A solid sample containing a simple mixture of NaHSO3 and Na2SO3 was dissolved in distilled water and titrated with a standard HCl solution. 13.88 mL was required to reach the first stoichiometric point, and an additional 45.12 mL to reach the second. What was the mass percentage of Na2SO3 present in the original sample?

Question

A solid sample containing a simple mixture of NaHSO3 and Na2SO3 was dissolved in distilled water and titrated with a standard HCl solution. 13.88 mL was required to reach the first stoichiometric point, and an additional 45.12 mL to reach the second. What was the mass percentage of Na2SO3 present in the original sample?

Answer 1

To find the mass percentage of Na2SO3 in the sample, we need to determine the number of moles of Na2SO3 and NaHSO3 present and calculate the mass percentage based on that information.

Here's how we can approach this problem step by step:

Step 1: Calculate the number of moles of HCl used in the titration for each stoichiometric point.
Given that 13.88 mL of HCl is required to reach the first stoichiometric point and an additional 45.12 mL to reach the second, we can find the total volume of HCl used by summing these two values: 13.88 mL + 45.12 mL = 59 mL.

Since HCl is a strong acid and reacts in a 1:1 ratio with both NaHSO3 and Na2SO3, we can assume that the number of moles of HCl used is equal to the number of moles of Na2SO3 and NaHSO3 present in the sample.

Step 2: Calculate the molarity of the HCl solution.
To find the molarity of the HCl solution, we need additional information: the concentration of the HCl solution. Without this information, we cannot proceed further to calculate the mass percentage.

Please provide any additional information about the concentration of the HCl solution so that we can continue with the calculation.