A chemistry student needs to standardize a fresh solution of sodium hydroxide. He carefully weighs out 143.mg of oxalic acid H2C2O4, a diprotic acid that can be purchased inexpensively in high purity and dissolves it in 250.mL of distilled water. The student then titrates the oxalic acid solution with his sodium hydroxide solution. When the titration reaches the equivalence point, the student finds he has used 55.7mL of sodium hydroxide solution. Calculate the molarity of the student's sodium hydroxide solution. Round your answer to 3 significant digits.
A chemistry student needs to standardize a fresh solution of sodium hydroxide. He carefully weighs out 143.mg of oxalic acid H2C2O4, a diprotic acid that can be purchased inexpensively in high purity and dissolves it in 250.mL of distilled water. The student then titrates the oxalic acid solution with his sodium hydroxide solution. When the titration reaches the equivalence point, the student finds he has used 55.7mL of sodium hydroxide solution. Calculate the molarity of the student's sodium hydroxide solution. Round your answer to 3 significant digits.
Chapter15: Acid-base Equilibria
Section: Chapter Questions
Problem 96AE: One method for determining the purity of aspirin (C9H8O4) is to hydrolyze it with NaOH solution and...
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A chemistry student needs to standardize a fresh solution of sodium hydroxide. He carefully weighs out 143.mg of oxalic acid H2C2O4, a diprotic acid that can be purchased inexpensively in high purity and dissolves it in 250.mL of distilled water. The student then titrates the oxalic acid solution with his sodium hydroxide solution. When the titration reaches the equivalence point, the student finds he has used 55.7mL of sodium hydroxide solution. Calculate the molarity of the student's sodium hydroxide solution. Round your answer to 3 significant digits.
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