Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 15: Q81E (page 877)

Question: In dilute aqueous solution HF acts as a weak acid. However, pure liquid HF (boiling point = 19.5 °C) is a strong acid. In liquid HF, HNO3 acts like a base and accepts protons. The acidity of liquid HF can be increased by adding one of several inorganic fluorides that are Lewis acids and accept F–ion (for example, BF3 or SbF5). Write balanced chemical equations for the reaction of pure HNO3 with pure HF and of pure HF with BF3.

Short Answer

Expert verified

The balanced chemical equations are

Step by step solution

01

Find the balanced chemical equations-:

Species that can accept two electrons are Lewis acids.

Bronsted Lowry acid - a compound that donates a proton

Let us write balanced chemical equations for the reaction of pure HNO3with pure HF and of pure HF with BF3.

  • The reaction of pure HNO3with pure HF
  • Since pure HF is a strong acid, HNO3acts like a base (so accepts a proton (H+)), we get

  • The reaction of pure HF with BF3
  • Here BF3acts like a Lewis acid, to it accepts F- ion, hence

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

Question: What are the concentrations of Ag+, CN–, and Ag (CN)2− in a saturated solution of AgCN?

Question: Magnesium metal (a component of alloys used in aircraft and a reducing agent used in the production of uranium, titanium, and other active metals) is isolated from seawater by the following sequence of reactions:

\(\begin{array}{*{20}{c}}{M{g^{2 + }}(aq) + Ca{{(OH)}_2}(aq) \to Mg{{(OH)}_2}(s) + C{a^{2 + }}(aq)}\\{Mg{{(OH)}_2}(s) + 2HCl(aq) \to MgC{l_2}(s) + 2{H_2}O(l)}\end{array}\)

\(MgC{l_2}(l)\mathop \to \limits^{\;electrolysis\;} Mg(s) + C{l_2}(g)\)

Sea water has a density of 1.026 g/cm3 and contains 1272 parts per million of magnesium \(M{g^{2 + }}(aq)\)by mass. What mass, in kilograms, \(Ca{(OH)_2}\)is required to precipitate 99.9% of the magnesium in 1.00 × 103 L of seawater?

Question: A solution contains \(1.0 \times 1{0^{ - 5}}\)mol of KBr and 0.10 mol of KCl per liter. \(AgN{O_3}\)is gradually added to this solution. Which forms first, solid AgBr or solid AgCl?

Even though Ca(OH)2 is an inexpensive base, its limited solubility restricts its use. What is theof a saturated solution of Ca(OH)2?

Assuming that no equilibria other than dissolution are involved, calculate the concentration of all solute species in each of the following solutions of salts in contact with a solution containing a common ion. Show that it is not appropriate to neglect the changes in the initial concentrations of the common ions.

(a) \(TlCl(s)\) in \(0.025MTlN{O_3}\)

(b) \(Ba{F_2}(\;s)\) in \(0.0313M\;KF\)

(c) \(Mg{C_2}{O_4}\) in \(2.250\;L\)of a solution containing \(8.156\;g\) of \(Mg{\left( {N{O_3}} \right)_2}\)

(d) \(Ca{(OH)_2}(\;s)\) in an unbuffered solution initially with a pH of \(12.700\)
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Reactions

Read Explanation

Chemical Analysis

Read Explanation

Organic Chemistry

Read Explanation

Physical Chemistry

Read Explanation

Chemistry Branches

Read Explanation

The Earths Atmosphere

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