Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 14: Q14.3-30 E (page 829)

Household ammonia is a solution of the weak base\(N{H_3}\) in water. List, in order of descending concentration, all of the ionic and molecular species present in a 1-M aqueous solution of this base.

Short Answer

Expert verified

Descending order of concentration as \({H_2}O > N{H_3} > NH_4^ + = O{H^ - } > {H^ + }\)

Step by step solution

01

Define Ions and Molecules:

Molecular compounds consist of atoms due to covalent bonding while ionic compounds are result of electron transfer and made due to ionic bonding.

02

Descending order of concentration:

1-molar solution water molecules are those with the highest concentration ammonia is a weak base there are more ammonia molecules than the products of the reaction of ammonia with water. Equal concentration have the products of the ammonia and water reaction the hydroxide ion and the ammonia ion. Lowest concentration has hydrogen ions. Always both\(O{H^ - }and\;{H^ + }\)ions in a solution, concentrations are equal, for an acidic or basic solution

Therefore, the descending order of concentrations are \({H_2}O > N{H_3} > NH_4^ + = O{H^ - } > {H^ + }\)

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 ionization constant for water\(({K_w})\) is\(2.9 \times 1{0^{ - 14}}\;at\;4{0^o}C\). Calculate\(\left( {{H_3}{O^ + }} \right),\left( {O{H^ - }} \right),pH,\;and\;pOH\) for pure water at \(4{0^o}C\).

The hydronium ion concentration of vinegar is approximately 4×10−3 M. What are the corresponding values of pOH and pH?

From the equilibrium concentrations given, calculate \({K_a}\)for each of the weak acids and \({K_b}\)for each of the weak bases.

\(\begin{aligned}(a)N{H_3}:\left( {O{H^ - }} \right) = 3.1 \times 1{0^{ - 3}}M\left( {NH_4^ + } \right) = 3.1 \times 1{0^{ - 3}}M;\left( {N{H_3}} \right) = 0.533M;\\(b)HN{O_2}:\left( {{H_3}{O^ + }} \right) = 0.011M;\left( {NO_2^ - } \right) = 0.0438M;\left( {HN{O_2}} \right) = 1.07M;\\(c){\left( {C{H_3}} \right)_3}\;N:\left( {{{\left( {C{H_3}} \right)}_3}\;N} \right) = 0.25M;\left( {{{\left( {C{H_3}} \right)}_3}N{H^ + }} \right) = 4.3 \times 1{0^{ - 3}}M;\left( {O{H^ - }} \right) = 4.3 \times 1{0^{ - 3}}M;\\(d)N{H_4} + :\left( {N{H_4} + } \right) = 0.100M;\left( {N{H_3}} \right) = 7.5 \times 1{0^{ - 6}}M;\left( {{H_3}{O^ + }} \right) = 7.5 \times 1{0^{ - 6}}M\end{aligned}\)

\(\begin{aligned}\left( {N{H_3}} \right) = 7.5 \times 1{0^{ - 6}}M\\\left( {{H_3}{O^ + }} \right) = 7.5 \times 1{0^{ - 6}}M\end{aligned}\)

State which of the following species are amphiprotic and write chemical equations illustrating the amphiprotic character of these species.

\({\rm{\;(a)\;N}}{{\rm{H}}_3}\)

\({\rm{\;(b)\;HPO}}_4^ - \)

\({\rm{\;(c)\;B}}{{\rm{r}}^ - }\).

\({\rm{\;(d)\;N}}{{\rm{H}}_4} + \)

\({\rm{\;(e)\;ASO}}_4^{3 - }\).

What two common assumptions can simplify calculation of equilibrium concentrations in a solution of a weak acid?
See all solutions

Recommended explanations on Chemistry Textbooks

Physical Chemistry

Read Explanation

Chemical Analysis

Read Explanation

Kinetics

Read Explanation

Chemistry Branches

Read Explanation

Chemical Reactions

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