TheSwede
Feb12-12, 09:27 PM
1. The problem statement, all variables and given/known data
Three milliliters of a 2.0 M solution of HCL are added to 1 liter of buffer solution containing 0.40 moles of the weak acid, propanoic acid (Ka = 1.4 x 10-5) and .50 moles of its conjugate base, sodium propanate.
1) find the ph of the buffer solution
2) find the ph when the strong acid is added to the buffer solution
2. Relevant equations
Henderson Hasselbach equation: pH = Pka + log( A- / HA)
3. The attempt at a solution
1) to find the pKa -log(1.4 x 10-5) = 4.85
pH = 4.85 + log(.4/.5) = 4.75
is this correct?
2) clueless
Three milliliters of a 2.0 M solution of HCL are added to 1 liter of buffer solution containing 0.40 moles of the weak acid, propanoic acid (Ka = 1.4 x 10-5) and .50 moles of its conjugate base, sodium propanate.
1) find the ph of the buffer solution
2) find the ph when the strong acid is added to the buffer solution
2. Relevant equations
Henderson Hasselbach equation: pH = Pka + log( A- / HA)
3. The attempt at a solution
1) to find the pKa -log(1.4 x 10-5) = 4.85
pH = 4.85 + log(.4/.5) = 4.75
is this correct?
2) clueless