Ch.4 - Chemical Quantities & Aqueous ReactionsWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: You choose to investigate some of the solubility guidelines for two ions not listed in the table below, the chromate ion (CrO42 - and the oxalate ion (C2O42-). You are given 0.01 M solutions (A, B, C, D) of four water-soluble salts: Solution Solute Color of Solution A Na2CrO4 Yellow B (NH4)2C2O4 Colorless C AgNO3 Colorless D CaCl2 Colorless When these solutions are mixed, the following observations are made: Experiment Number Solutions Mixed Result 1 A+B No precipitate, yellow solution 2 A+C Red precipitate forms 3 A+D Yellow precipitate forms 4 B+C White precipitate forms 5 B+D White precipitate forms 6 C+D White precipitate forms Write a net ionic equation for the reaction that occurs in each of the experiments. Identify the precipitate formed, if any, in each of the experiments.Write a net ionic equation for the reaction that occurs in the experiment 1.

Problem
You choose to investigate some of the solubility guidelines for two ions not listed in the table below, the chromate ion (CrO42 - and the oxalate ion (C2O42-).

Table 4.1 gives solubility guidelines for common ionic compounds in water and lists any important exceptions.

You are given 0.01 M solutions (A, B, C, D) of four water-soluble salts:

Solution Solute Color of Solution
A Na2CrO4 Yellow
B (NH4)2C2O4 Colorless
C AgNO3 Colorless
D CaCl2 Colorless

When these solutions are mixed, the following observations are made:

Experiment Number Solutions Mixed Result
1 A+B No precipitate, yellow solution
2 A+C Red precipitate forms
3 A+D Yellow precipitate forms
4 B+C White precipitate forms
5 B+D White precipitate forms
6 C+D White precipitate forms

Write a net ionic equation for the reaction that occurs in each of the experiments. Identify the precipitate formed, if any, in each of the experiments.

Write a net ionic equation for the reaction that occurs in the experiment 1.