In: Chemistry
A buffer contains 0.11 mol of propionic acid (C2H5COOH) and 0.17 mol of sodium propionate (C2H5COONa) in 1.20 L. What is the pH of this buffer?
What is the pH of the buffer after the addition of 0.02 mol of NaOH?
What is the pH of the buffer after the addition of 0.02 mol of HI?
no of moles of C2H5COOH = 0.11moles
molarity of C2H5COOH = no of moles/volume in L
= 0.11/1.2 = 0.0917 M
no of moles of C2H5COONa = 0.17moles
molarity of C2H5COONa = no of moles/volume in L
= 0.17/1.2 = 0.1417M
Pka of C2H5COOH = 4.87
PH = Pka + log[C2H5COONa]/[C2H5COOH]
= 4.87 + log0.1417/0.0917
= 4.87 + 0.189
= 5.06>>>>answer
no of moles of C2H5COOH after addition of 0.02moles of NaOH = 0.11-0.02 = 0.09moles
no of moles of C2H5COONa after addition of 0.02moles of NaOH = 0.17+0.02 = 0.19moles
PH = Pka + log[C2H5COONa]/[C2H5COOH]
= 4.87 + log0.19/0.09
= 4.87 + 0.3245
= 5.1945>>>>answer
no of moles of C2H5COOH after addition of 0.02moles of HCl = 0.11+0.02 = 0.13moles
no of moles of C2H5COONa after addition of 0.02moles of HCl = 0.17-0.02 = 0.15moles
PH = Pka + log[C2H5COONa]/[C2H5COOH]
= 4.87 + log0.15/0.13
= 4.87 + 0.06215
= 4.932>>>>answer