Ask a New Question

Asked by Aaron

calculate the pH of a solution after .054 moles of KOH is added to a 1.0L buffer solution of .25M HF (Ka=7.1 x 10^-4) and .10M KF
11 years ago

Answers

Answered by DrBob222
millimols KF = 1000 mL x 0.1M = 100
millimols HF - 1000 nK x 0.25 = 250
mmols KOH added = 54

.......HF + OH^- ==> F^- | H2O
I......250...0......100
added.......54...............
C......-54.-54.......+54
E......196...0........54........
Then pH = pKa + log (base)/(acid)
Substitute the E line into the HH equation and solve for pH.

11 years ago

Related Questions

Calculate the pH of a solution prepared by mixing 200.0 mL of 0.100 M NaOH with 150.0 mL of 0.200... Calculate the pH of a solution whose H3O+ concentration is 1.5 x 10-13M. Is the solution acidic, bas... Calculate the pH of a solution that has [OH^-] = 3.2 × 10^-2 M. Be sure your answer has the correct... Calculate the pH of a solution that has[OH^-] = 2.1x10^-2 M round your answer to 2 decimal places... CALCULATE THE PH OF A SOLUTION OF 0.005moldm-³ tetraoxosulphate (VI) acid. The answer plz Calculate the pH of a solution when adding 30.00 mL of 0.1000 M NaOH on 50.00 ml of 0.0500 M HCl wit... Calculate [H3O+] for a solution of hydrobromic acid for which pH = 5.79. Be sure your answer has the... Calculate the pH of solution involved in following electrode if the cell emf is 0.4786 V: calculate pH of HCl solution
Ask a New Question
Archives Contact Us Privacy Policy Terms of Use