A solution is prepared by adding 49.7 mL concentrated hydrochloric acid and 19.1 mL concentrated nitric acid to 300 mL water. More water is added untilthe final volume is 1.00 L. Calculate,, and the pH for this solution. [Hint: Concentrated is 38% (by mass) and has a density of 1.19 ; concentrated is70.% (by mass) and has a density of 1.42 .]MMpH =%3D

Answered: the final volume is 1.00 L. Calculate,,…

the final volume is 1.00 L. Calculate,, and the pH for this solution. [Hint: Concentrated is 38% (by mass) and has a density of 1.19 ; concentr. 70.% (by mass) and has a density of 1.42 .]

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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Question

A solution is prepared by adding 49.7 mL concentrated hydrochloric acid and 19.1 mL concentrated nitric acid to 300 mL water. More water is added until
the final volume is 1.00 L. Calculate,, and the pH for this solution. [Hint: Concentrated is 38% (by mass) and has a density of 1.19 ; concentrated is
70.% (by mass) and has a density of 1.42 .]
M
M
pH =
%3D

Expert Solution

Step 1

We are given 49.7mL HCl, 19.1mL nitric acid added in water to make 1 L solution

We have to find pH of the solution

Given HCl is 38% by mass, density = 1.19g/mL

Nitric acid is 70% by mass, density = 1.42g/ml

Step by step

Solved in 3 steps with 2 images

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