Question

= surviving chem 2!! Ah really O ACIDS AND BASES Calculating the pH of a weak acid titrated with a strong b... An analytical chemist is titrating 71.7 mL of a 1.100 M solution of propionic acid (HC,H,CO2) with a 0.3000 M solution of NaOH. The pK, of propionic acid is 4.89. Calculate the pH of the acid solution after the chemist has added 294. mL of the NaOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of NaOH solution added. Round your answer to 2 decimal places. pH = 1 | xs ?

Answer 1

pacid] = MIVE + 1.100x 71.7 vity) tha +294) +0.216 M 0.241m Vita) a 0.300x294 Th7+294) 0.025m molarity of base left = 0.241-0.216 poh= log (oh) = -log(0.025) →160 PH +pOH =TH pH = ln-logo = 12.40