Solutions and Aqueous Reactions

Solutions Vocab

100

Homogenous mixture

Solution

200

Minor component of solution (being dissolved)

Solute

300

Solution dilution equation

M₁V₁=M₂V₂ or C₁V₁=C₂V₂

400

Way to express solution concentration

Molarity

500

Large amount of solute compared to solvent

Concentrated solution

Solubility Vocab

100

Dissolves in water

Soluble

200

Materials that dissolve in water to form a solution that conducts electricity

Electrolytes

300

Does not dissolve in water

Insoluble

400

Materials that dissolve in water, but do not form ions in the solution

Nonelectrolytes

500

Partial dissociation of materials into ions

Weak electrolytes

Reaction Vocab

100

Insoluble solid product

Precipitate

200

Formulas for aqueous compounds are written as if they existed as molecules

Molecular equation

300

A solid forms when two solutions are mixed

Precipitation Reaction

400

No spectator ions

Net ionic equation

500

Describes the materials structure when dissolved

Complete ionic equation

Soluble/Insoluble (exception?)

100

C₂H₃O₂^- containing molecules

Soluble, no exceptions

200

PbI₂

Insoluble - this is an exception to I^-

300

LiOH

Soluble - this is an exception to OH^-

400

SrSO₄

Insoluble - this is an exception to SO₄^2-

500

Ba(OH)₂

Slightly soluble - this is an exception to OH^-

Practice Problems

100

Write the complete ionic equation, indicate the spectator ions, and then write the net ionic equations.

AgNO₃(aq) + KCl(aq) -> AgCl(s) + KNO₃(aq)

Complete Ionic: Ag⁺(aq) + NO₃^- (aq) + K⁺ (aq) + Cl¯ (aq) -> AgCl (s) + K⁺ (aq) + NO₃¯ (aq)

Spectator Ions: NO₃^-, K⁺

Net Ionic: Ag⁺(aq) + Cl^-(aq) -> AgCl (s)

200

Write the complete ionic equation, indicate the spectator ions, and then write the net ionic equations.

Mg(NO₃)₂ (aq) + Na₂CO₃ (aq) -> MgCO₃ (s) + NaNO₃ (aq)

Complete Ionic: Mg²⁺ (aq) + 2 NO₃¯ (aq) + 2 Na⁺ (aq) + CO₃^2- (aq) -> MgCO₃ (s) + 2 Na⁺ (aq) + 2 NO₃¯ (aq)

Spectator Ions: 2 NO₃^-, 2 Na⁺

Net Ionic: Mg²⁺ (aq) + CO₃^2- (aq) -> MgCO₃ (s)

300

Write the molecular equation, complete ionic equation, indicate the spectator ions, and then write the net ionic equations.

Strontium Bromide (aq) + Potassium Sulfate (aq) -> Strontium Sulfate (s) + Potassium Bromide (aq)

Molecular: SrBr₂ (aq) + K₂SO₄ (aq) -> SrSO₄ (s) + 2 KBr (aq)

Complete Ionic: Sr²⁺ (aq) + 2 Br¯ (aq) + 2 K⁺ (aq) + SO₄^2- (aq) -> SrSO₄ (s) + 2 K⁺ (aq) + 2 Br¯ (aq)

Spectator Ions: 2 Br^-, 2 K⁺

Net Ionic: Sr²⁺ (aq) + SO₄^2- (aq) -> SrSO₄ (s)

400

Write the molecular equation, complete ionic equation, indicate the spectator ions, and then write the net ionic equations.

Chromium(III)Nitrate(aq) + Iron(II)Sulfate(aq) -> Chromium(III)Sulfate(aq) + Iron(II)Nitrate(aq)

Molecular: 2 Cr(NO₃)₃ (aq) + 3 FeSO₄ (aq) -> 3 Fe(NO₃)₂ (aq) + Cr₂(SO₄)₃ (aq)

Complete Ionic: 2 Cr³⁺ (aq) + 6 NO₃¯ (aq) + 3 Fe²⁺ (aq) + 3 SO₄^2- (aq) -> 2 Cr³⁺ (aq) + 6 NO₃¯ (aq) + 3 Fe²⁺ (aq) + 3 SO₄^2- (aq)

Spectator Ions: All ions

Net Ionic: No reaction

500

Predict the products and their states of matter, write the molecular equation, the complete ionic equation, list the spectator ions, and write the net ionic equation.

Calcium Hydroxide + Iron (III) Chloride 

Molecular: 3 Ca(OH)₂ (aq) + 2 FeCl₃ (aq) -> 3 CaCl₂ (aq) + 2 Fe(OH)₃ (s)

Complete Ionic: 3 Ca²⁺ (aq) + 6 OH¯ (aq) + 2 Fe³⁺ (aq) + 6 Cl¯ (aq) -> 3 Ca²⁺ (aq) + 6 Cl¯ (aq) + 2 Fe(OH)₃ (s)

Spectator Ions: 3 Ca²⁺, 6 Cl^-

Net Ionic: 6 OH^- (aq) + 2 Fe³⁺ -> 2 Fe(OH)₃ (s) (simplified is 3:1:1 ratio)