NAME _____________________________ Quiz2 Ch 16
1) A 100.0 mL sample of 0.20 M HF is titrated with 0.10 M KOH. Determine the pH of the solution before the addition of any KOH. The Ka of HF is 3.5 x 10-4.
A) 4.15
B) 0.70
C) 2.08
D) 3.46
E) 1.00
2) A 100.0 mL sample of 0.20 M HF is titrated with 0.10 M KOH. Determine the pH of the solution after the addition of 100.0 mL of KOH. The Ka of HF is 3.5 × 10-4.
A) 2.08
B) 3.15
C) 4.33
D) 3.46
E) 4.15
3) A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3. Determine the pH of the solution after the addition of 100.0 mL of HNO3. The Kb of NH3 is 1.8 × 10-5.
A) 6.58 B) 10.56
C) 8.72
D) 3.44
E) 5.28
4) A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3. Determine the pH of the solution after the addition of 50.0 mL of HNO3. The Kb of NH3 is 1.8 × 10-5.
A) 4.74
B) 7.78
C) 7.05
D) 9.26
E) 10.34
5) A 100.0 mL sample of 0.20 M HF is titrated with 0.10 M KOH. Determine the pH of the solution after the addition of 300.0 mL of KOH. The Ka of HF is 3.5 × 10-4.
A) 12.40
B) 9.33
C) 5.06
D) 8.94
E) 12.00
1) [H+] = (Ka*C)^1/2
[H+] = (3.5*10^-4 * 0.20)^1/2
[H+] = 8.4*10^-3
Ph = -log[H+]
Ph = -log[8.4*10^-3]
Ph = 2.08
option C is correct
2)
no.of moles of HF = 0.20*0.1 lt = 0.02 moles
no. of moles of KOH = 0.1*0.1lt = 0.01 moles
0.01 moles of OH- will react with 0.01 moles of HF generating 0.01
moles of F- and leaving 0.01(0.02-0.01) moles of HF
Ph = Pka + log(0.01/0.01)
Pka = -log(Ka) = -log(3.5*10^-4)
Pka = 3.46
Ph = 3.46 + 0
Ph = 3.46
so option D is correct
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