SCH 3U1 Unit 6 Assign
2 – ACID-BASE pH measurements
1. a) In pure water, what is a) [H+] =...................................pH=......... b) [OH–] =.................................... pOH =.......
b) Is water a weak or strong electrolyte (poor/good conductor)
2. a) If you add acids to water what would happen to [H+] ?
..............................................
b) If you add bases to water what would happen to [OH–] ?
3.
+
* pH = –log10[H ]
..............................................
–
and
..............................................
pOH = -log10[OH ]
and
pH + pOH = 14
a) In a 1.0 x 10–1 M HCl sol’n, what is
i) [H+] =........................................
ii) pH = ....................
b) In a 4.0 x 10–1 M HCl sol’n, what is
i) [H+] =........................................
ii) pH = ....................
c) In a 1.0 x 10–3 M H2SO4 sol’n, what is
i) [H+] =.......................................
ii) pH = ....................
d) In a 4.0 x 10–3 M HC2H3O2 sol’n, what is i) [H+] =........................................
ii) pH = ....................
e) In a 1.5 x 10–4 M HNO3 sol’n, what is
i) [H+] =........................................
ii) pH =....................
f) In a 1.0 x 10–1 M NaOH sol’n, what is
i) [OH–] =.....................................
ii) pOH =........... pH = ...........
g) In a 4.0 x 10–1 M KOH sol’n, what is
i) [OH–] =....................................
ii) pOH =........... pH = ...........
h) In a 2.5 x 10–2 M NaOH sol’n, what is
i) [OH–] =....................................
ii) pOH =........... pH = ...........
i) In a 1.5 x 10–4 M Ba(OH)2 sol’n, what is i) [OH–] =....................................
ii) pOH =........... pH = ...........
4. ** if pH = -log10[H+] then [H+] = 10–pH
[H+]
[OH–]
pH
if pOH = -log10[OH–] then [OH–] = 10–pOH
pOH
[H+]
[OH–]
1 x 10–2
2 x 10–1
2 x 10–3
4 x 10–2
1 x 10–6
5 x 10–5
1.8
pH
POH
13.4
2.8
10.8
5. Calculate the pH of the following sol'ns ( all mol/L )
a) [H+] = 7 x 10–9 pH= ...................... b) [H+] = 5.2 x 10–3 pH= ...................... c) [OH–] = 0.18 pH= .....................
d) [OH–] = 7 x 10–4 pH= ......................e) [OH–] = 5.2 x 10–5 pH= ..................... f) [H+] = 0.18 pH= ......................
g) [H+] = 3 x 10–2 pH= ...................... h) [OH–] = 2.6x10–13 . pH= ....................
6. Calculate [H+] in solutions whose
c) pH =1.8
a) pH = 3.0 [H+] = .......................... b) pH = 4.6 . [H+] = ..............................
[H+] = ....................... d) pOH =11.5 [H+] = ........................ e) pH =7.315 [H+] = .........…….............
7. 5.0 g of HClO4 are dissolved in 200 mL of water, calculate the pH of this solution. (do on the back & show all your work)
8. 5.0 g of potassium hydroxide are dissolved in 200 mL of water, calculate the pH of this solution (do on the back &
show all your work)