Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 14: Problem 135

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

Short Answer

Expert verified
a. CaO forms a basic solution: CaO(s) + H2O(l) -> Ca(OH)2(aq) b. SO2 forms an acidic solution: SO2(g) + H2O(l) -> H2SO3(aq) c. Cl2O forms an acidic solution: Cl2O(g) + H2O(l) -> 2HClO(aq)

Step by step solution

01

a. CaO (Calcium oxide)

Calcium oxide (CaO) is a metal oxide, and it typically forms basic solutions when it reacts with water. The reaction between calcium oxide and water is as follows: CaO(s) + H2O(l) -> Ca(OH)2(aq) In this reaction, calcium oxide reacts with water to form calcium hydroxide, which is a strong base. Therefore, the solution formed when CaO is dissolved in water is basic.
02

b. SO2 (Sulfur dioxide)

Sulfur dioxide (SO2) is a nonmetal oxide, and it typically forms acidic solutions when it reacts with water. The reaction between sulfur dioxide and water is as follows: SO2(g) + H2O(l) -> H2SO3(aq) In this reaction, sulfur dioxide reacts with water to form sulfurous acid (H2SO3), which is a weak acid. Therefore, the solution formed when SO2 is dissolved in water is acidic.
03

c. Cl2O (Dichlorine monoxide)

Dichlorine monoxide (Cl2O) is a nonmetal oxide, and it typically forms acidic solutions when it reacts with water. The reaction between dichlorine monoxide and water is as follows: Cl2O(g) + H2O(l) -> 2HClO(aq) In this reaction, dichlorine monoxide reacts with water to form hypochlorous acid (HClO), which is a weak acid. Therefore, the solution formed when Cl2O is dissolved in water is acidic.

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

A \(0.050-M\) solution of the salt \(\mathrm{NaB}\) has a pH of \(9.00\). Calculate the \(\mathrm{pH}\) of a \(0.010-M\) solution of \(\mathrm{HB}\).

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. \(\mathrm{OCl}^{-}, \mathrm{OI}^{-}\)

A solution of formic acid \(\left(\mathrm{HCOOH}, K_{\mathrm{a}}=1.8 \times 10^{-4}\right)\) has a \(\mathrm{pH}\) of \(2.70 .\) Calculate the initial concentration of formic acid in this solution.
See all solutions

Recommended explanations on Chemistry Textbooks

The Earths Atmosphere

Read Explanation

Chemical Analysis

Read Explanation

Organic Chemistry

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Kinetics

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