Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 2: Problem 35

A sample of solid \(\mathrm{MgCl}_{2}\) would be most soluble in which of the following solutions? (A) \(\operatorname{LiOH}(a q)\) (B) \(\operatorname{CBr}_{4}(a q)\) (C) \(\operatorname{Mg}\left(\mathrm{NO}_{3}\right)_{2}(a q)\) (D) \(\mathrm{AlCl}_{3}(a q)\)

Short Answer

Expert verified
The sample of solid \(\mathrm{MgCl}_{2}\) would be most soluble in \(\mathrm{AlCl}_{3}(a q)\).

Step by step solution

01

Identify the Anion in \(\mathrm{MgCl}_{2}\)

The given salt is \(\mathrm{MgCl}_{2}\) and the anion in this salt is Cl-.
02

Compare the anion with the ions in given solvents

Now the aim is to find out a solvent which also has Cl- ions. Going through the solvents,(A) \(\operatorname{LiOH}(a q)\): Here, the solvent does not have Cl- ion.(B) \(\operatorname{CBr}_{4}(a q)\): This solvent also does not have Cl- ion.(C) \(\operatorname{Mg}\left(\mathrm{NO}_{3}\right)_{2}(a q)\): This solvent also does not have Cl- ion.(D) \(\mathrm{AlCl}_{3}(a q)\): This solvent does have Cl- ions.
03

Choose the correct option

The solvent with the same anion as the given salt is \(\mathrm{AlCl}_{3}(a q)\). So, \(\mathrm{MgCl}_{2}\) would be most soluble in \(\mathrm{AlCl}_{3}(a q)\) .

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

A sample of \(\mathrm{H}_{2} \mathrm{S}\) gas is placed in an evacuated, sealed container and heated until the following decomposition reaction occurs at \(1000 \mathrm{K} :\) $$2 \mathrm{H}_{2} \mathrm{S}(g) \rightarrow 2 \mathrm{H}_{2}(g)+\mathrm{S}_{2}(g) \qquad K_{\mathrm{c}}=1.0 \times 10^{-6}$$ As the reaction progresses at a constant temperature of 1000 K, how does the value for the Gibbs free energy constant for the reaction change? (A) It stays constant. (B) It increases exponentially. (C) It increases linearly. (D) It decreases exponentially.

\(\mathrm{SF}_{4}(g)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{SO}_{2}(g)+4 \mathrm{HF}(g) \Delta H=-828 \mathrm{kJ} / \mathrm{mol}\) Which of the following statements accurately describes the above reaction? (A) The entropy of the reactants exceeds that of the products. (B) \(\mathrm{H}_{2} \mathrm{O}(l)\) will always be the limiting reagent. (C) This reaction is never thermodynamically favored. (D) The temperature of the surroundings will increase as this reaction Progresses.

A solution of sulfurous acid, \(\mathrm{H}_{2} \mathrm{SO}_{3}\) , is present in an aqueous solution. Which of the following represents the concentrations of three different ions in solution? (A) \(\left[\mathrm{SO}_{3}^{2-}\right]>\left[\mathrm{HSO}_{3}^{-}\right]>\left[\mathrm{H}_{2} \mathrm{SO}_{3}\right]\) (B) \(\left[\mathrm{H}_{2} \mathrm{SO}_{3}\right]>\left[\mathrm{HSO}_{3}^{-}\right]>\left[\mathrm{SO}_{3}^{2-}\right]\) (C) \(\left[\mathrm{H}_{2} \mathrm{SO}_{3}\right]>\left[\mathrm{HSO}_{3}^{-}\right]=\left[\mathrm{SO}_{3}^{2-}\right]\) (D) \(\left[\mathrm{SO}_{3}^{2-}\right]=\left[\mathrm{HSO}_{3}^{-}\right]>\left[\mathrm{H}_{2} \mathrm{SO}_{3}\right]\)

20.0 \(\mathrm{mL}\) of 1.0 \(\mathrm{M} \mathrm{Na}_{2} \mathrm{CO}_{3}\) is placed in a beaker and titrated with a solution of \(1.0 \mathrm{M} \mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2},\) resulting in the creation of a precipitate. What will happen to the conductivity of the solution after additional \(\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}\) is added past the equivalence point? (A) The conductivity will increase as additional ions are being added to the solution. (B) The conductivity will stay constant as the precipitation reaction has gone to completion. (C) The conductivity will decrease as the solution will be diluted with the addition of additional \(\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}\). (D) The conductivity will stay constant as equilibrium has been established.

The average mass, in grams, of one mole of carbon atoms is equal to (A) the average mass of a single carbon atom, measured in amus (B) the ratio of the number of carbon atoms to the mass of a single carbon atom (C) the number of carbon atoms in one amu of carbon (D) the mass, in grams, of the most abundant isotope of carbon
See all solutions

Recommended explanations on Chemistry Textbooks

Nuclear Chemistry

Read Explanation

Making Measurements

Read Explanation

The Earths Atmosphere

Read Explanation

Chemical Reactions

Read Explanation

Physical 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