   Chapter 16, Problem 16.103QP General Chemistry - Standalone boo...

11th Edition
Steven D. Gammon + 7 others
ISBN: 9781305580343

Solutions

Chapter
Section General Chemistry - Standalone boo...

11th Edition
Steven D. Gammon + 7 others
ISBN: 9781305580343
Textbook Problem

An artificial fruit beverage contains 11.0 g of tartaric acid, H2C4H4O6, and 20.0 g of its salt, potassium hydrogen tartrate, per liter. What is the pH of the beverage? Ka1 = 1.0× 10−3.

Interpretation Introduction

Interpretation:

The pH of the given artificial fruit beverage containing 11.0 g of tartaric acid and 20.0 g of its salt, potassium hydrogen tartarate has to be calculated

Concept Introdution:

pH definition:

The pH of a solution is defined as the negative base-10 logarithm of the hydronium ion [H3O+] concentration.

pH=-log[H3O+]

Explanation

To Calculate: The pH of the given artificial fruit beverage containing 11.0 g of tartaric acid and 20.0 g of its salt, potassium hydrogen tartarate

Given data:

An artificial fruit beverage contains 11.0 g of tartaric acid and 20.0 g of its salt, potassium hydrogen tartarate per liter

The Ka1 value is 1.0×103

pH calculation:

Let us represent tartaric acid as (H2Tar) and hydrogen tartarate ion as (HTar)

The initial concentration of tartaric acid is calculated from 11.0 g of tartaric acid:

Initial conc. of tartaric acid =11.0 g H2Tar150.1 g/mol1.00 L =0.07328 M H2Tar

The initial concentration of tartarate ion is calculated from 20.0 g of potassium hydrogen tartarate:

Initial conc. of tartarate ion =20.0 g KHTar-188.2 g/mol1.00 L =0.1063 M [HTar]

Construct an equilibrium table for the hydrolysis of tartaric acid:

 H2Tar     +   H2O ⇌   H3O+     +     HTar− Initial (M) 0.07328 −x 0

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