Acids and Bases Flashcards

Question

How to get the following for weak acid with strong base - A. Initial pH B. Buffer region C. Equivalence point D. Overtitration

Answer 1

A. Only HA is present, find pH of weak acid B. HA and A- present, find pH with PUG followed by ICE/HH C. Only A- present, find pH with PUG followed by ICE, need Kb of conjugate base and consider dilution D. OH- and A- present, approximate as strong base PUG and consider dilution

Answer 2

A. Only base is present, find pH of weak base B. HB+ and B+ present, find pH with PUG followed by ICE/HH C. Only HB+ present, find pH with PUG followed by ICE only for equilibrium with Ka and consider dilution D. H30+ and HB+, use PUG, approximate as strong acid and consider dilution

Answer 3

Resist change in pH over a pH range of 2 values by consuming incoming acids with a base and vice versa, then re-equilibrating

Answer 4

1.) Add acid and conjugate base pair together 2.) Add until weak acid/base and conjugate acid/base are left

Answer 5

1.) Use stoichiometry to find the equivalence point (use L of one chemical and mole-to-mole ratio to get M) OR 2.) Use initial pH and experimentally determined Ka (use ICE table and add/subtract Ka/Kb and use Ka/Kb = [A][B]/[C] and solve for y to get M

Answer 6

1.) Net ionic equation with water 2.) Use 10 to the -pH/pOH for Ka/Kb 3.) Set up ICE using M and +/- Ka/Kb 4.) Solve for Ka/Kb using Ka/Kb = [A][B]/[C] Secondary Way (10 to the - pH) squared / (M - 10 to the -pH)

Answer 7

1.) pH= -log[M] 2.) Write out last dissociation 3.) Use ICE table with +/- M and Ka/Kb and solve for x 4.) You now have [H3O]/[OH] and can solve for pH

Answer 8

1.) Multiply ml by M to get mmol 2.) Net ionic equation mixing analyte/titrant (take out spectators) 3.) Use PUG table using mmol and +/- mmol titrant 4.) Use HH to calculate pH

Answer 9

1.) Get pKa/pKb using M 2.) Use HH with pKa/pKb and pH. Solve for (A-/HA or HB/B) and exponentiate to get acid:base ratio 3.) Convert g to ml x mole to mole ratio x M to get ml

Answer 10

1.) Get pH using Ka/Kb 2.) +/- 1 pH to find out range 3.) Use either end of +/- 1 as pH and the pH as pKa in HH equation and solve for (A/HA or HB/B) by expotentiating. Do for both extrema

Answer 11

Account for moles and multiply by them

Answer 12

Dissolves to a small extent

Answer 13

Dissolves to a large extent

Answer 14

The more the compound dissolves

Answer 15

1) Set up ICE table with dissociation (be sure to account for moles) 2) Ksp = [X] to the n [Y] to the m 3)Set it equal to given Ksp and solve for x 4) Multiply it by moles of ion if needed

Answer 16

Qsp = Ksp saturated solution; no more ions can be dissolved Qsp < Ksp unsaturated solution; more ions can be dissolved Qsp > Ksp supersaturated solution; no more ions will dissolve and a precipitate forms

Answer 17

Molarity of a saturated solution, max concentration of your compound

Answer 18

Multiply molar solubility by molar mass of compound

Answer 19

1) Write out equation and use the following for the potential solid that forms 2) Use M1V1 = M2V2, with V total for V2 for first ion (metal) 3) Use M1V1 = M2V2 for OH and multiply M by moles 4) Qsp = [Metal] to n and [OH] to m 5) Determine if precipitate forms given Ksp/Qsp rules

Answer 20

1) set up ICE table for compound in water and in a solution 2) Use just x for water and molarity +/- X for solution

Answer 21

If pH of conj acid/base is greater than 7 then solubility decreases If pH of conj acid/base is less than 7 then solubility increases