/*! 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 67 Write the balanced formula equat... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 4: Problem 67

Write the balanced formula equation for the acid-base reactions that occur when the following are mixed. a. potassium hydroxide (aqueous) and nitric acid b. barium hydroxide (aqueous) and hydrochloric acid c. perchloric acid \(\left[\mathrm{HClO}_{4}(a q)\right]\) and solid iron(III) hydroxide d. solid silver hydroxide and hydrobromic acid e. aqueous strontium hydroxide and hydroiodic acid

Short Answer

Expert verified
a. \(KOH (aq) + HNO3 (aq) \rightarrow H2O (l) + KNO3 (aq)\) b. \(Ba(OH)2 (aq) + 2 HCl (aq) \rightarrow 2 H2O (l) + BaCl2 (aq)\) c. \(3 HClO4 (aq) + Fe(OH)3 (s) \rightarrow 3 H2O (l) + Fe(ClO4)3 (aq)\) d. \(AgOH (s) + HBr (aq) \rightarrow H2O (l) + AgBr (s)\) e. \(Sr(OH)2 (aq) + 2 HI (aq) \rightarrow 2 H2O (l) + SrI2 (aq)\)

Step by step solution

01

a. Potassium hydroxide and nitric acid

For this reaction, the reactants are potassium hydroxide (KOH) and nitric acid (HNO3). In an acid-base reaction, the hydrogen (H+) from the acid will combine with the hydroxide (OH-) from the base to form water (H2O). The remaining ions will form a salt. In this case, the salt will be potassium nitrate (KNO3). So, we have: KOH (aq) + HNO3 (aq) 鈫� H2O (l) + KNO3 (aq) The equation is already balanced.
02

b. Barium hydroxide and hydrochloric acid

For this reaction, the reactants are barium hydroxide (Ba(OH)2) and hydrochloric acid (HCl). The acid-base reaction will produce water (H2O) and the salt barium chloride (BaCl2). The balanced equation is as follows: Ba(OH)2 (aq) + 2 HCl (aq) 鈫� 2 H2O (l) + BaCl2 (aq)
03

c. Perchloric acid and solid iron(III) hydroxide

This reaction involves perchloric acid (HClO4) and solid iron(III) hydroxide (Fe(OH)3). The products are water (H2O) and the salt iron(III) perchlorate (Fe(ClO4)3). The balanced equation is: 3 HClO4 (aq) + Fe(OH)3 (s) 鈫� 3 H2O (l) + Fe(ClO4)3 (aq)
04

d. Solid silver hydroxide and hydrobromic acid

The reactants in this case are solid silver hydroxide (AgOH) and hydrobromic acid (HBr). The products will be water (H2O) and the salt silver bromide (AgBr). The balanced equation is: AgOH (s) + HBr (aq) 鈫� H2O (l) + AgBr (s)
05

e. Aqueous strontium hydroxide and hydroiodic acid

Finally, we have the reaction between aqueous strontium hydroxide (Sr(OH)2) and hydroiodic acid (HI). The products will be water (H2O) and the salt strontium iodide (SrI2). The balanced equation is: Sr(OH)2 (aq) + 2 HI (aq) 鈫� 2 H2O (l) + SrI2 (aq)

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

If \(10 . \mathrm{g}\) of \(\mathrm{AgNO}_{3}\) is available, what volume of \(0.25 \mathrm{M} \mathrm{AgNO}_{3}\) solution can be prepared?

A solution was prepared by mixing \(50.00 \mathrm{~mL}\) of \(0.100 \mathrm{M} \mathrm{HNO}_{3}\) and \(100.00 \mathrm{~mL}\) of \(0.200 \mathrm{M} \mathrm{HNO}_{3} .\) Calculate the molarity of the final solution of nitric acid.

You are given a \(1.50-\mathrm{g}\) mixture of sodium nitrate and sodium chloride. You dissolve this mixture into \(100 \mathrm{~mL}\) of water and then add an excess of \(0.500 \mathrm{M}\) silver nitrate solution. You produce a white solid, which you then collect, dry, and measure. The white solid has a mass of \(0.641 \mathrm{~g}\). a. If you had an extremely magnified view of the solution (to the atomic- molecular level), list the species you would see (include charges, if any). b. Write the balanced net ionic equation for the reaction that produces the solid. Include phases and charges. c. Calculate the percent sodium chloride in the original unknown mixture.

What mass of solid \(\mathrm{AgBr}\) is produced when \(100.0 \mathrm{~mL}\) of \(0.150 \mathrm{M}\) \(\mathrm{AgNO}_{3}\) is added to \(20.0 \mathrm{~mL}\) of \(1.00 M \mathrm{NaBr} ?\)

You made \(100.0 \mathrm{~mL}\) of a lead(II) nitrate solution for lab but forgot to cap it. The next lab session you noticed that there was only \(80.0 \mathrm{~mL}\) left (the rest had evaporated). In addition, you forgot the initial concentration of the solution. You decide to take \(2.00 \mathrm{~mL}\) of the solution and add an excess of a concentrated sodium chloride solution. You obtain a solid with a mass of \(3.407 \mathrm{~g}\). What was the concentration of the original lead(II) nitrate solution?
See all solutions

Recommended explanations on Chemistry Textbooks

Physical Chemistry

Read Explanation

Organic Chemistry

Read Explanation

Kinetics

Read Explanation

Chemical Reactions

Read Explanation

The Earths Atmosphere

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.