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A student weights out 1.118g of impure KHP, dissolves the sample in deionized water and titrate it with 0.1001 M NaOH solution. If the titration requires 27.10 mL of the NaOH solution, and none of the impurities react with NaOH, what is the percent KHP in the sample?

A student weights out 1.118g of impure KHP, dissolves the sample in deionized water and titrate it with 0.1001 M NaOH solution. If the titration requires 27.10 mL of the NaOH solution, and none of the impurities react with NaOH, what is the percent KHP in the sample?

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Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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A student weights out 1.118g of impure KHP, dissolves the sample in deionized water and titrate it with 0.1001 M NaOH solution. If the titration requires 27.10 mL of the NaOH solution, and none of the impurities react with NaOH, what is the percent KHP in the sample?
**Problem: Determining Percent Purity of KHP in a Sample** A student weighs out 1.118 g of impure KHP (Potassium Hydrogen Phthalate), dissolves the sample in deionized water, and titrates with 0.1001 M NaOH solution. If the titration requires 21.10 mL of the NaOH solution, and none of the impurities react with NaOH, what is the percent KHP in the sample? **Calculation Approach:** To solve this problem, follow these steps: 1. **Calculate Moles of NaOH Used:** - Use the molarity and volume of NaOH solution to find the moles of NaOH used in the reaction. 2. **Relate Moles of NaOH to Moles of KHP:** - Based on the reaction stoichiometry, equate moles of NaOH to moles of KHP. 3. **Calculate the Mass of Pure KHP:** - Convert moles of KHP to mass using the molar mass of KHP (204.22 g/mol). 4. **Determine Percent Purity:** - Use the calculated mass of pure KHP to find the percent purity in the original impure sample. This calculation determines the purity level and ensures accurate quantitative analysis in experimental procedures.
Transcribed Image Text:**Problem: Determining Percent Purity of KHP in a Sample** A student weighs out 1.118 g of impure KHP (Potassium Hydrogen Phthalate), dissolves the sample in deionized water, and titrates with 0.1001 M NaOH solution. If the titration requires 21.10 mL of the NaOH solution, and none of the impurities react with NaOH, what is the percent KHP in the sample? **Calculation Approach:** To solve this problem, follow these steps: 1. **Calculate Moles of NaOH Used:** - Use the molarity and volume of NaOH solution to find the moles of NaOH used in the reaction. 2. **Relate Moles of NaOH to Moles of KHP:** - Based on the reaction stoichiometry, equate moles of NaOH to moles of KHP. 3. **Calculate the Mass of Pure KHP:** - Convert moles of KHP to mass using the molar mass of KHP (204.22 g/mol). 4. **Determine Percent Purity:** - Use the calculated mass of pure KHP to find the percent purity in the original impure sample. This calculation determines the purity level and ensures accurate quantitative analysis in experimental procedures.
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