Tartaric acid, H2C4H4O6, has two acidic hydrogens. The acid is often present in

Question

Tartaric acid, H2C4H4O6, has two acidic hydrogens. The acid is often present in wines and precipitates from solution as the wine ages. The neutralization reaction of tartaric is as follows: H2C4H4O6(aq)+2NaOH(aq)Na2C4H4O6(aq)+2H2O(l) A solution containing an unknown concentration of the acid is titrated with NaOH. It requires 21.65 mL of 0.2000 M NaOH solution to titrate both acidic protons in 50.00 mL of the tartaric acid solution.

Part A Calculate the molarity of the tartaric acid solution.

Express your answer using four significant figures.

Explanation / Answer

moles of OH- = .2000 x 21.65 / 1000 = 0.008977 moles

moles of tartaric acid at the eq point = 0.0089775 / 2 = 4.83*10^-3 moles

these moles are in 50 mL so moles per liter = 4.83*10^-3 x1000/ 50 = 0.0966M

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