CHEM 24112 Lecture Notes - Lecture 19: Lead, Cobalt(Ii) Chloride, Chemical Equation

36 views2 pages

yellowwildebeest520

29 Jun 2018

School

Department

Course

Professor

For unlimited access to Class Notes, a Class+ subscription is required.

CHEMISTRY 112 – DAY 19 Chapter 7 – Sections 1-3

2/26

Aqueous Chemical Reactions: What Drives Them?

Four Driving Forces Favor Chemical Change

Formation of a solid

Formation of water

Transfer of electrons

Formation of a gas

Precipitation: a reaction in which a solid forms is called a precipitation reaction.

Solid = precipitate

What Happens When an Ionic Compound Dissolves in Water?

The ions separate and move around independently.

Strong electrolyte – each unit of the substance that dissolves in water produces separated ions.

K2CrO4(aq) + Ba(NO3)2(aq)  Products

The mixed solution contains four types of ions: K+, CrO4

2–, Ba2+, and NO3

–.

NO3

-CrO4

K+

Ba2+

Using Solubility Rules

How to Predict Precipitates When Solutions of Two Ionic Compounds Are Mixed

1) Write the reactants as they actually exist before any reaction occurs. Remember that when a salt

dissolves, its ions separate.

2) Consider the various solids that could form. To do this, simply exchange the anions of the added salts.

find more resources at oneclass.com

Unlock document

This preview shows half of the first page of the document.
Unlock all 2 pages and 3 million more documents.

Already have an account? Log in

Document Summary

Precipitation: a reaction in which a solid forms is called a precipitation reaction. Strong electrolyte each unit of the substance that dissolves in water produces separated ions. The mixed solution contains four types of ions: k+, cro4. How to predict precipitates when solutions of two ionic compounds are mixed. Write the reactants as they actually exist before any reaction occurs. Remember that when a salt dissolves, its ions separate. To do this, simply exchange the anions of the added salts. Use the solubility rules to decide whether a solid forms and, if so, to predict the identity of the solid. Which of the following ions form compounds with pb2+ that are generally soluble in water? a) A sodium phosphate solution reacts with a lead(ii) nitrate solution. What precipitate, if any, will form? a) b) c) d) Consider a solution with the following ions present: Types of equations for reactions in aqueous solutions: molecular equation.

Related Questions

13-17 explanations

1. Please write balanced net ionic equations for some of the ionic solids that formed in the precipitation lab. (Use the lowest possible coefficients. Omit states-of-matter from your answer. Enter "NONE" if no reaction occurred.)

2. Identify the ionic solids below as soluble or insoluble in water.

3. During lab, students mixed two solutions of soluble ions in a ceramic well to determine if a precipitate forms. Write the dissolution reaction for the ionic solids below. (Use the lowest possible coefficients. Include states-of-matter under the given conditions in your answer.)

The two solutions, when mixed, will have two cations and two anions.

c. Based on your lab results, enter the cation and anion for which a precipitate will form. (Separate substances in a list with a comma.)

d. Write the net precipitation reaction that occurs. (Use the lowest possible coefficients. Include states-of-matter under the given conditions in your answer.)

4. During lab, students mixed two solutions of soluble ions in a ceramic well to determine if a precipitate forms. Based on extrapolation of your lab results, write the dissolution reaction for the ionic solids below. (Use the lowest possible coefficients. Include states-of-matter under the given conditions in your answer.)

The two solutions, when mixed, will have two cations and two anions.

c. Based on your lab results, enter the cation and anion for which a precipitate will form. (Separate substances in a list with a comma.)

d. Write the net precipitation reaction that occurs. (Use the lowest possible coefficients. Include states-of-matter under the given conditions in your answer.)

byzantiumwhale166

The Behavior of Substances in Water

Part 1:

Ammonia, NH₃, is a weak electrolyte. It forms ions in solution by reacting with water molecules to form the ammonium ion and hydroxide ion. Write the balanced chemical reaction for this process, including state symbols.
From everyday experience, you are probably aware that table sugar (sucrose), C₁₂H₂₂O₁₁, is soluble in water. When sucrose dissolves in water, it doesn’t form ions through any reaction with water. It just dissolves without forming ions, so it is a nonelectrolyte. Write the chemical equation for the dissolving of sucrose in water.
Both NH₃ and C₁₂H₂₂O₁₁ are soluble molecular compounds, yet they behave differently in an aqueous solution. Briefly explain why one is a weak electrolyte and the other is a nonelectrolyte.
Hydrochloric acid, HCl, is a molecular compound that is a strong electrolyte. Write the chemical reaction of HCl with water.
Compare the ammonia reaction with that of hydrochloric acid. Why are both of these substances considered electrolytes?
Explain why HCl is a strong electrolyte and ammonia is a weak electrolyte.
Classify each of the following substances as either ionic or molecular:

KCl
NH₃
CO₂
MgBr₂
HCl
Ca(OH)₂
PbS
HC₂H₃O₂

For those compounds above that, you classified as ionic, use the solubility rules to determine which are soluble.
The majority of ionic substances are solids at room temperature. Describe what you would observe if you placed a soluble ionic compound and an insoluble ionic compound in separate beakers of water.
Write the chemical equation(s), including state symbols, for what happens when each soluble ionic compound that you identified above is placed in water. Are these substances reacting with water when they are added to water?
How would you classify the soluble ionic compounds: strong electrolyte, weak electrolyte, or nonelectrolyte? Explain your answer.
Sodium chloride, NaCl, is a strong electrolyte, as is hydroiodic acid, HI. Write the chemical equations for what happens when these substances are added to water. m
Are NaCl and HI strong electrolytes because they have similar behavior in an aqueous solution? If not, describe, using words and equations, the different chemical process that takes place in each case.

Part 2:

You have two hypothetical molecular compounds, AX and AY. AX is a strong electrolyte and AY is a weak electrolyte. The compounds undergo the following chemical reactions when added to water.

AX (aq) + H₂O (l) → AH₂O⁺ (aq) + X⁻ (aq)

AY (aq) + H₂O (l) → AH₂O⁺ (aq) + Y⁻ (aq)

Explain how the relative amounts of AX ( aq ) and AY ( aq ) would compare if you had a beaker of water with AX and a beaker of water with AY.
How would the relative amounts of X⁻ ( aq) and Y⁻ ( aq) in the two beakers compare? Be sure to explain your answer.

indigolouse566

CHEM 24112 Lecture Notes - Lecture 19: Lead, Cobalt(Ii) Chloride, Chemical Equation

Document Summary

Get access

Related textbook solutions

Chemistry: Structure and Properties

Basic Chemistry

Principles of Chemistry Molecular Approach

Principles of Chemistry Molecular Approach

Chemistry: Structure and Properties

Chemistry: A Molecular Approach

Chemistry: A Molecular Approach

Principles of Chemistry: A Molecular Approach

Chemistry: The Central Science

Related Documents

CHEM 24112 Study Guide - Quiz Guide: Barium Chloride, Spectator Ion, Solubility

CHEM 24112 Lecture Notes - Lecture 20: Lithium Hydroxide, Chemical Equation, Sodium Hydroxide

CHEM 24112 Study Guide - Quiz Guide: Nickel(Ii) Chloride, Barium Nitrate, Potassium Sulfate

Related Questions