Saturday
April 19, 2014

Homework Help: Chemistry

Posted by Jill on Friday, March 22, 2013 at 9:45pm.

Calculate the pH of a solution that is 2.00M HF, 1.00M NaOH, and 0.393M NaG (Ka=7.2 x10^-4).

The answer I got was 4.76 ..

Answer this Question

First Name:
School Subject:
Answer:

Related Questions

Chemistry - .12M Lactic Acid (HC3H5O3, Ka=1.4x10^-4) is mixed with .10M NaC3H5O3...
Chemistry, Urgent! - I can't solve this! I keep trying but I can't get it. ...
chemistry - To 160.0 mL of a buffer solution containing 0.250 M ammonia and 0....
Chemistry - When 50.0ml of 1.00M HCl is titrated with 1.00M NaOH, the pH ...
chemistry - A. Strong Base 1.) What is the concentration of a solution of KOH ...
Chemistry - Consider a solution that contains both C6H5NH2 and C6H5NH3+. ...
Chemistry - Solution x has a pH of 4.35. Solution y has 10- times high [OH-] ...
chemistry - 1)A solution has a [OH-] of 5.2 x 10-4. What is the [H3O+] in the ...
chemistry - Hi, The problem is: "Calculate the concentration of OH- and the pH ...
chemistry - A 1.00M solution of a hypothetical weak acid (HB) has a pH of 2.85. ...

Search
Members