Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 14: Q1E (page 826)

Question: Write equations that show \(N{H_3}\) as both a conjugate acid and a conjugate base.

Short Answer

Expert verified

The equations which show \(N{H_3}\)as conjugate acid and conjugate base are as follows:

Conjugate acid: \(NH_2^ - + {H^ + } \to N{H_3}\)

Conjugate base: \(NH_4^ + (aq) + O{H^ - }(aq) \to N{H_3}(aq) + {H_2}O(l)\)

Step by step solution

01

Define conjugate acid-base pair

The compounds differ by the existence of one proton that is \({H^ + }\) said to be conjugate acid-base pairs. Every acid has its conjugate base; it is formed when the proton is donated, whereas every base has its conjugate acid; it is formed when a proton is accepted.

02

\(N{H_3}\)as conjugate acid

The chemical equation which shows \(N{H_3}\) as a conjugate acid is given by:

\(NH_2^ - + {H^ + } \to N{H_3}\)

In the above reaction, \(NH_2^ - \)acts as a base and \(N{H_3}\)acts as a conjugate acid because it accepts one proton that is \({H^ + }\).

03

Step 3: \(N{H_3}\)as a conjugate base

The chemical equation which shows \(N{H_3}\)as a conjugate base is given by:

\(NH_4^ + (aq) + O{H^ - }(aq) \to N{H_3}(aq) + {H_2}O(l)\)

In the above reaction,\(NH_4^ + \) acts as an acid and \(N{H_3}\)acts as a conjugate base because it is formed by donating a proton, resulting in the formation of water.

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

What do we represent when we write

\(C{H_3}C{O_2}H(aq) + {H_2}O(l) \rightleftharpoons{H_3}{O^ + }(aq) + C{H_3}CO_2^ - (aq)?\)

The indicator dinitrophenol is an acid with a \({K_a}\) of \(1.1 \times 1{0^{ - 4}}\). In a \(1.0 \times 1{0^{ - 4}} - M\) solution, it is colourless in acid and yellow in the base. Calculate the \(pH\) range over which it goes from \(10\% \) ionized (colourless) to \(90\% \) ionized (yellow).

The pH of a \(0.10 - M\) solution of caffeine is \(11.16. \) Determine \({K_b}\) for caffeine from these data:

\[{C_8}{H_{10}}\;{N_4}{O_2}(aq) + {H_2}O(l)\rightleftharpoons{C_8}{H_{10}}\;{N_4}{O_2}{H^ + }(aq) + O{H^ - }(aq)\]

Nitric acid reacts with insoluble copper (II) oxide to form soluble copper (II) nitrate,Cu (NO3)2, a compound that has been used to prevent the growth of algae in swimming pools. Write the balanced chemical equation for the reaction of an aqueous solution of HNO3 with CuO.

Saccharin, \({{\bf{C}}_{\bf{7}}}{{\bf{H}}_{\bf{4}}}{\bf{NS}}{{\bf{O}}_{\bf{3}}}{\bf{H}}\), is a weak acid\(\left( {{\bf{Ka = 2}}{\bf{.1 \times 1}}{{\bf{0}}^{{\bf{ - 2}}}}} \right)\). If \({\bf{0}}.{\bf{250}}{\rm{ }}{\bf{L}}\) of diet cola with a buffered pH of \({\bf{5}}.{\bf{48}}\) was prepared from \({\bf{2}}.{\bf{00}}{\rm{ }} \times {\rm{ }}{\bf{1}}{{\bf{0}}^{ - {\bf{3}}}}{\bf{g}}\) of sodium saccharide, \({\bf{Na}}\left( {{{\bf{C}}_{\bf{7}}}{{\bf{H}}_{\bf{4}}}{\bf{NS}}{{\bf{O}}_{\bf{3}}}} \right)\), what are the final concentrations of saccharine and sodium saccharide in the solution?
See all solutions

Recommended explanations on Chemistry Textbooks

Nuclear Chemistry

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Physical Chemistry

Read Explanation

Inorganic Chemistry

Read Explanation

Chemistry Branches

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