1. An aqueous solution contains 0.150 M HCl at 25.0 °C. The pH of the solution i
ID: 959990 • Letter: 1
Question
1. An aqueous solution contains 0.150 M HCl at 25.0 °C. The pH of the solution is ________.
2. Which solution has the higher pH, a 0.001 M solution of NaOH or a 0.001 M solution of Ba(OH)2?
3. calculate pH for all of the following:
a. 7.6×103 M HBr, b. 1.48 g of HNO3 in 480 mL of solution, c. 4.00 mL of 0.210 M HClO4 diluted to 46.0 mL, d. A solution formed by mixing 11.0 mL of 0.110 M HBr with 23.0 mL of 0.220 M HCl.
4. Calculate the concentration of an aqueous solution of NaOH that has a pH of 11.41. [NaOH] =?
5. The Ka of hypochlorous acid (HClO) is 3.0 10-8 at 25.0 °C. What is the percent ionization of hypochlorous acid in a 0.015 M aqueous solution of HClO at 25.0°C?
0.150 0.82 13.00 7.00 1.00Explanation / Answer
1 )
[H+] = 0.150
pH = -log [H+] = -log (0.150)
pH = 0.82 ---------------------> answer
2)
NaOH molariyt = 0.001
pOH = 3
pH = 11
Ba(OH)2 , OH- cocnetratrion =0.001 x 2 = 0.002 M
pOH = -log[OH-] = 2.70
pH = 11.3
so 0.001 M solution of Ba(OH)2 higher pH
3)
a ) answer : pH = 2.12
b) answer : pH = 1.32
c) answer : pH = 2.38
d) answer : pH = 0.73
4)
pH = 11.41
pOH = 2.59
[OH-] = 10^-pOH
[OH-] = 2.57 x 10^-3 M
[NaOH] = 2.57 x 10^-3 M
5)
answer : 0.14
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