Logout Open In App
Open In App
Warning: foreach() argument must be of type array|object, bool given in /var/www/html/web/app/themes/studypress-core-theme/template-parts/header/mobile-offcanvas.php on line 20

Chapter 4: Problem 25

Which ions remain in solution, unreacted, after each of the following pairs of solutions is mixed? (a) potassium carbonate and magnesium sulfate (b) lead nitrate and lithium sulfide (c) ammonium phosphate and calcium chloride

Short Answer

Expert verified
(a) The remaining ions in the solution after mixing potassium carbonate and magnesium sulfate are K\(^+\) and SO4\(^{2-}\). (b) The remaining ions in the solution after mixing lead nitrate and lithium sulfide are Li\(^+\) and NO3\(^-\). (c) The remaining ions in the solution after mixing ammonium phosphate and calcium chloride are NH4\(^+\) and Cl\(^-\).

Step by step solution

01

(a) Potassium Carbonate and Magnesium Sulfate

Potassium carbonate has the formula K2CO3 and magnesium sulfate has the formula MgSO4.
02

(b) Lead Nitrate and Lithium Sulfide

Lead nitrate has the formula Pb(NO3)2, and lithium sulfide has the formula Li2S.
03

(c) Ammonium Phosphate and Calcium Chloride

Ammonium phosphate has the formula (NH4)3PO4, and calcium chloride has the formula CaCl2. **Step 2: Identify the possible products formed when these reactants are combined**
04

(a) Potential products from Potassium Carbonate and Magnesium Sulfate reaction

When K2CO3 and MgSO4 react, they can form potassium sulfate (K2SO4) and magnesium carbonate (MgCO3).
05

(b) Potential products from Lead Nitrate and Lithium Sulfide reaction

When Pb(NO3)2 and Li2S react, they can form lead sulfide (PbS) and lithium nitrate (LiNO3).
06

(c) Potential products from Ammonium Phosphate and Calcium Chloride reaction

When (NH4)3PO4 and CaCl2 react, they can form ammonium chloride (NH4Cl) and calcium phosphate (Ca3(PO4)2). **Step 3: Determine whether these products would precipitate or remain in solution**
07

(a) Precipitation from Potassium Carbonate and Magnesium Sulfate reaction

In this case, MgCO3 would form a precipitate, while K2SO4 would remain in the solution.
08

(b) Precipitation from Lead Nitrate and Lithium Sulfide reaction

In this case, PbS would form a precipitate, and LiNO3 would remain in the solution.
09

(c) Precipitation from Ammonium Phosphate and Calcium Chloride reaction

In this case, Ca3(PO4)2 would form a precipitate, and NH4Cl would remain in the solution. **Step 4: Write the remaining ions that stay in the solution and do not precipitate**
10

(a) Ions remaining in solution after Potassium Carbonate and Magnesium Sulfate reaction

The remaining ions in the solution are K+ and SO4^2-.
11

(b) Ions remaining in solution after Lead Nitrate and Lithium Sulfide reaction

The remaining ions in the solution are Li+ and NO3^-.
12

(c) Ions remaining in solution after Ammonium Phosphate and Calcium Chloride reaction

The remaining ions in the solution are NH4+ and Cl^-.

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

You are presented with a white solid and told that due to careless labeling it is not clear if the substance is barium chloride, lead chloride, or zinc chloride. When you transfer the solid to a beaker and add water, the solid dissolves to give a clear solution. Next a \(\mathrm{Na}_{2} \mathrm{SO}_{4}(a q)\) solution is added and a white precipitate forms. What is the identity of the unknown white solid? [Section 4.2]

Classify each of the following substances as a nonelectrolyte, weak electrolyte, or strong electrolyte in water: (a) \(\mathrm{H}_{2} \mathrm{SO}_{3}\), (b) \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\) (ethanol), (c) \(\mathrm{NH}_{3}\), (d) \(\mathrm{KClO}_{3}\), (e) \(\mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2}\).

State whether each of the following statements is true or false. Justify your answer in each case. (a) Sulfuric acid is a monoprotic acid. (b) \(\mathrm{HCl}\) is a weak acid. (c) Methanol is a base.

(a) Starting with solid sucrose, \(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\), describe how you would prepare \(250 \mathrm{~mL}\) of a \(0.250 \mathrm{M}\) sucrose solution. (b) Describe how you would prepare \(350.0 \mathrm{~mL}\) of \(0.100 \mathrm{MC}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\) starting with \(3.00 \mathrm{~L}\) of \(1.50 \mathrm{M} \mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\).

The U.S. standard for arsenate in drinking water requires that public water supplies must contain no greater than 10 parts per billion ( \(\mathrm{ppb})\) arsenic. If this arsenic is present as arsenate, \(\mathrm{AsO}_{4}{ }^{3-}\), what mass of sodium arsenate would be present in a \(1.00\)-L sample of drinking water that just meets the standard? Parts per billion is defined on a mass basis as $$ \mathrm{ppb}=\frac{\mathrm{g} \text { solute }}{\text { g solution }} \times 10^{9} $$
See all solutions

Recommended explanations on Chemistry Textbooks

Making Measurements

Read Explanation

Chemistry Branches

Read Explanation

Physical Chemistry

Read Explanation

Kinetics

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Chemical Reactions

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