Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 4: Problem 39

Complete and balance the following molecular equations, and then write the net ionic equation for each: \begin{equation} \begin{array}{l}{\text { (a) } \operatorname{HBr}(a q)+\mathrm{Ca}(\mathrm{OH})_{2}(a q) \longrightarrow} \\ {\text { (b) } \mathrm{Cu}(\mathrm{OH})_{2}(s)+\mathrm{HClO}_{4}(a q) \longrightarrow} \\\ {\text { (c) } \mathrm{Al}(\mathrm{OH})_{3}(s)+\mathrm{HNO}_{3}(a q) \longrightarrow}\end{array} \end{equation}

Short Answer

Expert verified
The net ionic equations for the given molecular equations are: (a) \(2\mathrm{H}^{+}(a q)+ 2\mathrm{OH}^{-}(a q) \longrightarrow 2\mathrm{H}_{2}\mathrm{O}(l)\) (b) \(\mathrm{Cu}(\mathrm{OH})_{2}(s)+2\mathrm{H}^{+}(a q) \longrightarrow 2\mathrm{H}_{2}\mathrm{O}(l)+\mathrm{Cu}^{2+}(a q)\) (c) \(\mathrm{Al}(\mathrm{OH})_{3}(s)+3\mathrm{H}^{+}(a q) \longrightarrow 3\mathrm{H}_{2}\mathrm{O}(l)+\mathrm{Al}^{3+}(a q)\)

Step by step solution

01

(a) Identify reactants and products

For the reaction \(\operatorname{HBr}(a q)+\mathrm{Ca}(\mathrm{OH})_{2}(a q) \longrightarrow\), the reactants are HBr (hydrobromic acid) and Ca(OH)₂ (calcium hydroxide), which is an acid-base reaction. The products will be water H₂O (l) and a salt, calcium bromide CaBr₂ (aq).
02

(a) Determine balancing coefficients

To balance the equation, we need 2 moles of HBr for every mole of Ca(OH)₂, 2 moles of water H₂O, and 1 mole of CaBr₂.
03

(a) Write balanced molecular equation

The balanced molecular equation is: \[ 2\operatorname{HBr}(a q)+\mathrm{Ca}(\mathrm{OH})_{2}(a q) \longrightarrow 2\mathrm{H}_{2}\mathrm{O}(l)+\mathrm{CaBr}_{2}(a q) \]
04

(a) Write complete ionic equation

The complete ionic equation is: \[ 2\mathrm{H}^{+}(a q)+2\mathrm{Br}^{-}(a q)+\mathrm{Ca}^{2+}(a q)+ 2\mathrm{OH}^{-}(a q) \longrightarrow 2\mathrm{H}_{2}\mathrm{O}(l)+\mathrm{Ca}^{2+}(a q)+ 2\mathrm{Br}^{-}(a q) \]
05

(a) Net ionic equation

Cancel out spectator ions (Br⁻ and Ca²⁺) from both sides: \[ 2\mathrm{H}^{+}(a q)+ 2\mathrm{OH}^{-}(a q) \longrightarrow 2\mathrm{H}_{2}\mathrm{O}(l) \]
06

(b) Identify reactants and products

For the reaction \[\mathrm{Cu}(\mathrm{OH})_{2}(s)+\mathrm{HClO}_{4}(a q) \longrightarrow\], the reactants are Cu(OH)₂ (copper(II) hydroxide) and HClO₄ (perchloric acid), which is another acid-base reaction. The products will be water H₂O (l) and a salt, copper(II) perchlorate Cu(ClO₄)₂ (aq).
07

(b) Determine balancing coefficients

To balance the equation, we need 1 mole of Cu(OH)₂, 2 moles of HClO₄, 2 moles of water H₂O, and 1 mole of Cu(ClO₄)₂.
08

(b) Write balanced molecular equation

The balanced molecular equation is: \[ \mathrm{Cu}(\mathrm{OH})_{2}(s)+2\mathrm{HClO}_{4}(a q) \longrightarrow 2\mathrm{H}_{2}\mathrm{O}(l)+\mathrm{Cu}(\mathrm{ClO}_{4})_{2}(a q) \]
09

(b) Write complete ionic equation

The complete ionic equation is: \[ \mathrm{Cu}(\mathrm{OH})_{2}(s)+2\mathrm{H}^{+}(a q)+2\mathrm{ClO}_{4}^{-}(a q) \longrightarrow 2\mathrm{H}_{2}\mathrm{O}(l)+\mathrm{Cu}^{2+}(a q)+2\mathrm{ClO}_{4}^{-}(a q) \]
10

