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What is the pH of a solution formed by mixing 175.0 mL of

Introductory Chemistry | 5th Edition | ISBN: 9780321910295 | Authors: Nivaldo J Tro ISBN: 9780321910295 34

Solution for problem 110P Chapter 14

Introductory Chemistry | 5th Edition

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Introductory Chemistry | 5th Edition | ISBN: 9780321910295 | Authors: Nivaldo J Tro

Introductory Chemistry | 5th Edition

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Problem 110P

What is the pH of a solution formed by mixing 175.0 mL of 0.0880 M HI with 125.0 mL of 0.0570 M KOH?

Step-by-Step Solution:

Problem 110P :

Step 1:

Given :

Volume of HI = 175.0 mL

Molarity of HI = 0.0880 M

Volume of KOH = 125.0 mL

Molarity of KOH = 0.0570 M

pH of solution formed by mixing HI and KOH= ?

Here, HI is a strong acid and KOH is a strong base.

Let’s write the balanced chemical equation for it :

                HI(aq) + KOH(aq) → KI + H2O

First, let’s find the number of moles of HI and KOH :

We have the molarity and volume of HI and KOH, using this we will calculate the number of moles using the molarity formula :

                Molarity =

The formula for calculating the number of moles will be :

Number of moles = Molarity  Volume(in L)   

Volume of HI and KOH is in mL, so let’s convert to L :

1 L = 1000 mL

Therefore, 175 mL HI in L will be :

                = 175 mL

= 0.175 L

125 mL KOH in L will be :

                = 125 mL

= 0.125 L

Hence, number of moles in HI is :

                = 0.0880 M 0.175 L

                = 0.0154 moles.

Number of moles in KOH is :

                =  0.0570 M0.125 L

                = 0.007125 moles.

Now, if we take the difference between [H3O] and [OH] :

 = 0.0154 - 0.007125

 = 0.008275 moles

This tells that there are more [H+] ions in solution. Hence,  it is a acidic solution and there are 0.008275 moles excess in the solution

Step 2 of 2

Chapter 14, Problem 110P is Solved
Textbook: Introductory Chemistry
Edition: 5
Author: Nivaldo J Tro
ISBN: 9780321910295

The full step-by-step solution to problem: 110P from chapter: 14 was answered by , our top Chemistry solution expert on 05/06/17, 06:45PM. Introductory Chemistry was written by and is associated to the ISBN: 9780321910295. The answer to “What is the pH of a solution formed by mixing 175.0 mL of 0.0880 M HI with 125.0 mL of 0.0570 M KOH?” is broken down into a number of easy to follow steps, and 23 words. Since the solution to 110P from 14 chapter was answered, more than 381 students have viewed the full step-by-step answer. This textbook survival guide was created for the textbook: Introductory Chemistry, edition: 5. This full solution covers the following key subjects: formed, koh, mixing, solution. This expansive textbook survival guide covers 19 chapters, and 2045 solutions.

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