Date Quiz 8-1 Acids and Bases pH
Name __________________________________________________ Period ________ Date ______________________ Quiz 8-1 Acids and Bases pH – Version 9
Total Points: _______/10
1. (a) Name the acid HBr. Hydrobromic acid
(½ pt)
(b) Write the balanced dissociation equation for HBr in an aqueous solution. 𝐻𝐵𝑟(𝑎𝑞) → 𝐻 + (𝑎𝑞) + 𝐵𝑟 − (𝑎𝑞)
(c) Determine the [H+] in 0.0500 M HBr.
(½ pt)
Answer and Units (½ pt)
Show Work (1/4 pt)
Sigfigs (1/4 pt)
Ans. & U (½ pt)
Work (1/4)
SF (1/4)
Ans. & U (½ pt)
Work (1/4)
SF (1/4)
Ans. & U (½ pt)
Work (1/4)
SF (1/4 pt)
𝐻𝐵𝑟(𝑎𝑞) → 𝐻 + (𝑎𝑞) + 𝐵𝑟 − (𝑎𝑞) 0.0500 M 0.0500 M 0.0500 M [𝐻 + ] = 0.0500 𝑀 (d) Calculate the pH of 0.0500 M HBr. 𝑝𝐻 = −𝑙𝑜𝑔[𝐻 + ] = −𝑙𝑜𝑔(0.0500) = 1.301
(e) Calculate the pOH of 0.0500 M HBr. 𝑝𝐻 + 𝑝𝑂𝐻 = 14.00 𝑝𝑂𝐻 = 14.00 − 𝑝𝐻 = 14.00 − 1.301 = 12.699 (f) Calculate the [OH-] in 0.0500 M HBr. [𝑂𝐻 − ] = 10−𝑝𝑂𝐻 = 10−12.699 = 2.00 × 10−13 𝑀 2. (a) Write the chemical formula of barium hydroxide. Ba(OH)2
(½ pt)
(b) Write the balanced dissociation equation for barium hydroxide in an aqueous solution. 𝐵𝑎(𝑂𝐻)2 (𝑎𝑞) → 𝐵𝑎2+ (𝑎𝑞) + 2 𝑂𝐻 − (𝑎𝑞)
(½ pt)
(g) Determine the [H+] in barium hydroxide pH 10.60 [𝐻 + ] = 10−𝑝𝐻 = 10−10.60 = 2.5 × 10−11 𝑀
Ans. & U (½ pt)
Work (1/4)
SF (1/4 pt)
(h) Calculate the pOH of barium hydroxide pH 10.60 𝑝𝐻 + 𝑝𝑂𝐻 = 14.00
Ans. & U (½ pt)
Work (1/4)
SF (1/4 pt)
Ans. & U (½ pt)
Work (1/4)
SF (1/4 pt)
𝑝𝑂𝐻 = 14.00 − 𝑝𝐻 = 14.00 − 10.60 = 3.40 (i) Calculate the [OH-] in barium hydroxide pH 10.60 [𝑂𝐻 − ] = 10−𝑝𝑂𝐻 = 10−3.40 = 4.0 × 10−4 𝑀
Name __________________________________________________ Period ________ Date ______________________ 3. When pH paper is added to HBr what color does it turn? red
(½ pt)
4. When pH paper is added to a barium hydroxide solution, what color does it turn? blue
(½ pt)
Total Points: _______/10
1. (a) Name the acid HBr. Hydrobromic acid
(½ pt)
(b) Write the balanced dissociation equation for HBr in an aqueous solution. 𝐻𝐵𝑟(𝑎𝑞) → 𝐻 + (𝑎𝑞) + 𝐵𝑟 − (𝑎𝑞)
(c) Determine the [H+] in 0.0500 M HBr.
(½ pt)
Answer and Units (½ pt)
Show Work (1/4 pt)
Sigfigs (1/4 pt)
Ans. & U (½ pt)
Work (1/4)
SF (1/4)
Ans. & U (½ pt)
Work (1/4)
SF (1/4)
Ans. & U (½ pt)
Work (1/4)
SF (1/4 pt)
𝐻𝐵𝑟(𝑎𝑞) → 𝐻 + (𝑎𝑞) + 𝐵𝑟 − (𝑎𝑞) 0.0500 M 0.0500 M 0.0500 M [𝐻 + ] = 0.0500 𝑀 (d) Calculate the pH of 0.0500 M HBr. 𝑝𝐻 = −𝑙𝑜𝑔[𝐻 + ] = −𝑙𝑜𝑔(0.0500) = 1.301
(e) Calculate the pOH of 0.0500 M HBr. 𝑝𝐻 + 𝑝𝑂𝐻 = 14.00 𝑝𝑂𝐻 = 14.00 − 𝑝𝐻 = 14.00 − 1.301 = 12.699 (f) Calculate the [OH-] in 0.0500 M HBr. [𝑂𝐻 − ] = 10−𝑝𝑂𝐻 = 10−12.699 = 2.00 × 10−13 𝑀 2. (a) Write the chemical formula of barium hydroxide. Ba(OH)2
(½ pt)
(b) Write the balanced dissociation equation for barium hydroxide in an aqueous solution. 𝐵𝑎(𝑂𝐻)2 (𝑎𝑞) → 𝐵𝑎2+ (𝑎𝑞) + 2 𝑂𝐻 − (𝑎𝑞)
(½ pt)
(g) Determine the [H+] in barium hydroxide pH 10.60 [𝐻 + ] = 10−𝑝𝐻 = 10−10.60 = 2.5 × 10−11 𝑀
Ans. & U (½ pt)
Work (1/4)
SF (1/4 pt)
(h) Calculate the pOH of barium hydroxide pH 10.60 𝑝𝐻 + 𝑝𝑂𝐻 = 14.00
Ans. & U (½ pt)
Work (1/4)
SF (1/4 pt)
Ans. & U (½ pt)
Work (1/4)
SF (1/4 pt)
𝑝𝑂𝐻 = 14.00 − 𝑝𝐻 = 14.00 − 10.60 = 3.40 (i) Calculate the [OH-] in barium hydroxide pH 10.60 [𝑂𝐻 − ] = 10−𝑝𝑂𝐻 = 10−3.40 = 4.0 × 10−4 𝑀
Name __________________________________________________ Period ________ Date ______________________ 3. When pH paper is added to HBr what color does it turn? red
(½ pt)
4. When pH paper is added to a barium hydroxide solution, what color does it turn? blue
(½ pt)
