UNIT 8 | STUDY GUIDE
ACIDS & BASES
acids and bases
15-1, 15-2, 15-3, 16-1, 16-2 | Section Reviews
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acid-base theories
o Arrhenius, Brønsted-Lowry, Lewis
auto-ionization of water
hydrogen ion / proton (H1+), hydroxide
(OH1-), hydronium ion (H3O1+)
strong acid / base vs. weak acid / base
conjugate acid, conjugate base
acid + base  salt + water
Kwater = 1.00 X 10-14 M2= [H1+][ OH1-]
pH / pOH scales and calculations
neutralization reactions
o pH / pOH of resulting solution
titrations (setup and calculation)
Chapter 15 Review: 1, 2, 5, 7, 8, 9, 10, 13, 14,
17, 18, 19, 20, 26*, 27*, 29*, 34*, 37
*full formula equations only
Chapter 16 Review: 2, 5, 6, 15, 16, 17, 18, 19,
20, 21, 22, 23, 24, 25, 26, 27, 28, 29, 30, 31,
32, 33, 34, 35, 36, 37
answers to selected problems
Chapter 15 Review:
17) a: hydrochloric acid // b: hydrosulfuric
acid
18) a: nitric acid // b: sulfurous acid //
c: chloric acid // d: nitrous acid
19) a: HF // b: HI
20) a: HBrO4 // b: HClO2 // c: H3PO4 //
d: HClO
26) a: 1 HCl + 1 NaOH  1 NaCl + 1 H2O
// b: 1 HNO3 + 1 KOH  1 KNO3 +
1 H2O // c: 1 Ca(OH)2 + 2 HNO3 
1 Ca(NO3)2 + 2 H2O // d: 1 Mg(OH)2 +
2 HCl  1 MgCl2 + 2 H2O
27) 2 H3PO4 + 3 Mg(OH)2  1 Mg3(PO4)2 +
6 H2O
29) a: 1 HClO4 + 1 RbOH  1 RbClO4 +
1 H2O // b: 1 H2SO4 + 1 Ba(OH)2 
1 BaSO4 + 2 H2O // c: 2 HCl +
1 Ca(OH)2  1 CaCl2 + 2 H2O //
d: 1 H2SO4 + 2 KOH  1 K2SO4 + 2 H2O
34) a: 1 HNO3 + 1 LiOH  1 LiNO3 + 1 H2O
37) a: hydrofluoric acid // b: HC2H3O2 //
c: H3PO3 // d: perchloric acid //
e: phosphoric acid // f: HBr //
g: hypochlorous acid // h: carbonic acid
// i: H2SO4
CHEMISTRY MYP | KHAN
Chapter 16 Review:
15) a: 0.03 M H3O1+; 3 x 10-13 M OH1- //
b: 1 x 10-10 M H3O1+; 1 x 10-4 M OH1// c: 0.01 M H3O1+; 1 x 10-12 M OH1- //
d: 5 x 10-13 M H3O1+; 0.02 M OH116) a: 2.0 // b: 3.0 // c: 5.0 // d: 4.0
17) a: 8.0 // b: 5.0 // c: 12 // d: 7.0
18) a: 12 // b: 11 // c: 10.
19) a: 4.7 // b: 6.3 // c: 2.4
20) a: 1.0 x 10-3 M H3O1+ // b: 1.00 x
10-7 M H3O1+ // c: 1.00 x 10-11 M H3O1+
// d: 1.0 x 10-5 M H3O1+
21) a: 1.00 x 10-7 M OH1- // b: 1.000 x
10-3 M OH1- // c: 1.00 x 10-9 M OH1- //
d: 1.00 x 10-8 M OH122) a: 5.89 x 10-5 M H3O1+ // b: 2.24 x
10-8 M H3O1+ // c: 3.31 x 10-10 M H3O1+
23) a: 2.00 x 10-3 M H3O1+ // b: 5.01 x
10-12 M OH1- // c: 0.0110 mol HNO3 //
d: 0.691 g HNO3 // e: 0.702 mL conc
HNO3
24) a: 1.0 mol NaOH // b: 0.75 mol HNO3
// c: 0.10 mol Ba(OH)2 // d: 0.90 mol
H2SO4
25) 0.0750 M KOH 26) 0.0302 M HNO3
27) a: 8.0 x 10-4 M OH1- // b: 1.3 x 10-11 M
H3O1+
28) a: 7.0 // b: 3.0 // c: 12 // d: 5.0
29) 1.0 x 10-6 M H3O1+
30) 10.
31) a: 10. // b: 3.16 x 10-3 M H3O1+
32) a: 1.1 x 10-4 M OH1- // b: 9.3 x 10-11 M
H3O1+
33) a: 1.26 x 10-9 M H3O1+ // b: 7.94 x
10-6 M OH134) 4.8
35) 0.0106 M HCl
36) 9.00 x 10-4 M Ca(OH)2
37) 2.97 x 10-2 M HNO3
calculate the pH of final solutions
1) 125 mL of 0.0300 M nitric acid with 125
mL of 0.0300 M barium hydroxide.
2) 90.0 mL of 0.0145 M potassium
hydroxide with 50.0 mL of 0.0275 M
perchloric acid.
3) 5.00 mL of 0.160 M hydrobromic acid
with 10.00 mL of 0.110 M sodium
hydroxide.
4) 220. mL of 0.150 M sulfuric acid with 150
mL of 0.220 strontium hydroxide.