A community for students.
Here's the question you clicked on:
 0 viewing
anonymous
 one year ago
Calculate the pH of a solution prepared by mixing 10.0 mL 1.0 M NaOAc and 35.0 mL 0.4M HOAc. Ka = 1.8E5
anonymous
 one year ago
Calculate the pH of a solution prepared by mixing 10.0 mL 1.0 M NaOAc and 35.0 mL 0.4M HOAc. Ka = 1.8E5

This Question is Open

abb0t
 one year ago
Best ResponseYou've already chosen the best response.0start by writing down the balanced equilibrium equation.

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0PH=4.47+, 397 =5.137 Where 4.47 is the ve log Ka =pka And , 397 is log base/acid This is Handerson equation by which you can detrmine the ph of buffer solution

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0PH=Pka + log [base]/[acid] It is used only for buffer solution. Your compounds are salt of conjugate base which is NaOCN And acid which is HOAC And this is buffer solution.

VincentLyon.Fr
 one year ago
Best ResponseYou've already chosen the best response.1The formula given above is ok, but the calculation is wrong. You should be able to manage this now.

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0I think it is true , but if you have noticed something wrong , I'll be glade to learn it from you

VincentLyon.Fr
 one year ago
Best ResponseYou've already chosen the best response.1I mean the numerical values must be calculated again. pKa is not 4.47 and log [base]/[acid] is not +0.397
Ask your own question
Sign UpFind more explanations on OpenStudy
Your question is ready. Sign up for free to start getting answers.
spraguer
(Moderator)
5
→ View Detailed Profile
is replying to Can someone tell me what button the professor is hitting...
23
 Teamwork 19 Teammate
 Problem Solving 19 Hero
 Engagement 19 Mad Hatter
 You have blocked this person.
 ✔ You're a fan Checking fan status...
Thanks for being so helpful in mathematics. If you are getting quality help, make sure you spread the word about OpenStudy.