A strong acid or base _____________ in aqueous solution.
Completely dissociates
100
A weak acid or base ______________ in aqueous solution.
Partially dissociates
100
A buffer solution is one which ________ changes in pH when small quantities of an acid or a base are added to it.
Resists
100
What is the name of the symbol 'Ksp'?
Solubility product
200
Addition of NaF(aq) to a solution of HF(aq) would make the solution ______ acidic
less
200
10g of Sodium Iodoacetate are dissolved in 100ml of water. (pKa Iodoacetic acid is 3.12)
a) based on the information given above, is the solution acidic, basic, or neutral?
basic
200
Name a substance that would create a buffered solution when paired with NaC2H3CO2(aq)
Acetic Acid HC2H3CO2
200
Which of the following solids has the highest solubility in pure water?
a) Cd(OH)2; Ksp = 5.9x10^-15
b) Pb(OH)2; Ksp = 1.2x10^-15
c) Fe(OH)2; Ksp = 1.8x10^-15
a) Cd(OH)2
300
Calculate the pH of a solution that is 1.00M HNO2 and 1.00M NaNO2; Ka HNO2 = 4.0 x 10^-4
pH = 3.40
300
A 0.15 M solution of a weak acid is 3.0% dissociated. Calculate Ka.
Hint: think about HA<->H(pos) + A(neg)
1.4 x 10^-4
300
Calculate the pH of a mixture containing 0.100 M HC3H5O2 and 0.100M NaC3H5O2.
pH = 4.89
300
Which of the following solids has the LOWEST solubility in pure water?
a) Ag3PO4; Ksp = 1.8 x 10^-18
b) Co(OH)2; Ksp = 2.5 x 10^ -16
c) AgI; Ksp = 1.5 x 10^-16
AgI, 1.2 x 10^-8 M
400
Name six of the seven strong acids.
HI, HBr, HCl, HNO3, H2SO4, HClO4, HClO3
400
Calculate the pH of a solution of 0.050M NaCN Ka = 6.2 x 10^-10.
Remember CN- acts as a base in solution
Kw=Ka*Kb
pH= 10.95
400
How many moles of NaOH must be added to 1.0L of 2.0M HC2H3O2 to produce a solution buffered at the specified pH.
remember: pH = pKa + log([A-]/[HA]).
pKa HC2H3O2=4.74
solve for... pH=pKa
1.0 mol NaOH
400
The Ksp of silver sulfate (Ag2SO4) is 1.2 x 10^-5. Calculate the solubility of silver sulfate in each of the following.
a. Pure Water
b. 0.10M AgNO3
c. 0.20M K2SO4