Question

a. Calculate the pH of 200 mL of a 1.50 M solution of HCl?

b. What mass of LiOH must be added to 750.0 mL of 0.0550 M HCl to produce a solution having a pOH of 11.500?

c. A chemist had 2.000 L of a 0.00120 M KOH solution. What mass of HCl(g) would have to be added to the KOH solution to produce a solution having a pH of 10.875?

Answer 1

(a Gronketa of Ha = 1.5m. as Hel is any and so [u] = 15m pH = -logi (HT) o logio 15 - 0176 2.5 Bota n. 3 pH = 14 - port = 14 - 11.5 = [41] = 10-14 10-25 = 0.00 32M 1st let, the x mol of tiot ne for to add on Morate of 40 C 2 mot mof holy & Hel = 750x108x8-055 nafar 0004 I notes all titube by Lioa, ha test = (0.091 + x)onder. prolarity: 10-091-2 ) moisht 0.750 Non 0.091-ka 0.0032 ort - 60386 Mas of Liott = 0.0386 ml x 23.95gfoot - 0.9249

o ) BH = 10.875 in so it is basic pl. that means Hel won't neutrolire completely NOW, 2477pol = 14--00875" = 3.125 You-] = 10-3 125 0.00075 fele de mut Hel regent, & o mo of tiks of Kol = 2 ut f 0.0012 not feet = 0.0024 mola exes Ot & (0.002A - 2) mola out) - 1 0.0029-x) M 0.0024 x = 0.00025 2 x = 0.0oog. no of man of Hell = Armoul of ACIE 0.00g rol 0.009 mM x 3 8.46964 - 0.033g