A 5.296 g sample of a solid, weak, monoprotic acid is used to make a 100.0 mL solution. 30.00 mL of the resulting acid solution is then titrated with 0.09755 M NaOH. The pH after the addition of 21.00 mL of the base is 5.02, and the endpoint is reached after the addition of 46.38 mL of the base. (a) How many moles of acid were present in the 30.00 mL sample? 0.004524 mol
A 5.296 g sample of a solid, weak, monoprotic acid is used to make a 100.0 mL solution. 30.00 mL of the resulting acid solution is then titrated with 0.09755 M NaOH. The pH after the addition of 21.00 mL of the base is 5.02, and the endpoint is reached after the addition of 46.38 mL of the base. (a) How many moles of acid were present in the 30.00 mL sample? 0.004524 mol
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
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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A 5.296 g sample of a solid, weak, monoprotic acid is used to make a 100.0 mL solution. 30.00 mL of the resulting acid solution is then titrated with 0.09755 M NaOH. The pH after the addition of 21.00 mL of the base is 5.02, and the endpoint is reached after the addition of 46.38 mL of the base.
(a) How many moles of acid were present in the 30.00 mL sample?
0.004524 mol
(b) What is the molar mass of the acid?
351.1 g/mol
(c) What is the pKa of the acid?
0.004524 mol
(b) What is the molar mass of the acid?
351.1 g/mol
(c) What is the pKa of the acid?
just need help with part C
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