Buffers
What is the pH of a buffer solution where [HA] = [A-]?
pH=pKa
How do we calculate volume at the equivalence point of a monoprotic acid and monoprotic base?
CaVa=CbVb or using mole ratio
With hydrolysis how can I tell a salt is acidic
The anion will be from a strong acid
Sodium fluoride is added to a solution of hydrofluoric acid. What happens to the pH of the solution upon the the addition of NaF?
pH increases
pH decreases
pH increases
How do we pick indicators for an acid-base titration? i.e either weak acid-strong base or weak base-strong acid
Looking at the pH at the equivalence point
For a salt to be neutral what must it be made of
The cation of a strong base and the anion of a strong acid
A buffer solution contains acid as one component of the buffer and a base as the other. Can these components be HCl and NaOH?
No a buffer component needs to have a weak acid and its conjugate base or a weak base and its conjugate acid. HCl is a strong acid and NaOH is a strong base
What controls the pH of a weak acid-strong base titration at the equivalence point
The conjugate base of the weak acid does
Which compound is more soluble and why?
a) BaSO4 (Ksp = 1.1·10-10) or PbSO4 (Ksp = 1.6·10-8)
PbSO4 is more soluble because it has a higher Ksp value
How can we improve buffer capacity i.e how can we make buffers better at resisiting pH
By increasing the concentration of the weak acid and the weak base
In a weak base, strong acid titration, what controls the pH after the equivalence point?
The strong acid does
Calculate the molar solubility of silver arsenate, given that
Ag3AsO4(s) ↔ 3Ag+(aq) + AsO43-(aq) Ksp = 1.0·10-22
Hint: make the ICE table and find x
1.4*10^-6