   Chapter 16, Problem 7ALQ ### Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425

#### Solutions

Chapter
Section ### Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425
Textbook Problem
1 views

# Why is the pH of water at 25 °C equal to 7.00? 6. Consider two separate solutions: one containing a weak acid. HA, and one containing HCI. Assume that you start with 10 molecules of each. a. Draw a molecular-level picture of what each solution looks like. b. Arrange the following from strongest to weakest base: Cl-, H2O, A-. Explain.

Interpretation Introduction

Interpretation:

The pH of level of a solution should be calculated.

Concept Introduction:

The pH of a solution shows the acidity or the basicity of a solution. If the value of pH is low, the solution is said to be acidic and vice versa. pH of a solution is calculated by using the following equation;

pH=log10[H+(aq)]

Usually pH measurements are taken at 250C and a pH value which is less than 7 is considered as acidic, pH value greater than 7 is considered as basic and pH7 is considered as neutral.

Explanation

The pH of a solution can be calculated with the following equation;

pH=log10[H+(aq)]

Water H2O can act as an acid and a base H2O in a solution is in following equilibrium.

H2O(l)H+(aq)+OH(aq)

The dissociation constant (Kw ) for the above reaction can be written as;

Kw=H+(aq)+OH(aq)H2O(l)

At 250C the H2O concentration is =1

Therefore the Kw equation simplifies to Kw=H+(aq)+OH(aq)

The Kw value of the water at 250C is 1×1014. The water dissociates in to H+(aq) and OH(aq) resulting in the same concentrations

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