How Does Electrolysis Affect pH in a HBr Solution?

AI Thread Summary
Electrolysis of a 1.30 L solution of 0.550M HBr with a current of 10.7 Amps converts some H+ ions to hydrogen gas (H2), affecting the solution's pH. After calculating the moles of H+ removed during 77 minutes, the resulting concentration of H+ is found to be 0.394M. The pH is then calculated as 0.405, which was initially deemed incorrect due to not accounting for the starting amount of H+. The correct approach requires subtracting the moles of H+ converted from the initial concentration. Ultimately, the discussion emphasizes the importance of considering both the initial and remaining concentrations of H+ in pH calculations.
harrietstowe
Messages
46
Reaction score
0

Homework Statement


A current of 10.7 Amps is applied to a 1.30 L solution of 0.550M HBr converting some of the H+ to H2(g), which bubbles out of solution. What is the PH of the solution after 77 minutes.


Homework Equations





The Attempt at a Solution


(10.7 C/s)(1 mol e/96485 C)(2 mol H+/2 mol e)(60s/min)(77 min) = .512 mol H+

.512 mol H+/1.30L = .394M H+
-log(.394M) = .405 = PH

This was incorrect
 
Physics news on Phys.org
You started with a certain amount of H+ in the solution. The electrolysis removed some. Now you need to calculate what's left.
 
I see will try, thank you
 
It worked, thank you
 

Thread 'Prove that evolution is constant (Provide at least two arguments to support your position)'

I don't get how to argue it. i can prove: evolution is the ability to adapt, whether it's progression or regression from some point of view, so if evolution is not constant then animal generations couldn`t stay alive for a big amount of time because when climate is changing this generations die. but they dont. so evolution is constant. but its not an argument, right? how to fing arguments when i only prove it.. analytically, i guess it called that (this is indirectly related to biology, im...
View full post »
Thread 'How to find the pH of a galvanic cell (MIT OCW problem set)'

Thread 'How to find the pH of a galvanic cell (MIT OCW problem set)'

This is the final problem in this problem set from MIT OCW. Here is what I did to try to solve it The table cited in the problem is below We can easily spot the two redox couples that are in the electrochemical cell we are given. The hydrogen-based electrode has standard potential zero, and the silver-based electrode has standard potential 0.22. Thus, the hydrogen electrode, with the lower potential, is the reducing agent (ie, it is where oxidation happens) and is the anode. Electrons...
View full post »

Similar threads

How Does Pre-existing CH3COONa Affect Buffer pH Calculation?
Replies
4
Views
2K
What is the pH of this new solution?
Replies
2
Views
2K
How do you calculate the pH of 35.0-mL of 0.15M acetic acid?
Replies
6
Views
6K
Calculating the molar concentration of H3O+ and pH of solutions
Replies
4
Views
6K
Solved: Calculate pH of Aqueous Solution w/ HBr(g)
Replies
3
Views
4K
Acid Mixture pH Problem: Calculating Solution pH with CH3COOH, CH3COONa, and HCl
Replies
5
Views
2K
Find pH of Buffer: NaH2PO4 & Na2HPO4 Solution
Replies
6
Views
4K
How Does Adding Nitric Acid Affect the pH of a Carbonate Buffer Solution?
Replies
12
Views
12K
Calculating pH for Strong Acid-Base Titration
Replies
1
Views
10K
Electrochemical Cells (involving partial pressures and pH)
Replies
7
Views
6K

Hot Threads

Recent Insights

Back
Top