Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 17: Problem 19

Which of the following solutions is a buffer? (a) 0.10\(M\) \(\mathrm{CH}_{3} \mathrm{COOH}\) and \(0.10 \mathrm{MCH}_{3} \mathrm{CONa},(\mathbf{b}) 0.10 \mathrm{MCH}_{3} \mathrm{COOH}\) (c) 0.10 \(\mathrm{M} \mathrm{HCl}\) and \(0.10 \mathrm{M} \mathrm{NaCl},(\mathbf{d})\) both a and \(\mathrm{c},(\mathbf{e})\) all of a, \(\mathrm{b},\) and \(\mathrm{c} .\)

Short Answer

Expert verified
The correct answer is (a) 0.10 M CH3COOH and 0.10 M CH3COONa, as it consists of a weak acid (acetic acid) and its conjugate base (acetate).

Step by step solution

01

Identify the components of each solution

In the given exercise, we are given the following solutions: (a) 0.10 M CH3COOH and 0.10 M CH3COONa (b) 0.10 M CH3COOH (c) 0.10 M HCl and 0.10 M NaCl (d) Both a and c (e) All of a, b, and c We now need to identify the components of each solution and determine if they can form a buffer.
02

Analyze the solutions

(a) 0.10 M CH3COOH (acetic acid) and 0.10 M CH3COONa (sodium acetate): In this solution, CH3COOH is a weak acid and CH3COO- (from the dissociation of CH3COONa) is its conjugate base. Thus, this solution can act as a buffer. (b) 0.10 M CH3COOH (acetic acid): In this solution, there is only a weak acid present, and no conjugate base is available. Therefore, this solution cannot act as a buffer. (c) 0.10 M HCl (hydrochloric acid) and 0.10 M NaCl (sodium chloride): In this solution, HCl is a strong acid and completely dissociates into H+ and Cl-. Since HCl is not a weak acid, this solution cannot be a buffer.
03

Choose the correct answer

Based on our analysis in step 2, we can conclude that: (a) is a buffer (b) is not a buffer (c) is not a buffer Thus, the correct answer is (a) 0.10 M CH3COOH and 0.10 M CH3COONa.

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) Calculate the percent ionization of 0.0075\(M\) butanoic acid \(\left(K_{a}=1.5 \times 10^{-5}\right) .\) (b) Calculate the percent ionization of 0.0075\(M\) butanoic acid in a solution containing 0.085\(M\) sodium butanoate.

A sample of 7.5 \(\mathrm{L}\) of \(\mathrm{NH}_{3}\) gas at \(22^{\circ} \mathrm{C}\) and 735 torr is bubbled into a 0.50 -L solution of 0.40 \(\mathrm{M}\) HCl. Assuming that all the \(\mathrm{NH}_{3}\) dissolves and that the volume of the solution remains \(0.50 \mathrm{L},\) calculate the \(\mathrm{pH}\) of the resulting solution.

Rainwater is acidic because \(\mathrm{CO}_{2}(\mathrm{g})\) dissolves in the water, creating carbonic acid, \(\mathrm{H}_{2} \mathrm{CO}_{3}\) . If the rainwater is too acidic, it will react with limestone and seashells (which are principally made of calcium carbonate, CaCO_ \(_{3} ) .\) Calculate the concentrations of carbonic acid, bicarbonate ion \(\left(\mathrm{HCO}_{3}^{-}\right)\) and carbonate ion \(\left(\mathrm{CO}_{3}^{2-}\right)\) that are in a raindrop that has a pH of 5.60 , assuming that the sum of all three species in the raindrop is \(1.0 \times 10^{-5} M .\)

A solution containing several metal ions is treated with dilute HCl; no precipitate forms. The \(\mathrm{pH}\) is adjusted to about \(1,\) and \(\mathrm{H}_{2} \mathrm{S}\) is bubbled through. Again, no precipitate forms. The \(\mathrm{pH}\) of the solution is then adjusted to about \(8 .\) Again, \(\mathrm{H}_{2} \mathrm{S}\) is bubbled through. This time a precipitate forms. The filtrate from this solution is treated with \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{HPO}_{4} .\) No precipitate forms. Which of these metal cations are either possibly present or definitely absent: \(\mathrm{Al}^{3+}, \mathrm{Na}^{+}, \mathrm{Ag}^{+}, \mathrm{Mg}^{2+} ?\)

You have to prepare a pH \(=3.50\) buffer, and you have the following 0.10\(M\) solutions available: \(\mathrm{HCOOH}, \mathrm{CH}_{3} \mathrm{COOH}\) , \(\mathrm{H}_{3} \mathrm{PO}_{4}, \mathrm{HCOONa}, \mathrm{CH}_{3} \mathrm{COONa}\) , and \(\mathrm{NaH}_{2} \mathrm{PO}_{4} .\) Which solutions would you use? How many milliliters of each solution would you use to make approximately 1 L of the buffer?
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Reactions

Read Explanation

Organic Chemistry

Read Explanation

Inorganic Chemistry

Read Explanation

The Earths Atmosphere

Read Explanation

Nuclear Chemistry

Read Explanation

Making Measurements

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