Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 17: Problem 65

The buffer range is defined by the equation \(\mathrm{pH}=\) \(\mathrm{p} K_{\mathrm{a}} \pm 1 .\) Calculate the range of the ratio [conjugate base \(]\) / [acid] that corresponds to this equation.

Short Answer

Expert verified
The buffer range, defined by pH = pKa ± 1, corresponds to a [conjugate base]/[acid] ratio between 0.1 and 10.

Step by step solution

01

Understanding the Buffer Range

The buffer range is defined by the equation pH = pKa ± 1. This equation is derived from the Henderson Hasselbalch equation, which is pH = pKa + log([conjugate base]/[acid]). In this range, pH varies by one unit from the pKa value. We are aiming to find the [conjugate base]/[acid] ratio that corresponds to this buffer range.
02

Solving For Lower Bound

First, we solve for the lower boundary of our buffer range where pH = pKa - 1. Substituting this into the Henderson Hasselbalch equation gives us pKa - 1 = pKa + log([conjugate base]/[acid]), which simplifies to -1 = log([conjugate base]/[acid]). Using the inverse of the logarithm function, we find that [conjugate base]/[acid] = 10^(-1) = 0.1.
03

Solving for Upper Bound

Next, we solve for the upper boundary of our buffer range where pH = pKa + 1. Substituting this into the Henderson Hasselbalch equation we get pKa + 1 = pKa + log([conjugate base]/[acid]), which simplifies to 1 = log([conjugate base]/[acid]). Using the inverse of the logarithm function, we find that [conjugate base]/[acid] = 10^(1) = 10.
04

Determining the Buffer Range

We have found the minimum and maximum [conjugate base]/[acid] ratio that corresponds to the buffer range where pH = pKa ± 1. The buffer range is thus when [conjugate base]/[acid] is between 0.1 and 10.

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

A 5.00 -g quantity of a diprotic acid is dissolved in water and made up to exactly \(250 \mathrm{~mL}\). Calculate the molar mass of the acid if \(25.0 \mathrm{~mL}\) of this solution required \(11.1 \mathrm{~mL}\) of \(1.00 \mathrm{M} \mathrm{KOH}\) for neutralization. Assume that both protons of the acid are titrated.

The \(\mathrm{p} K_{\mathrm{a}}\) of butyric acid (HBut) is 4.7 . Calculate \(K_{\mathrm{b}}\) for the butyrate ion (But \(^{-}\) ).

Calculate the \(\mathrm{pH}\) of the \(0.20 \mathrm{M} \mathrm{NH}_{3} / 0.20 \mathrm{M} \mathrm{NH}_{4} \mathrm{Cl}\) buffer. What is the \(\mathrm{pH}\) of the buffer after the addition of \(10.0 \mathrm{~mL}\) of \(0.10 \mathrm{M} \mathrm{HCl}\) to \(65.0 \mathrm{~mL}\) of the buffer?

Write the formation constant expressions for these complex ions: (a) \(\mathrm{Zn}(\mathrm{OH})_{4}^{2-},\) (b) \(\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}^{3+}\) (c) \(\mathrm{HgI}_{4}^{2-}\).

The solubility product of \(\mathrm{PbBr}_{2}\) is \(8.9 \times 10^{-6} .\) Determine the molar solubility (a) in pure water, (b) in \(0.20 M\) KBr solution, (c) in \(0.20 \mathrm{M} \mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}\) solution.
See all solutions

Recommended explanations on Chemistry Textbooks

The Earths Atmosphere

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Chemical Reactions

Read Explanation

Chemistry Branches

Read Explanation

Chemical Analysis

Read Explanation

Inorganic Chemistry

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