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Chapter 4 Unit 2

TermDefinition
Solution Homogeneous mixture containing at least two components.
Solvent Substance present in largest number of moles.
Solute Substances other than the solvent in a solution
Aqueous Solution Solution where water is the solvent.
Polarity Property of molecules with uneven electron distribution.
Electronegativity Tendency of an atom to attract electrons.
Dissolution Process where solvent surrounds solute particles.
Molarity Concentration unit defined as moles per liter.
Stock Solution Solution with a standardized concentration for dilutions.
Dilution Equation McVc = MdVd for concentration calculations.
Electrolyte Solution Conducts electricity due to dissociated ions.
Nonelectrolyte Solution Does not conduct electricity; no dissociated ions.
Strong Electrolyte Fully dissociates into ions in solution.
Weak Electrolyte Partially dissociates, resulting in fewer ions.
Carboxylic Acid Weak electrolyte containing a carboxyl group.
Dynamic Equilibrium Forward and reverse processes occur at equal rates.
Solubility Rules Guidelines predicting ionic substance solubility.
Precipitation Reaction Formation of an insoluble compound from solutions.
Precipitate Solid formed in a precipitation reaction.
Forumla Unit Equation Chemical formulas and phases of compounds shown.
Complete Ionic Equation Dissociated ions shown for soluble compounds.
Net Ionic Equation Includes only participating chemical species.
Spectator Ions Nonreacting ions omitted from net ionic equations.
Solution Stoichiometry Molarity allows conversion to moles for reactions.
Arrhenius Acid Substance increasing hydrogen ion concentration in water.
Hydrochloric Acid Strong acid represented as HCl(aq).
Dissociation Process where acids release H+ ions in solution.
Polyprotic acids Acids with more than one acidic proton.
Diprotic acids Acids that release two protons in solution.
Arrhenius base Substance increasing hydroxide ions in solution.
Saponification Reaction of bases with fats to produce soap.
Neutralization Reaction Reaction between acid and base producing water and salt.
pH scale Measures acidity or basicity of a solution.
pH formula pH = -log[H+(aq)] for hydrogen ion concentration.
pOH forumla pOH = -log[OH-(aq)] for hydroxide ion concentration.
pH and pOH relationship pH + pOH = 14 at 25°C.
Titration Technique to determine unknown solution concentration.
Equivalence point Point where titration neutralizes the solution.
Gas-forming reactions Reactions producing gas as a product.
Oxidation-reduction reactions Reactions involving electron transfer between substances.
Oxidizing agent Substance that gains electrons in redox reactions
OIL Oxidation Is Loss of electrons.
RIG Reduction Is Gain of electrons
Precipitation reactions Reactions forming an insoluble solid from solutions.
Acidic solution Solution with pH less than 7.
Basic solution Solution with pH greater than 7.
Weak acids Acids that partially dissociate in solution.
Strong Acids Acids that completely dissociate in solution.
Weak bases Bases that partially dissociate or react with water.
Strong bases Bases that completely dissociate in solution.
Reducing agent Substance that loses electrons in redox reactions.
Created by: Erob22
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