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A 50.0 mL solution of Ca(OH)2 with an unknown concentration was titrated with 0.340 M HNO3. To reach the endpoint, a total of 18.8 mL of HNO3 was required. Given that 0.00639 mol of HNO3 are used in the titration, What quantity in moles of Ca(OH)2 had to be present in the initial reaction?

A 50.0 mL solution of Ca(OH)2 with an unknown concentration was titrated with 0.340 M HNO3. To reach the endpoint, a total of 18.8 mL of HNO3 was required. Given that 0.00639 mol of HNO3 are used in the titration, What quantity in moles of Ca(OH)2 had to be present in the initial reaction?

Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter4: Reactions In Aqueous Solution
Section: Chapter Questions
Problem 78QAP: When 85.0 mL of 0.250 M Ba(OH)2 solution is added to 85.00 mL of 0.250 M Al (NO3)3 solution, a white...
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A 50.0 mL solution of Ca(OH)2 with an unknown concentration was titrated with 0.340 M HNO3. To reach the endpoint, a total of 18.8 mL of HNO3 was required. Given that 0.00639 mol of HNO3 are used in the titration, What quantity in moles of Ca(OH)2 had to be present in the initial reaction?
Transcribed Image Text:A 50.0 mL solution of Ca(OH)2 with an unknown concentration was titrated with 0.340 M HNO3. To reach the endpoint, a total of 18.8 mL of HNO3 was required. Given that 0.00639 mol of HNO3 are used in the titration, What quantity in moles of Ca(OH)2 had to be present in the initial reaction?
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