/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 44 As \(\mathrm{K}_{2} \mathrm{O}\)... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 4: Problem 44

As \(\mathrm{K}_{2} \mathrm{O}\) dissolves in water, the oxide ion reacts with water molecules to form hydroxide ions. Write the molecular and net ionic equations for this reaction. Based on the definitions of acid and base, what ion is the base in this reaction? What is the acid? What is the spectator ion in the reaction?

Short Answer

Expert verified
The molecular and net ionic equations for the reaction are: Molecular equation: \[ K_{2}O_{(s)} + H_{2}O_{(l)} \rightarrow 2KOH_{(aq)} \] Net ionic equation: \[ O^{2-}_{(aq)} + H_{2}O_{(l)} \rightarrow 2OH^{-}_{(aq)} \] The base in this reaction is the oxide ion (O^2-), the acid is water (H2O), and the spectator ion is the potassium ion (K+).

Step by step solution

01

Find the reaction of K2O with water

To start, let's write the balanced equation for the reaction of K2O (potassium oxide) with water (H2O). K2O will dissociate in water, and the oxide ion (O^2-) will react with water molecules to form hydroxide ions (OH-). The balanced equation is: \[ K_{2}O_{(s)} + H_{2}O_{(l)} \rightarrow 2KOH_{(aq)} \]
02

Write the molecular equation

In the molecular equation, we show the complete formulas of all the species involved in the reaction. In this case, the molecular equation is the same as the balanced equation. So, the molecular equation is: \[ K_{2}O_{(s)} + H_{2}O_{(l)} \rightarrow 2KOH_{(aq)} \]
03

Write the total ionic equation

To write the total ionic equation, we need to represent all the soluble species as ions. Total ionic equation: \[ 2K^{+}_{(aq)} + O^{2-}_{(aq)} + H_{2}O_{(l)} \rightarrow 2K^{+}_{(aq)} + 2OH^{-}_{(aq)} \]
04

Write the net ionic equation

The net ionic equation is found by canceling the spectator ions on both sides of the total ionic equation. In this case, the spectator ion is K+. Net ionic equation: \[ O^{2-}_{(aq)} + H_{2}O_{(l)} \rightarrow 2OH^{-}_{(aq)} \]
05

Identify the base, acid, and spectator ion

According to the Bronsted-Lowry theory, an acid is a proton (H+) donor, and a base is a proton (H+) acceptor. In the net ionic equation, the oxide ion (O^2-) accepts a proton from water, forming two hydroxide ions (OH-). Thus, O^2- is acting as a base. Water (H2O) donates a proton to the oxide ion, so it acts as an acid in this reaction. As mentioned earlier, the spectator ion is \( K^{+} \) because it does not participate in the reaction and appears on both sides of the equation in the same form. In conclusion, the molecular and net ionic equations for the reaction are: Molecular equation: \[ K_{2}O_{(s)} + H_{2}O_{(l)} \rightarrow 2KOH_{(aq)} \] Net ionic equation: \[ O^{2-}_{(aq)} + H_{2}O_{(l)} \rightarrow 2OH^{-}_{(aq)} \] The base in this reaction is the oxide ion (O^2-), the acid is water (H2O), and the spectator ion is the potassium ion (K+).

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.

Over 30 million students worldwide already upgrade their learning with 91影视!

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 safe drinking water standard for arsenic (which is usually found as arsenate, see \(4.115)\) is 50 parts per billion (ppb) in most developing countries. (a) How many grams of sodium arsenate are in 55 gallons of water, if the concentration of arsenate is 50 ppb? (b) In 1993 , naturally occurring arsenic was discovered as a major contaminant in the drinking water across the country of Bangladesh. Approximately 12 million people in Bangladesh still drink water from wells that have higher concentrations of arsenic than the standard. Recently, a chemistry professor from George Mason University was awarded a \(\$ 1\) million Grainger Challenge Prize for Sustainability for his development of a simple, inexpensive system for filtering naturally occuring arsenic from drinking water. The system uses buckets of sand, cast iron, activated carbon, and wood chips for trapping arsenic-containing minerals. Assuming the efficiency of such a bucket system is \(90 \%\) (meaning, \(90 \%\) of the arsenic that comes in is retained in the bucket and \(10 \%\) passes out of the bucket), how many times should water that is 500 ppb in arsenic be passed through to meet the 50 ppb standard?

Salts of the sulfite ion, \(\mathrm{SO}_{3}^{2-}\), react with acids in a way similar to that of carbonates. (a) Predict the chemical formula, and name the weak acid that forms when the sulfite ion reacts with acids. (b) The acid formed in part (a) decomposes to form water and a gas. Predict the molecular formula, and name the gas formed. (c) Use a source book such as the CRC Handbook of Chemistry and Physics to confirm that the substance in part (b) is a gas under normal room-temperature conditions. (d) Write balanced net ionic equations of the reaction of \(\mathrm{HCl}(a q)\) with (i) \(\mathrm{Na}_{2} \mathrm{SO}_{3}(a q)\), (ii) \(\mathrm{Ag}_{2} \mathrm{SO}_{3}(s)\), (iii) \(\mathrm{KHSO}_{3}(s)\), and (iv) \(\mathrm{ZnSO}_{3}(a q)\)

Which of the following are redox reactions? For those that are, indicate which element is oxidized and which is reduced. For those that are not, indicate whether they are precipitation or acid-base reactions. (a) \(\mathrm{Cu}(\mathrm{OH})_{2}(s)+2 \mathrm{HNO}_{3}(a q) \longrightarrow\) \(\mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2}(a q)+2 \mathrm{H}_{2} \mathrm{O}(I)\) (b) \(\mathrm{Fe}_{2} \mathrm{O}_{3}(s)+3 \mathrm{CO}(g) \longrightarrow 2 \mathrm{Fe}(s)+3 \mathrm{CO}_{2}(g)\) (c) \(\mathrm{Sr}\left(\mathrm{NO}_{3}\right)_{2}(a q)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \longrightarrow\) (d) \(\mathrm{SrSO}_{4}(\mathrm{~s})+2 \mathrm{HNO}_{3}(a q)\) \(\mathrm{Zn}(s)+10 \mathrm{H}^{+}(a q)+2 \mathrm{NO}_{3}^{-}(a q) \longrightarrow\) \(4 \mathrm{Zn}^{2+}(a q)+\mathrm{N}_{2} \mathrm{O}(g)+5 \mathrm{H}_{2} \mathrm{O}(l)\)

Explain how a redox reaction involves electrons in the same way that an acid- base reaction involves protons. [Sections \(4.3\) and \(4.4]\)

The metal cadmium tends to form \(\mathrm{Cd}^{2+}\) ions. The following observations are made: (i) When a strip of zinc metal is placed in \(\mathrm{CdCl}_{2}(a q)\), cadmium metal is deposited on the strip. (ii) When a strip of cadmium metal is placed in \(\mathrm{Ni}\left(\mathrm{NO}_{3}\right)_{2}(a q)\), nickel metal is deposited on the strip. (a) Write net ionic equations to explain each of the observations made above. (b) What can you conclude about the position of cadmium in the activity series? (c) What experiments would you need to perform to locate more precisely the position of cadmium in the activity series?
See all solutions

Recommended explanations on Chemistry Textbooks

Making Measurements

Read Explanation

The Earths Atmosphere

Read Explanation

Inorganic Chemistry

Read Explanation

Chemical Reactions

Read Explanation

Organic 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.