Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 15: Problem 58

Write a balanced equation to show what happens when \(\mathrm{CaBr}_{2}\) dissolves in water. Use the \((a q)\) symbol when necessary.

Short Answer

Expert verified
The balanced chemical equation for the dissolution of CaBr2 in water is: \[ \mathrm{CaBr}_{2}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{Ca}^{2+}(a q)+2 \mathrm{Br}^{-}(a q) \]

Step by step solution

01

Write the reactants and products

In this step, we need to determine the reactants and products in the reaction. Calcium bromide (CaBr2) is the solute, dissolving in water (H2O) as the solvent. When it dissolves, it dissociates into its constituent ions, calcium (Ca) and bromine (Br). So, the reactants are CaBr2 and water (H2O), and the products are the calcium (Ca) and bromide (Br) ions. Reactants: CaBr2 + H2O Products: Ca^(2+) + 2Br^(-)
02

Include states of matter

In this step, we add the states of matter for each substance in the reaction. Since calcium bromide is dissolving in water, it is in the aqueous phase \((aq)\). Water, as the solvent, is in the liquid phase \((l)\). The ions in the products are surrounded by water molecules and are in the aqueous phase \((aq)\) as well. Reactants: CaBr2\((aq)\) + H2O\((l)\) Products: Ca^(2+)\((aq)\) + 2Br^(-)\((aq)\)
03

Write the balanced chemical equation

Finally, we will write the balanced chemical equation by connecting the reactants and products. Check that the number of atoms for each element is the same on both sides of the equation. CaBr2\((aq)\) + H2O\((l)\) -> Ca^(2+)\((aq)\) + 2Br^(-)\((aq)\) The balanced chemical equation for the dissolution of CaBr2 in water is: \[ \mathrm{CaBr}_{2}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{Ca}^{2+}(a q)+2 \mathrm{Br}^{-}(a q) \]

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

A solution is prepared by dissolving \(2.00\) moles of \(\mathrm{HNO}_{3}\) in enough water to get \(800.0 \mathrm{~mL}\) of solution. What are the \(\mathrm{H}_{3} \mathrm{O}^{+}\) and the \(\mathrm{OH}\) molar concentrations?

The pH of a solution is \(-1\). What are the \(\mathrm{H}_{3} \mathrm{O}^{+}\) and OH concentrations? Is the solution acidic or basic?

If \(0.378 \mathrm{~g}\) of HBr dissolved in enough water to make \(1.25 \mathrm{~L}\) of solution, what is the \(\mathrm{H}_{3} \mathrm{O}^{+}\) concentration? What is the \(\mathrm{OH}^{-}\) concentration?

Write the mathematical definition of \(\mathrm{pH}\), and explain what fundamental change there would be in the pH scale if you left the negative out.

Indicate whether each compound is an electrolyte or a nonelectrolyte in water: (a) \(\mathrm{N}_{2}\) (b) \(\mathrm{NH}_{4} \mathrm{ClO}_{4}\) (c) \(\mathrm{HI}\) (d) \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{3}\) (propane) (e) \(\mathrm{Li}_{3} \mathrm{PO}_{4}\) (f) \(\mathrm{AgNO}_{3}\) (g) \(\mathrm{CCl}_{4}\)
See all solutions

Recommended explanations on Chemistry Textbooks

The Earths Atmosphere

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Nuclear Chemistry

Read Explanation

Chemistry Branches

Read Explanation

Chemical Analysis

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