A community for students.
Here's the question you clicked on:
 0 viewing
adam160596
 11 months ago
What would the pH of 0.56M HF be? How would I go about solving this
adam160596
 11 months ago
What would the pH of 0.56M HF be? How would I go about solving this

This Question is Closed

shoba
 11 months ago
Best ResponseYou've already chosen the best response.1is there any other information given..? pka value?

shoba
 11 months ago
Best ResponseYou've already chosen the best response.1HF <=>H+ + F initial no of mols HF = 0.56 H+ = 0 F = 0 at equilibrium HF = 0.56  x H+ = x F = x ka = [H+] * [F] / [HF] pka = log ka from that you can find ka and ka = x * x / (0.56  x) from this x can be calculated. x is the H+ mols and since we got to the 1000 cm3 (we simply got the concentration as no of mols) x = [H+] then ph can be calculated. ... ka = 10^ 3.14 ka = 7.244 * 10 ^4 7.244 * 10 ^4 = x^2/ [0.56x] x is very small so 0.56  x can be take as 0.56 7.244 * 10 ^4 = x^2/ 0.56 x^2 = 0.0004032 x = 0.0200798 = [H+] pH = log [H+] pH = 1.697 *assumed the pka value 3.14
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.