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Drill: Determine the pH of 0.25 M HZ. K aHZ = 2.5 x 10 -7. Buffer Solutions. Buffer Solution. A solution that resists changes in pH. Buffer Solution. Made from the combination of a weak acid & its salt. Buffer Solution. Made from the combination of a weak base & its salt. Buffer Examples. - PowerPoint PPT Presentation
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Drill: Determine the pH of 0.25 M HZ.KaHZ = 2.5 x 10-7
Buffer Solutions
Buffer Solution
•A solution that resists changes in
pH
Buffer Solution•Made from the combination of a weak acid & its
salt
Buffer Solution•Made from the combination of a weak base & its
salt
Buffer Examples•Mix acetic acid &
sodium acetate
•Mix ammonia & ammonium chloride
Buffer Solution•A buffer solution
works best when the acid to salt ratio is
1 : 1
Buffer Solution•A buffer solution
works best when the base to salt ratio is
1 : 1
Buffer Solution•The buffering capacity of a solution works best when the pH is near the
pKa
pKa or pKb
•pKa = - log Ka
•pKb = - log Kb
Buffer Problems•Calculate the pH of a solution containing 0.10
M HAc in 0.10 M NaAc: Ka = 1.8 x 10-5
Buffer Problems•Calculate the pH of 0.10 M NH3 in 0.20
M NH4NO3:
•Kb = 1.8 x 10-5
Buffer ProblemsCalculate the pH of a
solution containing
0.10 M HBz in 0.20 M NaBz: Ka = 6.4 x 10-5
Buffer ProblemsCalculate the pH of a
solution containing
0.50 M HQ in 0.10 M NaQ: Ka = 4.0 x 10-5
DrillCalculate the pH of a
solution containing
0.30 M HZ in 0.10 M NaZ: Ka = 3.0 x 10-5
Lab Requirements• To make accurate
measurements, we must have solutions with accurately measured concentrations
Standard Solution•A solution with known concentration
•2.004 M HCl
STD ProblemsCalculate the mass of KHP (MW = 204.23)
required to make 1.0 L of 0.100 M KHP
Henderson-Hasselbach Eq
[A-]
[HA]pH = pKa + log
Henderson-Hasselbach Eq
[B+]
[B]pOH = pKb+ log
Buffer Problems•Calculate the salt to acid
ratio to make a buffer solution with pH = 5.0
•Ka for HBZ = 2.0 x 10-5
Buffer ProblemsCalculate the salt to base
ratio to make a buffer solution with pH = 9.48
• Kb for MOH = 2.0 x 10-5
Calculate the HCO3- to
H2CO3 ratio in blood with pH = 7.40
•Ka1 for H2CO3 = 4.4 x 10-7
150 ml of 0.10 M NaOH is added to 100.0 ml of 0.10 M H2CO3. Calculate all.
• Ka1 for H2CO3 = 4.4 x 10-7
• Ka2 for H2CO3 = 4.7 x 10-11