Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 13: Problem 137

Identify the Lewis acid and the Lewis base in each of the following reactions. a. \(\mathrm{B}(\mathrm{OH})_{3}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{B}(\mathrm{OH})_{4}^{-}(a q)+\mathrm{H}^{+}(a q)\) b. \(\mathrm{Ag}^{+}(a q)+2 \mathrm{NH}_{3}(a q) \rightleftharpoons \mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}^{+}(a q)\) c. \(\mathrm{BF}_{3}(g)+\mathrm{F}^{-}(a q) \rightleftharpoons \mathrm{BF}_{4}^{-}(a q)\)

Short Answer

Expert verified
In the given reactions: a. Lewis base: \(\mathrm{H}_{2} \mathrm{O}\) (water), Lewis acid: \(\mathrm{B}(\mathrm{OH})_{3}\) b. Lewis base: \(\mathrm{NH}_{3}\) (ammonia), Lewis acid: \(\mathrm{Ag}^{+}\) (silver ion) c. Lewis base: \(\mathrm{F}^{-}\) (fluoride ion), Lewis acid: \(\mathrm{BF}_{3}\) (boron trifluoride)

Step by step solution

01

a. Identifying Lewis acid and Lewis base

For the reaction: \(\mathrm{B}(\mathrm{OH})_{3}(a q)+\mathrm{H}_{2} \mathrm{O}(l)\rightleftharpoons \mathrm{B}(\mathrm{OH})_{4}^{-}(a q)+\mathrm{H}^{+}(a q)\) In this reaction, water \(\mathrm{H}_{2}\mathrm{O}\) is donating a pair of electrons to \(\mathrm{B}(\mathrm{OH})_{3}\) to form \(\mathrm{B}(\mathrm{OH})_{4}^{-}\). So the Lewis base is: \(\mathrm{H}_{2} \mathrm{O}\) (water) And the Lewis acid is: \(\mathrm{B}(\mathrm{OH})_{3}\)
02

b. Identifying Lewis acid and Lewis base

For the reaction: \(\mathrm{Ag}^{+}(a q)+2 \mathrm{NH}_{3}(a q) \rightleftharpoons \mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}^{+}(a q)\) Here, ammonia \(\mathrm{NH}_{3}\) is donating a pair of electrons to the silver ion \(\mathrm{Ag}^{+}\) to form the complex ion \(\mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}^{+}\). So the Lewis base is: \(\mathrm{NH}_{3}\) (ammonia) And the Lewis acid is: \(\mathrm{Ag}^{+}\) (silver ion)
03

c. Identifying Lewis acid and Lewis base

For the reaction: \(\mathrm{BF}_{3}(g)+\mathrm{F}^{-}(a q) \rightleftharpoons \mathrm{BF}_{4}^{-}(a q)\) In this reaction, the fluoride ion \(\mathrm{F}^{-}\) is donating a pair of electrons to boron trifluoride \(\mathrm{BF}_{3}\) to form the tetrafluoroborate ion \(\mathrm{BF}_{4}^{-}\). So the Lewis base is: \(\mathrm{F}^{-}\) (fluoride ion) And the Lewis acid is: \(\mathrm{BF}_{3}\) (boron trifluoride)

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

Place the species in each of the following groups in order of increasing acid strength. Explain the order you chose for each group. a. \(\mathrm{HIO}_{3}, \mathrm{HBrO}_{3}\) b. \(\mathrm{HNO}_{2}, \mathrm{HNO}_{3}\) c. HOCI, HOI d. \(\mathrm{H}_{3} \mathrm{PO}_{4}, \mathrm{H}_{3} \mathrm{PO}_{3}\)

Codeine \(\left(\mathrm{C}_{18} \mathrm{H}_{21} \mathrm{NO}_{3}\right)\) is a derivative of morphine that is used as an analgesic, narcotic, or antitussive. It was once commonly used in cough syrups but is now available only by prescription because of its addictive properties. If the \(\mathrm{pH}\) of a \(1.7 \times 10^{-3}-M\) solution of codeine is \(9.59,\) calculate \(K_{\mathrm{b}}\)

Would you expect \(\mathrm{Fe}^{3+}\) or \(\mathrm{Fe}^{2+}\) to be the stronger Lewis acid? Explain.

Calculate the \(\mathrm{pH}\) of a \(0.050-M\) Al(NO_3)a solution. The \(K_{\mathrm{a}}\) value for \(\mathrm{Al}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}^{3+}\) is \(1.4 \times 10^{-5}\).

Calculate the \(\mathrm{pH}\) of a \(0.200-M\) solution of \(\mathrm{C}_{5} \mathrm{H}_{5} \mathrm{NHF}\). Hint: \(\mathrm{C}_{5} \mathrm{H}_{5} \mathrm{NHF}\) is a salt composed of \(\mathrm{C}_{5} \mathrm{H}_{5} \mathrm{NH}^{+}\) and \(\mathrm{F}^{-}\) ions. The principal equilibrium in this solution is the best acid reacting with the best base; the reaction for the principal equilibrium is $$\begin{aligned} \mathrm{C}_{5} \mathrm{H}_{5} \mathrm{NH}^{+}(a q)+\mathrm{F}^{-}(a q) & \rightleftharpoons \\ \mathrm{C}_{5} \mathrm{H}_{5} \mathrm{N}(a q) &+\mathrm{HF}(a q) \quad K=8.2 \times 10^{-3}\end{aligned}$$
See all solutions

Recommended explanations on Chemistry Textbooks

Inorganic Chemistry

Read Explanation

Nuclear Chemistry

Read Explanation

Making Measurements

Read Explanation

Physical Chemistry

Read Explanation

Organic Chemistry

Read Explanation

Chemical Analysis

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