Thursday, May 15th: “A” DayFriday, May 16th: “B” Day

AgendaCollect Crossword PuzzleCollect Concept ReviewCh. 15 Review – pass back/warm-upCh. 15 Test

Looking Ahead Mon/Tues: Finals Review

Wed/Thurs: Fun Lab/Sr. Finals (Thurs) Fri/Tues: Sr. Finals (Fri)/2nd Semester Final

Jeopardy

Ch. 15 Review/Warm-up

#21 Write an equation for the reaction between hydrocyanic acid, HCN, and water. Label the acid, base, conjugate acid and conjugate base.

HCN + H2O ?

HCN + H2O CN- + H3O+

Acid Base Conjugate Base Conjugate Acid

Ch. 15 Review/Warm-up

#40 If the hydronium ion concentration of a solution is 1.63 X 10-8 M, what is the hydroxide ion concentration?

[H3O+] [OH-] = 1.00 X 10-14 M

(1.63 X 10-8 M) [OH-] = 1.00 X 10-14 M

[OH-] = 6.13 X 10-7 M

Ch. 15 Review/Warm-up# 47 If [OH-] of an aqueous solution is 0.0134 mol/L, what is the pH?

pH = -log [H3O+]

[H3O+] [OH-] = 1.00 X 10-14 M

[H3O+] (0.0134 M) = 1.00 X 10-14 M

[H3O+] = 7.46 X 10-13 M

pH = -log (7.46 X 10-13 M)

pH = 12.1

Ch. 15 Review/Warm-up#49 LiOH is a strong base. What is the pH of a 0.082

M LiOH solution?pH = -log [H3O+]

LiOH Li+ + OH-

0.082 M 0.082 M[H3O+] [OH-] = 1.00 X 10-14 M

[H3O+] (0.082 M) = 1.00 X 10-14 M

[H3O+] = 1.2 X 10-13 M

pH = -log (1.2 X 10-13 )

pH = 13 (2 sig figs)

Ch. 15 Review/Warm-up# 63 What is the hydroxide ion concentration in a

solution of pH 8.72?

[H3O+] = 10-pH

[H3O+] = 10-8.72

[H3O+] = 1.91 X 10-9 M

[H3O+] [OH-] = 1.00 X 10-14 M

1.91 X 10-9 M [OH-] = 1.00 X 10-14 M

[OH-] = 5.24 X 10-6 M

Ch. 15 Review/Warm-up#78 If 50.00 mL of 1.000 M HI is neutralized by

35.41 mL of KOH, what is the molarity of the KOH?

HI + H2O I- + H3O+

1.000 M 1.000 M(C OH-) (V OH-) = (C H3O+) (V OH-)

(C OH-) (0.03541 L) = (1.000 M) (0.05000 L)

(C OH-) = 1.412 M

KOH K+ + OH- 1.412 M 1.412 M

Ch. 15 Test“Acids and Bases”

You may use your notes, a periodic table, ion charts, and a calculator.