ap chem ch. 4

sour taste

• react with metals to produce hydrogen gas

• electrolytes (think electrochemical cells)

• affect indicators (of course)

conduct electric current when dissolved in water (galvanic/voltaic and electrolytic cells)

a solution used to see when the endpoint of a titration reaction has been reached (by pH, but it does not affect the pH). indicators only work at a certain pH range.

• bitter taste

• forms electrolytes

• affect indicators (of course)

acids produce H+ ions when dissolved (ionized) in water and bases produce OH- when dissolved (ionized) in water

separation of ions in a solution

neutral molecules (covalent) react with water to form ions

acids donate protons (H+) in a chemical reaction and bases accept protons (H+) in a chemical reaction

the particle left over after the acid donates a proton

the particle left over after the base accepts a proton

an acid is any substance that accepts an electron pair and a base is any substance that donates an electron pair. use electron dot diagrams to determine if a substance is a lewis acid or base

HO(X)/H(X): where “X” is any element

• if X is more electronegative, then it acts as a bronsted-lowry acid, giving up the H+

• if X is more electropositive, then it acts as a bronsted-lowry base, accepting the H+

• so, nonmetals tend to form acids while metals tend to form bases when dissolved in water

  • HCl + H2O -→ Cl- + H3O+

  • NaOH + H2O -→ NaH2O + OH- (remember, Na is a spectator ion)

• not all acids completely ionize in water (ex. weak acids or weak bases)

acids and bases that have had water removed

• acids:

  • SO2 + H2O -→ H2SO3

• bases:

  • Na2O + H2O -→ 2NaOH

an ionic compound that does not consist of H+ or OH-

• an acid that reacts with a base to produce a salt and water

• double displacement

• NaOH + HCl -→ NaCl + H2O

acids that go through multiple steps of ionization; second step always results in a weak acid

• H2SO4 (2 steps)

• H3PO4 (3 steps)

describes the extent to which a solid will dissolve in water

increase in oxidation number (decrease in electrons)

decrease in oxidation number (increase in electrons)

combination of half-oxidation and half-reduction equations; one chemical oxidizes/gains change and and the other reduces/looses charge

oxidizing agent is the one that gets reduced (does the oxidizing), reducing agent is the one that gets oxidized (does the reducing)