15.1-15.2: Precipitation/Dissolution Equilibria,

• The solubility product constant (Ksp) is the equilibrium constant for the dissociation reaction.
• Soluble salts have high Ksp values while insoluble salts have low Ksp values.
• What is Ksp?


  The solubility product constant,  the equilibrium constant for a solid substance dissolving in an aqueous solution
• Ksp is ___ and ___ dependent

  solute, solvent
• What is molarity?


  mol solute/L solution
• What is the solubility product Ksp equilibrium formula

  MpXn(s) --> pM^n+(aq) + nX^p-(aq)
• Ksp =


  [M^n+]^p[X^p]^n
• What does it mean that Q > K

  Too much product, will shift towards reactants and precipitates forms
• What does it mean that Q < K or Q = K

  No precipitation is formed
• What is the common ion effect?

  Shift in equilibrium caused by the addition of a common ion. The solubility of the salt in a solution that already contains one or the ions in the salt will be lower than in pure H2O.
• Compare to pure H2O ([OH-] = 1.0x10^-12 M) it is ___ in a basic solution ([OH-] > 1.0x10^-12 M)

  less soluble
• Compare to pure H2O ([OH-] = 1.0x10^-12 M) it is ___ in an acidic solution ([OH-] < 1.0x10^-12 M)

  soluble
• What are coordinate covalent bonds?

  Shared electrons from one atom are donated to a bond. Bonds formed between chemical species where both e- come from one of the species
• Lewis bases ___ e- to bond and Lewis acids ___ e- during bond formation

  donates, accept
• What are ligands?

  Molecules or ions that bind to a central metal atom or ion.
• Non-metal atomic anions/cations =

  acid-base properties of their conjugate acids
• Metal atomic cations are ___, highly charged, usually high ____ and act as ___

  small, electronegativity, acids
• Metal atomic ions: ___, low charge, usually low ____, will act as

  large, electronegativity, neutral
• Be^2+ acts as a weak acid because of it's...

  small size
• Bronsted-Lowry acids/bases will act as a Lewis acid/base but is it true for the opposite?


  No
• What can't compounds act as?

  Lewis acid/bases
• How do you write half reactions in an acidic solution?

  1.Balance elements expect oxygen and hydrogen, 2. Balance oxygen by adding H2O to which side has few O2 atoms, 3. Balance H+ by adding to side with less H+, add e- to which side is gaining or losing e-
• How to write half reactions in a basic solution?

  Balance the atoms and charges in the half reaction, then add OH- ions to balance the hydrogen atoms and water molecules to balance the oxygen atoms. Then subtract H2O from each side to get rid of one
• Reactant being oxidized =

  reducing agent
• reactant being reduced =

  oxidized agent
• What doe AOCR stand for?

  anode, oxidation, cathode, reduction