapefruit juice with 0.1030 M NaOH. The initial buret reading was 0.13 mL, and the final buret reading was 10.76 mL.

A. Calculate the volume, in milliliters, of NaOH solutions required for the titration.

B. Calculate the number of moles of NaOH required for the titration.

C. Calculate the number of moles of H₃C₆H₅O₇ titrated.

D. Calculate the mass of H₃C₆H₅O₇ present in the juice sample.

E. Calculate the mass of H₃C₆H₅O₇ present in 1.0 mL of the juice.

Answer 1

Calculate the volume, in milliliters, of NaOH solutions required for the titration.

A. volume of NaOH = final - initial volume = 10.76 - 0.13 = 10.63 mL

M = moles/volume

B. moles of NaOH = M* volume = 0.1030*0.01063 = 0.00109 moles.

C. citric acid = 3 times moles of NaOH = 3*0.00109 = 0.00327 moles of citric acid

D. mass of citric acid = moles * molarmass =0.00327*192 = 0.628 g

E.20.0 ml of citric acid mass = 0.628 g then 1.0 mL of citric acid mass = 0.628/20 = 0.0314 g