Question

Part 1: Buffers Considering the acetic acid sodium acetate buffer, complete the table below NaOH added/mL. measured pH 0.0 20 Did the pH change a little or a lot when NaOH was added to the butter? Was the change you observed consistent with the action of a butter? For the ammonium chloride-ammonia buffer give the measured pH for the 50.0 mL of 0.10 Mammonia. Is this solution acidic, neutral, or basic? Did the pH of the ammonia increase or decrease when you added NH CI? Considering the ammonium chloride-ammonia buffer, complete the table below NaOH added/mL 0.0 measured pH Calculate the mass of NH CI (FM = 53.49 g/mol) needed to prepare 50.0 mL of 0.325 M NHCI. Use the Henderson-Hasselbalch equation to calculate the pH of a buffer containing 0.175 M HOCI (hypochlorous acid) and 0.105 M NaOCI (sodium hypochlorite). The K. for hypochlorous acid is 2.9 x 10

Answer 1

1000 © 50 w. P 0325(M) NHẠC Solution = 50xC1325 A. NH44 3 50X0.325 453.49 g Niach :The required mass of NH4Cl = 0.8699 Cans) 08693 Nac{ © ÞH = pka (HOL) + log [Naocel ka (HOCI)= 2.9x108 == log (219x1ö9) + log (0,105) [Nece Ol = 0105 CM) a nno trog 10.1757 [HOU] = 01175(M) = 7.54-0.22 = 7.32 The pH of Hoel - Naoel buffer solution = 7:32 Cans)