Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 15: Problem 32

Calculate the \(\mathrm{pH}\) of a solution that is \(0.60 \mathrm{M} \mathrm{HF}\) and \(1.00 M \mathrm{KF}\).

Short Answer

Expert verified
The pH of the solution that is 0.60 M HF and 1.00 M KF is approximately 3.40.

Step by step solution

01

Find the pKa value for HF

Use the formula: \( pKa = -\log{Ka} \) Using the given Ka value for HF: \( pKa = -\log{(6.6 × 10^{-4})} \) Calculating the pKa value: \( pKa \approx 3.18 \)
02

Apply the Henderson-Hasselbalch equation

Use the formula: \( pH = pKa + \log{\frac{[A^-]}{[HA]}} \) Substitute the values we found in step 1 and the given concentrations: \( pH = 3.18 + \log{\frac{1.00}{0.60}} \) Simplify and calculate the pH value: \( pH = 3.18 + \log{1.67} \) \( pH \approx 3.18 + 0.22 \) \( pH \approx 3.40 \) So, the pH of the solution that is 0.60 M HF and 1.00 M KF is approximately 3.40.

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

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 \(\left[\mathrm{OH}^{-}\right]=1.0 M ?\)

Which of the following mixtures would result in a buffered solution when \(1.0 \mathrm{~L}\) of each of the two solutions are mixed? a. \(0.2 \mathrm{M} \mathrm{HNO}_{3}\) and \(0.4 \mathrm{M} \mathrm{NaNO}_{3}\) b. \(0.2 \mathrm{M} \mathrm{HNO}_{3}\) and \(0.4 \mathrm{M} \mathrm{HF}\) c. \(0.2 \mathrm{M} \mathrm{HNO}_{3}\) and \(0.4 M \mathrm{NaF}\) d. \(0.2 \mathrm{M} \mathrm{HNO}_{3}\) and \(0.4 \mathrm{M} \mathrm{NaOH}\)

A buffered solution is made by adding \(50.0 \mathrm{~g} \mathrm{NH}_{4} \mathrm{Cl}\) to \(1.00\) \(\mathrm{L}\) of a \(0.75-M\) solution of \(\mathrm{NH}_{3} .\) Calculate the \(\mathrm{pH}\) of the final solution. (Assume no volume change.)

What quantity (moles) of \(\mathrm{HCl}(g)\) must be added to \(1.0 \mathrm{~L}\) of 2.0 \(M \mathrm{NaOH}\) to achieve a pH of \(0.00 ?\) (Neglect any volume changes.)

Figure \(15.4\) shows the \(\mathrm{pH}\) curves for the titrations of six different acids by \(\mathrm{NaOH}\). Make a similar plot for the titration of three different bases by \(0.10 \mathrm{M} \mathrm{HCl}\). Assume \(50.0 \mathrm{~mL}\) of \(0.20 M\) of the bases and assume the three bases are a strong base \((\mathrm{KOH})\), a weak base with \(K_{\mathrm{b}}=1 \times 10^{-5}\), and another weak base with \(K_{\mathrm{b}}=1 \times 10^{-10}\).
See all solutions

Recommended explanations on Chemistry Textbooks

Kinetics

Read Explanation

Chemistry Branches

Read Explanation

Inorganic Chemistry

Read Explanation

Physical Chemistry

Read Explanation

Nuclear Chemistry

Read Explanation

Ionic and Molecular Compounds

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