: (a) By titration, 15.0 ml of 0.1008 M sodium hydroxide Problem 106 Chapter 4

Chemistry: A Molecular Approach | 3rd Edition

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Problem 106

Problem106: (a) By titration, 15.0 ml of 0.1008 M sodium hydroxide is needed to neutralize a 0.2053-g sample of a weak acid. What is the molar mass of the acid if it is monoprotic? (b) An elemental analysis of the acid indicates that it is composed of 5.89% H, 70.6% C, and 23.5% O by mass. What is its molecular formula? ?

Step-by-Step Solution:
Step 1 of 3

Solution: Here, we are going to determine the molar mass of the monoprotic acid used. Also, we are going to determine the molecular formula of the acid. Step1: a) Given, molarity of the NaOH solution used = 0.1008 M 15.0 Volume of the NaOH solution used = 15.0 mL = 1000L = 0.015 L Therefore, number of moles of NaOH solution = Volume of solution in litres X Molarity = 0.015 L X 0.1008 M = 0.0015 mol Since, the acid is monoprotic, so 1 mol of NaOH will neutralize 1 mol of the acid Therefore, 0.0015 mol of NaOH will neutralize 0.0015 mol of the acid. Step2: Given mass of the acid sample = 0.2053 g Therefore, molar mass of the acid sample = given mass of the acid / number of moles = 0.2053 g / 0.0015 mol = 136.9 g/mol Thus, molar mass of the acid is 136.9 g/mol. Step3: b) The percentage by mass composition...

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ISBN: 9780321809247

This full solution covers the following key subjects: acid, mass, Molar, elemental, formula. This expansive textbook survival guide covers 82 chapters, and 9464 solutions. Chemistry: A Molecular Approach was written by Sieva Kozinsky and is associated to the ISBN: 9780321809247. Since the solution to 106 from 4 chapter was answered, more than 948 students have viewed the full step-by-step answer. The answer to “Problem106: (a) By titration, 15.0 ml of 0.1008 M sodium hydroxide is needed to neutralize a 0.2053-g sample of a weak acid. What is the molar mass of the acid if it is monoprotic? (b) An elemental analysis of the acid indicates that it is composed of 5.89% H, 70.6% C, and 23.5% O by mass. What is its molecular formula? ?” is broken down into a number of easy to follow steps, and 62 words. This textbook survival guide was created for the textbook: Chemistry: A Molecular Approach, edition: 3rd. The full step-by-step solution to problem: 106 from chapter: 4 was answered by Sieva Kozinsky, our top Chemistry solution expert on 02/22/17, 04:35PM.

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