I need help understanding what exactly I need to do to work this problem out. Pl

Question

I need help understanding what exactly I need to do to work this problem out. Please don't just give me the answer but explain the steps you got to get the answer.

Lemon juice has a pH of about 2.5. Assuming that the acidity of lemon juice is due solely to citric acid, that citric acid is a monoprotic acid, and that the density of lemon juice is 1.0 g/mL, then the citric acid concentration calculates to 0.5% by mass. Estimate the volume of 0.0100 M NaOH required to neutralize a 3.71-g sample of lemon juice. The molar mass of citric acid is 190.12 g/mol.

Explanation / Answer

given :

density of lemon juice is 1.0 g/mL

lemon juice has a pH of about 2.5

citric acid concentration calculates to 0.5% by mass

molar mass of citric acid is 190.12 g/mol

concentration of NaOH = 0.0100 M

mass citric acid = 0.5 x 3.71 / 100 =0.01855 g
moles = 0.01855 g / 190.12 g/mol = 9.76 x 10-5 mol of citric acid

= moles NaOH
V = 9.76 x 10-5 mol of citric acid / 0.0100 M of NaOH = 0.00976 L = 9.76 mL

9.76 ml of 0.0100 M NaOH required to neutralize a 3.71g sample of lemon juice

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