(b) Net ionic equation

Cancel out spectator ions (ClO₄⁻) from both sides: \[ \mathrm{Cu}(\mathrm{OH})_{2}(s)+2\mathrm{H}^{+}(a q) \longrightarrow 2\mathrm{H}_{2}\mathrm{O}(l)+\mathrm{Cu}^{2+}(a q) \]
11

(c) Identify reactants and products

For the reaction \[\mathrm{Al}(\mathrm{OH})_{3}(s)+\mathrm{HNO}_{3}(a q) \longrightarrow\], the reactants are Al(OH)₃ (aluminum hydroxide) and HNO₃ (nitric acid), which is another acid-base reaction. The products will be water H₂O (l) and a salt, aluminum nitrate Al(NO₃)₃ (aq).
12

(c) Determine balancing coefficients

To balance the equation, we need 1 mole of Al(OH)₃, 3 moles of HNO₃, 3 moles of water H₂O, and 1 mole of Al(NO₃)₃.
13

(c) Write balanced molecular equation

The balanced molecular equation is: \[ \mathrm{Al}(\mathrm{OH})_{3}(s)+3\mathrm{HNO}_{3}(a q) \longrightarrow 3\mathrm{H}_{2}\mathrm{O}(l)+\mathrm{Al}(\mathrm{NO}_{3})_{3}(a q) \]
14

(c) Write complete ionic equation

The complete ionic equation is: \[ \mathrm{Al}(\mathrm{OH})_{3}(s)+3\mathrm{H}^{+}(a q)+3\mathrm{NO}_{3}^{-}(a q) \longrightarrow 3\mathrm{H}_{2}\mathrm{O}(l)+\mathrm{Al}^{3+}(a q)+3\mathrm{NO}_{3}^{-}(a q) \]
15

(c) Net ionic equation

Cancel out spectator ions (NO₃⁻) from both sides: \[ \mathrm{Al}(\mathrm{OH})_{3}(s)+3\mathrm{H}^{+}(a q) \longrightarrow 3\mathrm{H}_{2}\mathrm{O}(l)+\mathrm{Al}^{3+}(a q) \]

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) By titration, 15.0 \(\mathrm{mL}\) of 0.1008 \(\mathrm{M}\) sodium hydroxide is needed to neutralize a \(0.2053-\mathrm{g}\) sample of a weak acid. What is the molar mass of the acid if it is monoprotic? (b) An elemental analysis of the acid indicates that it is composed of \(5.89 \% \mathrm{H}, 70.6 \% \mathrm{C},\) and 23.5\(\% \mathrm{O}\) by mass. What is composed of \(5.89 \% \mathrm{H}, 70.6 \% \mathrm{C},\) and 23.5\(\% \mathrm{O}\) by mass. What is its molecular formula?

Tartaric acid, \(\mathrm{H}_{2} \mathrm{C}_{4} \mathrm{H}_{4} \mathrm{O}_{6}\) , has two acidic hydrogens. The acid is often present in wines and a salt derived from the acid precipitates from solution as the wine ages. A solution containing an unknown concentration of the acid is titrated with NaOH. It requires 24.65 \(\mathrm{mL}\) of 0.2500 \(\mathrm{M}\) NaOH solution to titrate both acidic protons in 50.00 \(\mathrm{mL}\) of the tartaric acid solution. Write a balanced net ionic equation for the neutralization reaction, and calculate the molarity of the tartaric acid solution.

Would you expect that an anion would be physically closer to the oxygen or to the hydrogens of water molecules that surround it in solution?

An aqueous solution contains 1.2 \(\mathrm{mM}\) of total ions. (a) If the solution is NaCl(aq), what is the concentration of chloride ion? (b) If the solution is \(\mathrm{FeCl}_{3}(a q),\) what is the concentration of chloride ion? [Section 4.5\(]\)

The concept of chemical equilibrium is very important. Which one of the following statements is the most correct way to think about equilibrium? (a) If a system is at equilibrium, nothing is happening. (b) If a system is at equilibrium, the rate of the forward reaction is equal to the rate of the back reaction. (c) If a system is at equilibrium, the product concentration is changing over time. Section 4.1\(]\)
See all solutions

Recommended explanations on Chemistry Textbooks

Making Measurements

Read Explanation

Physical Chemistry

Read Explanation

The Earths Atmosphere

Read Explanation

Chemical Analysis

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Organic 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