Textbook 6D.3
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Textbook 6D.3
I've been working this problem and I wrote out the ice chart correctly according to an older chem community post, however, the values that I'm getting at the end. The value of x should be 0.06 which makes HClO2 eq 0.04, however the value that I'm getting for x is 0.054. I can't manage to change any values by rounding or by putting more sig figs to get the correct value so I'm wondering what I'm doing wrong here. The first value I got was 0.063 after I found the K from the given pH 1.2.
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Re: Textbook 6D.3
Hi and happy friday :) I believe the first value you got (0.063) is the correct molar concentration for H3O+. However, I'm not sure what error you made after that. Since the chlorous acid is acting as an acid, the value of K (equilibrium constant) is also the Ka value. I included a picture of the work I did. My answers don't match the book exactly but I used exact values so the book probably rounded their intermediate values. Let me know if that helps!
Re: Textbook 6D.3
Kaitlin Eblen 1I wrote:Hi and happy friday :) I believe the first value you got (0.063) is the correct molar concentration for H3O+. However, I'm not sure what error you made after that. Since the chlorous acid is acting as an acid, the value of K (equilibrium constant) is also the Ka value. I included a picture of the work I did. My answers don't match the book exactly but I used exact values so the book probably rounded their intermediate values. Let me know if that helps!
Did you use the quadratic equation to solve for x or did you use a graphing calculator?
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- Posts: 104
- Joined: Wed Feb 17, 2021 12:24 am
Re: Textbook 6D.3
905767718 wrote:Kaitlin Eblen 1I wrote:Hi and happy friday :) I believe the first value you got (0.063) is the correct molar concentration for H3O+. However, I'm not sure what error you made after that. Since the chlorous acid is acting as an acid, the value of K (equilibrium constant) is also the Ka value. I included a picture of the work I did. My answers don't match the book exactly but I used exact values so the book probably rounded their intermediate values. Let me know if that helps!
Did you use the quadratic equation to solve for x or did you use a graphing calculator?
I plugged 10^-1.2 into my calculator and got 0.063 (which is the H3O+ concentration of HClO2 at equilibrium and therefore also the equilibrium state of HClO2 in the ice table). This means the "+x+ must also be 0.063. Did I answer your question?
Re: Textbook 6D.3
Kaitlin Eblen 1I wrote:905767718 wrote:Kaitlin Eblen 1I wrote:Hi and happy friday :) I believe the first value you got (0.063) is the correct molar concentration for H3O+. However, I'm not sure what error you made after that. Since the chlorous acid is acting as an acid, the value of K (equilibrium constant) is also the Ka value. I included a picture of the work I did. My answers don't match the book exactly but I used exact values so the book probably rounded their intermediate values. Let me know if that helps!
Did you use the quadratic equation to solve for x or did you use a graphing calculator?
I plugged 10^-1.2 into my calculator and got 0.063 (which is the H3O+ concentration of HClO2 at equilibrium and therefore also the equilibrium state of HClO2 in the ice table). This means the "+x+ must also be 0.063. Did I answer your question?
Yea I realized my mistake, thanks!
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