1) If you weigh out 0.2349 g of tris, what volume of the 0.1 M HCl solution will you need to reach the end point of this titration? (Note: this is a nice way to get the approximate volume before starting a titration!) 2) If you weighed out 0.4670 g of KHP, what volume of the 0.1 M NaOH solution will you need to reach the end point of this titration?

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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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1) If you weigh out 0.2349 g of tris, what volume of the 0.1 M HCl solution will you need to reach the end point of this titration? (Note: this is a nice way to get the approximate volume before starting a titration!)

2) If you weighed out 0.4670 g of KHP, what volume of the 0.1 M NaOH solution will you need to reach the end point of this titration?
Transcribed Image Text:1) If you weigh out 0.2349 g of tris, what volume of the 0.1 M HCl solution will you need to reach the end point of this titration? (Note: this is a nice way to get the approximate volume before starting a titration!) 2) If you weighed out 0.4670 g of KHP, what volume of the 0.1 M NaOH solution will you need to reach the end point of this titration?
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In the context of analytical chemistry, the process of titration is a fundamental technique used to determine the concentration of a solution (titrand) by reacting it with a solution of known concentration (titrant) until a chemical reaction reaches its endpoint. The information provided in this question pertains to two different titration scenarios, each involving a unique combination of substances and solutions.

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