   Chapter 15, Problem 15.127QP 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

A solution contains 4.25g of ammonia per 250.0 mL of solution. Electrical conductivity measurements at 25°C show that 0.42% of the ammonia has reacted with water. Write the equation for this reaction and calculate the pH of the solution.

Interpretation Introduction

Interpretation:

The equation for the given information has to be written and the pH of the given solution has to be calculated.

Concept introduction:

pH is an logarithmic expression to express a solution is acidic, basic or neutral.  pH scale lies values between 1-14 and on which 7 is neutral, below 7 values are more acidic in nature and above 7 values are more basic in nature.

Total pH of a solution is pH + pOH = 14

Explanation

From the given information,

Ammonia reacts with water to produce ammonium ion and hydroxide ion and the reaction equation can be written as follows.

NH3(aq) + H2O(l) NH4+(aq) + OH-(aq)

To calculate pH of the given solution, first we have to calculate the molarity of initial concentration of ammonia is as follows.

We know that, molar mass of ammonia is 17.03g/mol.

Now,

Molarity = 4.25gNH3×1molNH317

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