Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 13: Problem 169

Consider 0.10 \(M\) solutions of the following compounds: \(\mathrm{AlCl}_{3}, \mathrm{NaCN}, \mathrm{KOH}, \mathrm{CsClO}_{4},\) and NaF. Place these solutions in order of increasing \(\mathrm{pH}\).

Short Answer

Expert verified
The solutions in order of increasing pH are: \(\mathrm{AlCl}_3 < \mathrm{CsClO}_4 < \mathrm{NaF} < \mathrm{NaCN} < \mathrm{KOH}\).

Step by step solution

01

Identify Cations and Anions

For each ionic compound, the cation (positive ion) comes before the anion (negative ion): - \(\mathrm{AlCl}_3\): Cation = Al\(^{3+}\), Anion = Cl\(^-\) - \(\mathrm{NaCN}\): Cation = Na\(^+\), Anion = CN\(^-\) - \(\mathrm{KOH}\): Cation = K\(^+\), Anion = OH\(^-\) - \(\mathrm{CsClO}_4\): Cation = Cs\(^+\), Anion = ClO\(_4^-\) - NaF: Cation = Na\(^+\), Anion = F\(^-\)
02

Determine acid/base properties of cations and anions

Cations and anions can have acidic or basic properties depending on how they react with water. - Al\(^{3+}\): Acidic cation (hydrolyzes to form Al(OH)\(^{2+}\) and H\(^+\)) - Cl\(^-\): Neutral anion (no reaction with water) - Na\(^+\): Neutral cation (no reaction with water) - CN\(^-\): Basic anion (hydrolyzes to form HCN and OH\(^-\)) - K\(^+\): Neutral cation (no reaction with water) - OH\(^-\): Basic anion (reacts with water to form more OH\(^-\)) - Cs\(^+\): Neutral cation (no reaction with water) - ClO\(_4^-\): Neutral anion (no reaction with water) - F\(^-\): Basic anion (hydrolyzes to form HF and OH\(^-\))
03

Arrange solutions in order of increasing pH

Now, we can arrange the solutions in order of increasing pH based on the acidity/basicity determined above: 1. \(\mathrm{AlCl}_3\): acidic solution (Al\(^{3+}\) is acidic), lowest pH 2. \(\mathrm{CsClO}_4\): neutral solution (Cs\(^+\) and ClO\(_4^-\) are both neutral) 3. \(\mathrm{NaCN}\): basic solution (CN\(^-\) is basic) 4. NaF: basic solution (F\(^-\) is basic but less basic than CN\(^-\)) 5. \(\mathrm{KOH}\): highly basic solution (OH\(^-\) is very basic), highest pH In order of increasing pH: \(\mathrm{AlCl}_3 < \mathrm{CsClO}_4 < \mathrm{NaF} < \mathrm{NaCN} < \mathrm{KOH}\).

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

The equilibrium constant \(K_{\mathrm{a}}\) for the reaction $$\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}^{3+}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons{\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5}}(\mathrm{OH})^{2+}(a q)+\mathrm{H}_{3} \mathrm{O}^{+}(a q)$$ is \(6.0 \times 10^{-3}\) a. Calculate the \(\mathrm{pH}\) of a \(0.10-M\) solution of \(\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}^{3+}\) b. Will a \(1.0-M\) solution of iron(II) nitrate have a higher or lower \(\mathrm{pH}\) than a \(1.0-M\) solution of iron(III) nitrate? Explain.

Is an aqueous solution of NaHSO_ acidic, basic, or neutral? What reaction occurs with water? Calculate the pH of a 0.10-M solution of \(\mathrm{NaHSO}_{4}\).

Calculate the percentage of pyridine \(\left(\mathrm{C}_{5} \mathrm{H}_{5} \mathrm{N}\right)\) that forms pyridinium ion, \(\mathrm{C}_{5} \mathrm{H}_{5} \mathrm{NH}^{+},\) in a \(0.10-M\) aqueous solution of pyridine \(\left(K_{\mathrm{b}}=1.7 \times 10^{-9}\right)\)

Will the following oxides give acidic, basic, or neutral solutions when dissolved in water? Write reactions to justify your answers. a. \(\mathrm{Li}_{2} \mathrm{O}\) b. \(\mathrm{CO}_{2}\) c. SrO

Consider the species \(\mathrm{PO}_{4}^{3-}, \mathrm{HPO}_{4}^{2-},\) and \(\mathrm{H}_{2} \mathrm{PO}_{4}^{-} .\) Each ion can act as a base in water. Determine the \(K_{\mathrm{b}}\) value for each of these species. Which species is the strongest base?
See all solutions

Recommended explanations on Chemistry Textbooks

Kinetics

Read Explanation

Physical Chemistry

Read Explanation

Making Measurements

Read Explanation

Chemical Analysis

Read Explanation

Chemical Reactions

Read Explanation

Organic 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