Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 8: Problem 129

Write the complete ionic equation and the net ionic equation for the reaction that occurs between aqueous solutions of: (a) Silver nitrate and potassium iodide (b) Lithium sulfate and silver acetate

Short Answer

Expert verified
For part (a), the complete ionic equation is: Ag+ (aq) + NO3- (aq) + K+ (aq) + I- (aq) -> AgI (s) + K+ (aq) + NO3- (aq) The net ionic equation is: Ag+ (aq) + I- (aq) -> AgI (s) For part (b), the complete ionic equation is: 2Li+ (aq) + SO4^2- (aq) + 2Ag+ (aq) + 2C2H3O2- (aq) -> Ag2SO4 (s) + 2Li+ (aq) + 2C2H3O2- (aq) The net ionic equation is: 2Ag+ (aq) + SO4^2- (aq) -> Ag2SO4 (s)

Step by step solution

01

Complete ionic equation

The reaction between silver nitrate (AgNO3) and potassium iodide (KI) can be written as follows: AgNO3 (aq) + KI (aq) -> AgI (s) + KNO3 (aq) AgI is a solid because it is insoluble in water, while KNO3 is soluble and remains in the aqueous state. 2. Write the complete ionic equation
02

Complete ionic equation

The complete ionic equation includes all the ions present in the reaction. It can be written as: Ag+ (aq) + NO3- (aq) + K+ (aq) + I- (aq) -> AgI (s) + K+ (aq) + NO3- (aq) 3. Write the net ionic equation
03

Net ionic equation

The net ionic equation includes only the ions that are involved in the formation of the product and removes the spectator ions that remain unreacted. In this case, K+ and NO3- are spectator ions and can be removed. The net ionic equation for the reaction is: Ag+ (aq) + I- (aq) -> AgI (s) #For part (b)# 1. Identify products of the reaction
04

Identify products of the reaction

The reaction between lithium sulfate (Li2SO4) and silver acetate (AgC2H3O2) can be written as follows: Li2SO4 (aq) + 2AgC2H3O2 (aq) -> Ag2SO4 (s) + 2LiC2H3O2 (aq) Ag2SO4 is a solid because it is insoluble in water, while LiC2H3O2 is soluble and remains in the aqueous state. 2. Write the complete ionic equation
05

Complete ionic equation

The complete ionic equation includes all the ions present in the reaction. It can be written as: 2Li+ (aq) + SO4^2- (aq) + 2Ag+ (aq) + 2C2H3O2- (aq) -> Ag2SO4 (s) + 2Li+ (aq) + 2C2H3O2- (aq) 3. Write the net ionic equation
06

Net ionic equation

The net ionic equation includes only the ions that are involved in the formation of the product and removes the spectator ions that remain unreacted. In this case, Li+ and C2H3O2- are spectator ions and can be removed. The net ionic equation for the reaction is: 2Ag+ (aq) + SO4^2- (aq) -> Ag2SO4 (s)

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

Classify each reaction as combination, decomposition, single-replacement, or double-replacement: (a) \(2 \mathrm{NaCl} \rightarrow 2 \mathrm{Na}+\mathrm{Cl}_{2}\) (b) \(\mathrm{Ba}_{3} \mathrm{~N}_{2} \rightarrow 3 \mathrm{Ba}+\mathrm{N}_{2}\) (c) \(\mathrm{Cl}_{2}+2 \mathrm{NaI} \rightarrow 2 \mathrm{NaCl}+\mathrm{I}_{2}\) (d) \(\mathrm{KNO}_{3}+\mathrm{AgBr} \rightarrow \mathrm{AgNO}_{3}+\mathrm{KBr}\)

Consider the covalent bond in \(\mathrm{H}_{2}\). Why must energy be added to break this bond (in other words, what is the added energy used for)?

Why must a chemical equation be balanced?

Calcium hydroxide can be used as an antacid to neutralize \(\mathrm{HCl}\), the acid found in the stomach. Water and calcium chloride, \(\mathrm{CaCl}_{2}\), are the products of the reaction. Write the balanced equation for the reaction.

Fill in this table: $$ \begin{array}{lll} & & \text { Soluble or } \\ \text { Name } & \text { Formula } & \text { insoluble } \\ \hline \text { Sodium phosphate } & & \\ & \mathrm{Ba}\left(\mathrm{CH}_{3} \mathrm{CO}_{2}\right)_{2} & \\ & \left(\mathrm{NH}_{4}\right)_{2} \mathrm{~S} & \\ \text { Iron(II) carbonate } & & \\ \text { Mercury(II) chloride } & & \\ & \mathrm{Co}(\mathrm{OH})_{2} & \\ & \mathrm{HgCl} & \\ \hline \end{array} $$
See all solutions

Recommended explanations on Chemistry Textbooks

Nuclear Chemistry

Read Explanation

Making Measurements

Read Explanation

The Earths Atmosphere

Read Explanation

Kinetics

Read Explanation

Chemistry Branches

Read Explanation

Inorganic 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