Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 15: Problem 51

Consider the titration of \(40.0 \mathrm{~mL}\) of \(0.200 \mathrm{M} \mathrm{HClO}_{4}\) by \(0.100\) \(M\) KOH. Calculate the \(\mathrm{pH}\) of the resulting solution after the following volumes of KOH have been added. a. \(0.0 \mathrm{~mL}\) d. \(80.0 \mathrm{~mL}\) b. \(10.0 \mathrm{~mL}\) e. \(100.0 \mathrm{~mL}\) c. \(40.0 \mathrm{~mL}\)

Short Answer

Expert verified
The pH values for the given volumes of KOH are as follows: a. \(0.0 \mathrm{~mL}\): pH = 0.70 b. \(10.0 \mathrm{~mL}\): pH = 1.30 c. \(40.0 \mathrm{~mL}\): pH = 7.00 d. \(80.0 \mathrm{~mL}\): pH = 13.07 e. \(100.0 \mathrm{~mL}\): pH = 13.52

Step by step solution

01

Calculate the initial moles of HClO4

Firstly, we need to determine the initial number of moles of HClO4 in the solution. The moles of a substance can be calculated using the formula: moles = concentration × volume. Here, the concentration of HClO4 is 0.200M and the volume is 40.0 mL (which we'll convert to L by dividing by 1000). Initial moles of HClO4 = (0.200 mol/L) × (40.0 mL ÷ 1000) = 0.008 mol
02

Calculate the moles of KOH added

For each volume of KOH, we need to calculate the moles of KOH added to the solution. The moles of KOH can be calculated using the formula: moles = concentration × volume. Here, the concentration of KOH is 0.100M. We will do this step for each of the given volumes: a. 0.0 mL b. 10.0 mL c. 40.0 mL d. 80.0 mL e. 100.0 mL
03

Balance the moles of acid and base

For each case, we need to find the difference between the moles of HClO4 and the moles of KOH added, to determine the remaining moles of acid or base in the solution. For each volume, calculate the remaining moles of HClO4 and KOH: Remaining moles of HClO4 = Initial moles of HClO4 - Moles of KOH added
04

Calculate the new concentration of acid or base

Now we need to calculate the new concentration of HClO4 or OH- ions in the solution after the addition of the respective volumes of KOH. New concentration = (Remaining moles of HClO4 or OH-) ÷ (Initial volume of HClO4 + Added volume of KOH) Calculate the new concentration for each case.
05

Calculate the pH of the solution

Finally, we will use the new concentrations of HClO4 or OH- ions to calculate the pH of the solution in each case. If HClO4 is present in excess, we can calculate the pH directly using: pH = -log10([HClO4]) If OH- ions are in excess, we can calculate the pOH first: pOH = -log10([OH-]) And then, convert it to pH using the formula: pH = 14 - pOH Find the pH for each case. Please note that the steps to calculate pH may require additional steps in some cases. OnTriggerEnterRestBoundary_Error, but this approach should suffice for this exercise.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Methyl red has the following structure: CN(C)c1ccc(N=Nc2ccccc2C(=O)O)cc1 It undergoes a color change from red to yellow as a solution gets more basic. Calculate an approximate \(\mathrm{pH}\) range for which methyl red is useful. What is the color change and the \(\mathrm{pH}\) at the color change when a weak acid is titrated with a strong base using methyl red as an indicator? What is the color change and the \(\mathrm{pH}\) at the color change when a weak base is titrated with a strong acid using methyl red as an indicator? For which of these two types of titrations is methyl red a possible indicator?

Amino acids are the building blocks for all proteins in our bodies. A structure for the amino acid alanine is All amino acids have at least two functional groups with acidic or basic properties. In alanine, the carboxylic acid group has \(K_{\mathrm{a}}=4.5 \times 10^{-3}\) and the amino group has \(K_{\mathrm{b}}=7.4 \times 10^{-5} .\) Because of the two groups with acidic or basic properties, three different charged ions of alanine are possible when alanine is dissolved in water. Which of these ions would predominate in a solution with \(\left[\mathrm{H}^{+}\right]=1.0 M ?\) In a solution with \(\left[\mathrm{OH}^{-}\right]=\) \(1.0 M ?\)

A certain indicator HIn has a \(\mathrm{p} K_{2}\) of \(3.00\) and a color change becomes visible when \(7.00 \%\) of the indicator has been converted to \(\mathrm{In}^{-}\). At what \(\mathrm{pH}\) is this color change visible?

Calculate the volume of \(1.50 \times 10^{-2} \mathrm{M} \mathrm{NaOH}\) that must be added to \(500.0 \mathrm{~mL}\) of \(0.200 \mathrm{M} \mathrm{HCl}\) to give a solution that has \(\mathrm{pH}=2.15\)

In the titration of \(50.0 \mathrm{~mL}\) of \(1.0 \mathrm{M}\) methylamine, \(\mathrm{CH}_{3} \mathrm{NH}_{2}\) \(\left(K_{\mathrm{b}}=4.4 \times 10^{-4}\right)\), with \(0.50 \mathrm{M} \mathrm{HCl}\), calculate the \(\mathrm{pH}\) under the following conditions. a. after \(50.0 \mathrm{~mL}\) of \(0.50 \mathrm{M} \mathrm{HCl}\) has been added b. at the stoichiometric point
See all solutions

Recommended explanations on Chemistry Textbooks

Inorganic Chemistry

Read Explanation

Making Measurements

Read Explanation

Organic Chemistry

Read Explanation

Chemical Analysis

Read Explanation

The Earths Atmosphere

Read Explanation

Chemistry Branches

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free