Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 4: Problem 16

What is the advantage of writing net ionic equations?

Short Answer

Expert verified
The advantage of net ionic equations is that they simplify chemical reactions in aqueous solution, highlighting the reactive species and omitting the spectator ions to focus on the actual chemical process. This makes it easier to analyze, understand, and predict these reactions.

Step by step solution

01

Understanding Ionic Equations

Ionic equations represent the reactions of ions in a chemical reaction, in which all compounds are presented as dissociated ions. For instance, the reaction of silver nitrate and sodium chloride to give silver chloride solid and aqueous sodium nitrate can be depicted as: \( AgNO_3(aq) + NaCl(aq) \rightarrow AgCl(s) + NaNO_3(aq) \) which is the molecular equation.
02

Forming the Net Ionic Equation

This molecular equation can be transformed to an ionic equation by representing all aqueous (dissolved) substances as dissociated ions: \( Ag^+(aq) + NO_3^-(aq) + Na^+(aq) + Cl^-(aq) \rightarrow AgCl(s) + Na^+(aq) + NO_3^-(aq) \). The net ionic equation is then found by cancelling out the ions that appear on both sides of the equation (spectator ions): \( Ag^+(aq) + Cl^-(aq) \rightarrow AgCl(s) \)
03

Advantage of Net Ionic Equations

The key advantage of net ionic equations is that they highlight the essential process involved in a chemical reaction – the formation of a product from its reactant ions. Spectator ions, which do not participate in the reaction, are removed and as a result, the net ionic equation more accurately represents what is occurring on the molecular level in an aqueous solution. It therefore simplifies the reaction and allows concentration on the direct reactive species, making these reactions easier to understand, analyze, and predict.

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 concentration of sulfate in water can be determined by adding a solution of barium chloride to precipitate the sulfate ion. Write the net ionic equation for this reaction. Treating a 145-mL sample of water with excess \(\mathrm{BaCl}_{2}(a q)\) precipitated \(0.330 \mathrm{~g}\) of \(\mathrm{BaSO}_{4} .\) Determine the concentration of sulfate in the original water sample.

Describe the basic steps involved in an acid-base titration. Why is this technique of great practical value?

If \(30.0 \mathrm{~mL}\) of \(0.150 \mathrm{M} \mathrm{CaCl}_{2}\) is added to \(15.0 \mathrm{~mL}\) of \(0.100 M \mathrm{AgNO}_{3},\) what is the mass in grams of \(\mathrm{AgCl}\) precipitate?

Classify the following redox reactions. (a) \(\mathrm{P}_{4}+10 \mathrm{Cl}_{2} \longrightarrow 4 \mathrm{PCl}_{5}\) (b) \(2 \mathrm{NO} \longrightarrow \mathrm{N}_{2}+\mathrm{O}_{2}\) (c) \(\mathrm{Cl}_{2}+2 \mathrm{KI} \longrightarrow 2 \mathrm{KCl}+\mathrm{I}_{2}\) (d) \(3 \mathrm{HNO}_{2} \longrightarrow \mathrm{HNO}_{3}+\mathrm{H}_{2} \mathrm{O}+2 \mathrm{NO}\)

Phosphoric acid \(\left(\mathrm{H}_{3} \mathrm{PO}_{4}\right)\) is an important industrial chemical used in fertilizers, in detergents, and in the food industry. It is produced by two different methods. In the electric furnace method, elemental phosphorus \(\left(\mathrm{P}_{4}\right)\) is burned in air to form \(\mathrm{P}_{4} \mathrm{O}_{10},\) which is then reacted with water to give \(\mathrm{H}_{3} \mathrm{PO}_{4} .\) In the wet process, the mineral phosphate rock fluorapatite \(\left[\mathrm{Ca}_{5}\left(\mathrm{PO}_{4}\right)_{3} \mathrm{~F}\right]\) is reacted with sulfuric acid to give \(\mathrm{H}_{3} \mathrm{PO}_{4}\) (and \(\mathrm{HF}\) and \(\mathrm{CaSO}_{4}\) ). Write equations for these processes and classify each step as precipitation, acid-base, or redox reaction.
See all solutions

Recommended explanations on Chemistry Textbooks

Kinetics

Read Explanation

The Earths Atmosphere

Read Explanation

Making Measurements

Read Explanation

Nuclear Chemistry

Read Explanation

Chemical Reactions

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