In: Chemistry
A solution of volume 70.0 mL contains 16.0 mmolHCHO2 and 8.50 mmol NaCHO2.
Part A
What is the pH of this solution?
Express your answer using two decimal places.
Part B
If 0.25 mmol Ba(OH)2 is added to the solution, what will be the pH?
Express your answer using two decimal places.
Part C
If 1.10 mL of 12 M HCl is added to the original solution, what will be the pH?
Express your answer using two decimal places.
Pka of HCO2H = 3.75
no of mmoles of HCO2Na = 8.5mmoles
no of mmoles of HCO2H = 16 mmoles
PH = PKa + log[HCO2Na]/[HCO2H]
= 3.75 + log8.5/16
= 3.75-0.2747 = 3.4753
part-B
no of mmoles of HCO2Na after addition of 0.25 mmoles of Ba(OH)2 = 8.5+0.25 = 8.75mmoles
no of mmoles of HCO2H after addition of 0.25 mmoles of Ba(OH)2 = 16-0.25 = 15.75 mmoles
PH = Pka + log[HCO2Na]/[HCO2H]
= 3.75 + log8.75/15.75
= 3.75-0.2552 = 3.4948>>>answer
part-C
no of mmoles of HCl = molarity * volume in ml
= 12*1.1 = 13.2mmoles
The excess of HCl total converted HCO2Na to HCO2H
no of mmoles of excess = 13.2-8.5 = 4.7 mmoles
conc of HCl = no of mmole of HCl/total volume in ml = 4.7/70.1 = 0.067M
[H^+] = 0.067M
PH = -log[H^+]
= -log0.067
= 1.1739 >>>>>answer