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48 Cards in this Set
- Front
- Back
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Dissociation
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The process in which ions separate
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Strong electrolyte
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A compound that is completely converted to ions when it forms an aqueous solution
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CHCOO⁻
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Acetate
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Precipitate
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Insoluble product
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Spectator ions
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Ions in a solution that remain after a reaction has taken place
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Net Ionic Equation
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An equation that includes only the symbols or formulas of ions in solution or compounds that undergo change
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Acid
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Any substance that increases the concentration of H⁺, hydrogen ions, when dissolved in pure water
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H₃O⁺
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Hydronium ion
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Strong Acid
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Acids that are entirely converted to ions (completely ionized) when dissolved in water
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Weak electrolytes
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Acids and other substances that ionize only slightly
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Examples of Strong Acids (Strong electrolytes)
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HCl Hydrochloric acid
HNO₃ Nitric Acid H₂SO₄ Sulfuric Acid HClO₄ Perchloric Acid HBr Hydrobromic Acid HI Hydroiodic Acid |
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Examples of Strong Bases (Strong electrolytes)
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LiOH Lithium hydroxide
NaOH Sodium hydroxide KOH Potassium hydroxide Ca(OH)₂ Calcium hydroxide Ba(OH)₂ Barium hydroxide Sr(OH)₂ Strontium hydroxide |
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Examples of Weak Acids (Weak electrolytes)
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H₃PO₄ Phosphoric Acid
CH₃COOH Acetic Acid H₂CO₃ Carbonic Acid HCN Hydrocyanic Acid C₆H₅COOH Benzoic acid |
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Examples of Weak Bases (Weak electrolytes)
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NH₃ Ammonia
CH₃NH₂ Methylamine |
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Amines
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Related to ammonia
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Base
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A substance that increases the concentration of hydroxide ions, OH⁻, when dissolved in pure water
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Ammonia
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NH₃; a common weak base that does not have an OH⁻ ion. It produces OH⁻ when combined with water:
NH₃ + H₂O -> NH₄⁺ + OH⁻ |
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Salt
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An ionic compound whose cation comes from a base and whose anion comes from an acid
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Three ways exchange reactions can occur
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formation of:
gas precipitate water |
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Reduced
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Gain of electrons
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Oxidized
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Loss of electrons
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Reducing Agent
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Donor of electrons, causes reduction, gets oxidized
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Oxidizing agent
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Recipient of electrons, causes oxidation, gets reduced
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An oxidation number compares the ______ of an uncombined atom with its actual _______ or its relative _______ in a compound
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An oxidation number compares the _charge_ of an uncombined atom with its actual _charge_ or its relative _charge_ in a compound
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The oxidation # of a pure element
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0
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The oxidation # of a monatomic ion equals:
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Its charge
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Hydrogen's oxidation # when combined with a metal
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+1
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Hydrogen's oxidation # when combined with a non-metal
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-1
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Fluorine's oxidation #:
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-1
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Oxygen's oxidation #:
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-2; except in peroxides (combined with H) when it is -1 (and H is +1)
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The sum of oxidation #s in a neutral compound equals . . .
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0
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The sum of oxidation #s in a polyatomic ion equals . . .
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. . . the charge on the ion
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Every reaction in which an element becomes combined in a compound is a . . .
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. . . redox reaction
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Metal Activity Series
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A ranking of relative reactivity of metals in displacement and other kinds of reactions
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An element higher in the activity series will ________ an element below it in the series from its compounds
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An element higher in the activity series will _displace_ an element below it in the series from its compounds
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The halogens, in oxidizing strength order
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F₂, Cl₂, Br₂, I₂
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Solution is a homogeneous mixture of a _______ and a _______
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Solution is a homogeneous mixture of a _solute_ and a _solvent_
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Solute
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The substance that has been dissolved
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Solvent
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The substance into which the solute has been dissolved
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Concentration of a solution
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The relative quantities of solute and solvent
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Molarity
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Relates the ratio of solute to the solution; expresses concentration
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Molarity formula
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Molarity = (Moles of solute) / (liters of solution)
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Symbol for molarity
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M
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Formula for calculating dilution or concentration of a slution
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MOLARITY (conc) * VOLUME (conc) = MOLARITY (dil) * VOLUME (dil)
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Standard solution
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A solution whose molarity/concentration is known accurately
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Equivalence point
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The point in a titration at which the stoichiometrically equivalent amount of standard solution has been added to an unknown
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End point
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The point in a titration at which an indicator is seen to change color
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Oxidation-Reduction reaction
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A reaction in which one reactant is oxidized while another is reduced.
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