CHEM 1A03 Lecture Notes - Lecture 17: Solubility Equilibrium, Ionic Compound, Conjugate Acid

26 views11 pages

lemonkoala962

28 Jun 2016

School

Department

Course

Professor

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

itsmealionline and 39769 others unlocked

CHEM 1A03 Full Course Notes

Verified Note

35 documents

Document Summary

Solubility is a quantitative property of compounds that describes the concentration of a saturated solution in a particular solvent at a given temperature. Weak electrolytes are ionic compounds with relatively low, or partial, solubility in water. The solubility product constant, ksp, is the value obtained from the equilibrium law applied to a saturated solution. Describes the equilibrium between the solid ionic compound and the dissolved aqueous ions. When mixing solutions of soluble compounds, ions of insoluble compounds may form precipitates depending on the value of ksp. Similar to the reaction quotient, the trial ion product is calculated and compared to the soluble product constant to determine if a precipitate will form. No precipitate (more solid could be dissolved) supersaturated saturated unsaturated. By introducing a common ion into a saturated system, it reduces the solubility of the ionic compound. The common ion arises from a highly soluble compound. Common anions can be paired with na+

Related Questions

Will rate the best explained submission

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 1A03 Lecture Notes - Lecture 17: Solubility Equilibrium, Ionic Compound, Conjugate Acid

CHEM 1A03 Full Course Notes

Document Summary

Get access

Related textbook solutions

Chemistry: Structure and Properties

Basic Chemistry

Principles of Chemistry Molecular Approach

Chemistry: Structure and Properties

Principles of Chemistry Molecular Approach

Chemistry: A Molecular Approach

Chemistry: A Molecular Approach

Principles of Chemistry: A Molecular Approach

Chemistry: The Central Science

Related Documents

CHEM 1A03 Chapter Notes -Sodium Chloride, Sodium Bromide, Alkali Metal

CHEM 1A03 Lecture Notes - Lecture 8: Inert Gas, Hydrophile, Equilibrium Constant

CHEM 1A03 Lecture Notes - Lecture 7: Equilibrium Constant, Dynamic Equilibrium, Rice Chart

Related Questions