Chapter 9: Introduction to Solutions & Aqueous Reactions Flashcards
Aqueous Solutions
Solutions in which water acts as the solvent.
Solution
A homogenous mixture of two substances.
Solvent
The majority component of a solution.
Solute
The minority component of a solution.
Dilute Solution
A solution that contains a very small amount of solute relative to the amount of solvent.
Concentrated Solution
A solution that contains a very large amount of solute relative to the amount of solvent.
Molarity (M)
A means of expressing solution concentration as the number of moles of solute per liter of solution.
M = amount of solute (mol)/volume of solution (L)
Stock Solution
A highly concentrated form of a solution used in laboratories to make less concentrated solution via dilution.
Dilution Equation
M1V1=M2V2
M1 = initial molarity of concentrated solution
V1 = initial volume of concentrated solution
M2 = molarity of final diluted solution
V2 = volume of final diluted solution
Solution Stoichiometry
The volume and concentration of a reactant or product can be used to calculate its amount in moles. Then the stoichiometric coefficients in the chemical equation to convert the amount in moles of another reactant or product.
Conceptual Plan of Solution Stoichiometry
Volume A –> Amount A (moles) —> Amount B (moles) —> Volume B
Electrolyte
A substance that dissolves in water to form solutions that conduct electricity.
Strong Electrolyte
A substance that completely dissociates into ions when dissolved in water.
Nonelectrolyte
A compound that does not dissociate into ions when dissolved in water. It creates solutions called nonelectrolyte solutions that do not conduct electricity. Most molecular compounds (except acids) dissolve in water as intact molecules.
Nonelectrolyte Solutions
Solutions that do not conduct electricity.
Acids
Molecular compounds that ionize to form H+ ions when they dissolve in water.
Strong Acid
An acid that completely ionizes in a solution.
- They are also strong electrolytes since they completely ionize in a solution
Chemical Equation of a Strong Acid
Represent the complete ionization of a strong acid with a reaction arrow between the acid and its ionized form:
HCl (aq) –> H+ (aq) + Cl- (aq)
Weak Acid
An acid that does not completely ionize in water. Are classified as weak electrolytes.
Chemical Equation of a Weak Acid
Represent the partial ionization of a weak acid with opposing half arrows between the reactant and product:
HC2H3O2 (aq) H+ (aq) + C2H3O2- (aq)
Weak Electrolyte Solutions
The resulting solution of a weak acid.
Weak Electrolyte
A substance that does not completely ionize in the water and only weakly conducts electricity in solution.
Soluble
Describes a compound that is able to dissolve to a significant extent, usually in water.
Insoluble
Describes a compound that is incapable of dissolving in water or extremely difficult to dissolve in water.
Solubility of a Compound Containing L+
Soluble
Solubility of a Compound Containing Na+
Soluble
Solubility of a Compound Containing K+
Soluble
Solubility of a Compound Containing NH4+
Soluble
Solubility of a Compound Containing NO3-
Soluble
Solubility of a Compound Containing C2H3O2-
Soluble
Solubility of a Compound Containing Cl-
Soluble unless paired with Ag+, H2+2, or Pb2+.
Solubility of a Compound Containing Br-
Soluble unless paired with Ag+, H2+2, or Pb2+.
Solubility of a Compound Containing I-
Soluble unless paired with Ag+, H2+2, or Pb2+.
Solubility of a Compound Containing SO42-
Soluble unless paired with Sr2+, Ba2+, Pb2+, Ag+, or Ca2+.
Solubility of a Compound Containing OH-
Insoluble unless paired with Li+, Na+, K+, or NH4+. When paired with Ca2+, Sr2+, or Ba2+, the resulting compound is slightly soluble.
Solubility of a Compound Containing S2-
Insoluble unless paired with Li+, Na+, K+, or NH4+, Ca2+, Sr2+, or Ba2+.
Solubility of a Compound Containing CO32-
Insoluble unless paired with Li+, Na+, K+, or NH4+.
Solubility of a Compound Containing PO43-
Insoluble unless paired with Li+, Na+, K+, or NH4+.
Precipitation Reaction
A reaction in which a solid, insoluble product forms upon mixing two solutions.
Precipitate
A solid, insoluble ionic compound that forms in, and separate from, a solution.
- Only insoluble compounds form precipitates
- If the possible products are both soluble, no reaction occurs and no precipitate forms
- if one or both of the possible products are insoluble, a precipitation reaction occurs.
Molecular Equation
A chemical equation showing the complete neutral formula for each compound in the reaction.
Complete Ionic Equation
A chemical equation that lists individually all of the ions present as either reactants or products in a chemical reaction.
Spectator Ion
An ion in a complete ionic equation that does not participate in the reaction and therefore remains in the solution. Spectator ions are emitted from the equation.
Acid-Base Reactions (Neutralization Reactions)
An acid reacts with a base and the two neutralize each other, producing water or in some cases a weak electrolyte.
