Question

(A) A solution has a hydroxide concentration of 122.846 mM. What is the pH?

(B)Calculate the pH of a 252.85 μM solution of HNO₃

(C)Calculate the pH of a 4.193 μM solution of KOH.

(D)Determine the pH of a 0.0302 mM solution of Mg(OH)₂

(E)What concentration of HCl is needed to have a solution with a pH = 3.52? Report your answer in mM.

Answer 1

Hope it will help you. Thank you.

Before start, Remember these points: pH = -log (H+) por= -log (our pH + POH = 14 Always: (A) 122.846 milli molar = 0.123 Molar solution. [OH-] = 0.123 - log [02-) = por= 0.91 PH 14-0.91 13.09. Ans (B) HNO3 → 100% dissociation 252.85 UM = 0.000253 Molar [ht] 2.538104 Molar solution Ans (C) -log[ht] = 3.60 =ph Kon > Strong Base: [on] = 4.193x166 Molar -log (OH) 5:38 pon Ans. - pH = 14-5:38 8.62 concentration 3.02 x 10-5 = 1.8x10-11 Ksp for Mg(OH)2 Mg(OH)2 ² Mg 2+ (aq. )+ 204 (aq) s 28 's is Solubility Ksp = = [Mg2+] [on-2 8.(28) 48² Ksp Vz 1.8x10111 (4.5 x1013) 8 = (or] =28= = 1.65*604 3,3x164 -log (04-) = 3.48 por PH = 14-3.48 = 10.52 Ans.