Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 14: Problem 21

Which of the following conditions indicate a basic solution at \(25^{\circ} \mathrm{C} ?\) a. \(\mathrm{pOH}=11.21\) b. \(\mathrm{pH}=9.42\) c. \(\left[\mathrm{OH}^{-}\right]>\left[\mathrm{H}^{+}\right]\) d. \(\left[\mathrm{OH}^{-}\right]>1.0 \times 10^{-7} M\)

Short Answer

Expert verified
The conditions that indicate a basic solution at \(25^{\circ} \mathrm{C}\) are: b. pH=9.42 c. \([\mathrm{OH}^{-}] > [\mathrm{H}^{+}]\) d. \([\mathrm{OH}^{-}]>1.0 \times 10^{-7} M\)

Step by step solution

01

Recall the pH scale

The pH scale ranges from 0 to 14, where 7 is considered neutral. Values below 7 indicate an acidic solution, while values above 7 indicate a basic (alkaline) solution.
02

Relationship between pH and pOH

At 25°C, we know that: $$ pH + pOH = 14 $$
03

Evaluate Option a

Given pOH = 11.21, we can infer the pH using the relationship: $$ pH= 14 - pOH $$ $$ pH = 14 - 11.21 = 2.79 $$ Since the pH is less than 7, it represents an acidic solution. Therefore, option a is incorrect.
04

Evaluate Option b

Given pH = 9.42, it is clear that the solution is basic as the pH value is greater than 7. Therefore, option b indicates a basic solution.
05

Evaluate Option c

The presence of a higher concentration of hydroxide ions \([\mathrm{OH}^{-}]\) compared to hydrogen ions \([\mathrm{H}^{+}]\) indicates a basic solution. Therefore, option c indicates a basic solution.
06

Evaluate Option d

At 25°C, the neutral concentration of hydroxide ions \([\mathrm{OH}^{-}]\) and hydrogen ions \([\mathrm{H}^{+}]\) is given by: $$[\mathrm{OH}^{-}]=[\mathrm{H}^{+}]=1.0 \times 10^{-7} M$$ If \([\mathrm{OH}^{-}]>1.0 \times 10^{-7} M\), it indicates a basic solution. Therefore, option d also indicates a basic solution.
07

Conclusion

The conditions that indicate a basic solution at \(25^{\circ} \mathrm{C}\) are: b. pH=9.42 c. \([\mathrm{OH}^{-}] > [\mathrm{H}^{+}]\) d. \([\mathrm{OH}^{-}]>1.0 \times 10^{-7} M\)

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

Consider \(1000 . \mathrm{mL}\) of a \(1.00 \times 10^{-4}-M\) solution of a certain acid HA that has a \(K_{\mathrm{a}}\) value equal to \(1.00 \times 10^{-4}\). How much water was added or removed (by evaporation) so that a solution remains in which \(25.0 \%\) of HA is dissociated at equilibrium? Assume that HA is nonvolatile.

Place the species in each of the following groups in order of increasing base strength. Give your reasoning in each case. a. \(\mathrm{IO}_{3}^{-}, \mathrm{BrO}_{3}^{-}\) b. \(\mathrm{NO}_{2}^{-}, \mathrm{NO}_{3}^{-}\) c. \(\mathrm{OCl}^{-}, \mathrm{OI}^{-}\)

The \(\mathrm{pH}\) of \(1.0 \times 10^{-8} \mathrm{M}\) hydrochloric acid is not \(8.00\). The correct \(\mathrm{pH}\) can be calculated by considering the relationship between the molarities of the three principal ions in the solution \(\left(\mathrm{H}^{+}, \mathrm{Cl}^{-}\right.\), and \(\left.\mathrm{OH}^{-}\right) .\) These molarities can be calculated from algebraic equations that can be derived from the considerations given below. a. The solution is electrically neutral. b. The hydrochloric acid can be assumed to be \(100 \%\) ionized. c. The product of the molarities of the hydronium ions and the hydroxide ions must equal \(K_{\mathrm{w}}\). Calculate the \(\mathrm{pH}\) of a \(1.0 \times 10^{-8}-\mathrm{M} \mathrm{HCl}\) solution.

Calculate \(\left[\mathrm{OH}^{-}\right]\) in a \(3.0 \times 10^{-7}-M\) solution of \(\mathrm{Ca}(\mathrm{OH})_{2}\).

Will \(0.10 M\) solutions of the following salts be acidic, basic, of neutral? See Appendix 5 for \(K_{\mathrm{a}}\) values. a. ammonium bicarbonate b. sodium dihydrogen phosphate c. sodium hydrogen phosphate d. ammonium dihydrogen phosphate e. ammonium formate
See all solutions

Recommended explanations on Chemistry Textbooks

Ionic and Molecular Compounds

Read Explanation

Organic Chemistry

Read Explanation

Chemical Analysis

Read Explanation

Chemistry Branches

Read Explanation

Making Measurements

Read Explanation

Kinetics

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