Question

1. A sample of hydrochloric acid is standardized using sodium bicarbonate. a. Write the balanced chemical...

1. A sample of hydrochloric acid is standardized using sodium bicarbonate.

a. Write the balanced chemical equation for the reaction of hydrochloric acid with sodium bicarbonate, NaHCO3

b. Calculate the molar concentration of the hydrochloric acid if 35.18 mL of hydrochloric acid was required to neutralize 0.450 g of sodium bicarbonate to a phenolphthalein end point.

c. Calculate the mass percent concentration of hydrochloric acid using the molar concentration calculated in part b and assuming the density of the solution is 1.01 g/mL

2. Malonic acid, H2C3H2O4, is a diprotic acid, so 2 moles of hydroxide ions are required per mole of malonic acid for complete neutralization.

a. Write the balanced chemical equation for the reaction of the malonic acid with potassium hydroxide.

b. Calculate the molar concentration of the malonic acid if 38.17 mL of 0.315 M potassium hydroxide was required to neutralize 25.0 mL of molanic acid to a phenolphthalein end point.

c. Calculate the mass percent concentration of molanic acid using molar concentration calculated in part b and assuming the density of the solution is 1.01 g/mL

3. Citric acid is a tripotic acid, so 3 moles of hydroxide ions are required per mole of citric acid for complete neutralization.

a. Write the balanced chemical equation for the reaction of citric acid with sodium hydroxide. (Note that citrate ion is actually a polyatomic ion with carbon, hydrogen, and oxygen atoms and an overall charge of -3. For now, please express citrate ion as Cit^3-)

b. If 36.10 mL of 0.223 M NaOH is used to neutralize a 0.515 g sample of citric acid, what is the molar mass of the acid?

Homework Answers

Answer #1

1. A sample of hydrochloric acid is standardized using sodium bicarbonate.

a. Write the balanced chemical equation for the reaction of hydrochloric acid with sodium bicarbonate, NaHCO3

NAHCO3 + HCl = NACl + H2O + CO2

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b. Calculate the molar concentration of the hydrochloric acid if 35.18 mL of hydrochloric acid was required to neutralize 0.450 g of sodium bicarbonate to a phenolphthalein end point.

(0.450 g NAHCO3) / (84.007 g NAHCO3/mol) x (1 mol HCl / 1 mol NAHCO3) / (0.03518 L) = 0.152mol/L HCl

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