A Carbon dioxide dissolves in water to produce carbonic acid (H;co,). Under normal atmospheric conditions, the total amount of carbonic acid (in all forms) in water is 1.2 x 10* M. Which is the correct mass balance equation for carbonate? Equation 1: [H;CO3] = [HC05] + [co5²] Equation 2: [H*] = [OH-]+ [HCO5]+ 2 × [[co5*] 1.2 x 10 -8 = [H;CO3] + [HCO5]+ [CO5²] 1.2 x 10-8 = [OH-]+ [HCO5]+ 2 × [co5] Equation 5: 1.2 x 10 -º = [H2CO3] + [HCO5]+ 2 × [co5ª] Equation 3: Equation 4: B What is the predominant form of the triprotic acid, citric acid, at pH 6.2? Answer options: H,A, H;A', HA*?, A Calculate oma and la. for acetic acid in a solution that has a pH of 5.32. Answer options: 0.05 and 0.95; 0.21 and 0.79; 0.56 and 0.44; 0.72 and 0.28
A Carbon dioxide dissolves in water to produce carbonic acid (H;co,). Under normal atmospheric conditions, the total amount of carbonic acid (in all forms) in water is 1.2 x 10* M. Which is the correct mass balance equation for carbonate? Equation 1: [H;CO3] = [HC05] + [co5²] Equation 2: [H*] = [OH-]+ [HCO5]+ 2 × [[co5*] 1.2 x 10 -8 = [H;CO3] + [HCO5]+ [CO5²] 1.2 x 10-8 = [OH-]+ [HCO5]+ 2 × [co5] Equation 5: 1.2 x 10 -º = [H2CO3] + [HCO5]+ 2 × [co5ª] Equation 3: Equation 4: B What is the predominant form of the triprotic acid, citric acid, at pH 6.2? Answer options: H,A, H;A', HA*?, A Calculate oma and la. for acetic acid in a solution that has a pH of 5.32. Answer options: 0.05 and 0.95; 0.21 and 0.79; 0.56 and 0.44; 0.72 and 0.28
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter4: Reactions In Aqueous Solution
Section: Chapter Questions
Problem 60QAP: Gold metal will dissolve only in aqua regia, a mixture of concentrated hydrochloric acid and...
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![A Carbon dioxide dissolves in water to produce carbonic acid (H;CO;). Under normal atmospheric conditions,
the total amount of carbonic acid (in all forms) in water is 1.2 x 10° M. Which is the correct mass balance
equation for carbonate?
[H;CO3] = [HC05]+ [co5²]
Equation 2: [H+]= [0H-]+ [HCO5]+ 2 × [co;?]
1.2 x 10 -8 = [H2CO3:] + [HCO5]+ [cO5²]
1.2 x 10-8 = [OH-]+ [HcO5]+ 2 x [co5?]
Equation 5: 1.2 x 10 - = [H¿CO3] + [HCO5]+ 2 × [co;°]
Equation 1:
Equation 3:
Equation 4:
What is the predominant form of the triprotic acid, citric acid, at pH 6.2?
Answer options: H;A, H;A', HA?, A
Calculate cua and a,. for acetic acid in a solution that has a pH of 5.32.
Answer options: 0.05 and 0.95; 0.21 and 0.79; 0.56 and 0.44; 0.72 and 0.28](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9a5a0ee6-3378-4d6f-956a-809d7f653ec8%2Fe7b5e9c3-b025-4e75-b124-c92a4398afdb%2Fnwilrz_processed.png&w=3840&q=75)
Transcribed Image Text:A Carbon dioxide dissolves in water to produce carbonic acid (H;CO;). Under normal atmospheric conditions,
the total amount of carbonic acid (in all forms) in water is 1.2 x 10° M. Which is the correct mass balance
equation for carbonate?
[H;CO3] = [HC05]+ [co5²]
Equation 2: [H+]= [0H-]+ [HCO5]+ 2 × [co;?]
1.2 x 10 -8 = [H2CO3:] + [HCO5]+ [cO5²]
1.2 x 10-8 = [OH-]+ [HcO5]+ 2 x [co5?]
Equation 5: 1.2 x 10 - = [H¿CO3] + [HCO5]+ 2 × [co;°]
Equation 1:
Equation 3:
Equation 4:
What is the predominant form of the triprotic acid, citric acid, at pH 6.2?
Answer options: H;A, H;A', HA?, A
Calculate cua and a,. for acetic acid in a solution that has a pH of 5.32.
Answer options: 0.05 and 0.95; 0.21 and 0.79; 0.56 and 0.44; 0.72 and 0.28
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