Please find the solutions without using the Hasselbach equation. Please show all calculations.
Find [H^+] in an aqueous 25 degrees Celsius that is .20 M in HC2H3O2 and .48 M in NaC2H3O2. For HC2H3O2, Ka = 1.8 x 10^-5 at 2 degrees Celsius.
A solution is prepared by adding HCl and HC2H3O2 to water. In the equilibrium constant.
Ka = [H^+] [C2H3O2^-]/[HC2H3O2]
Which of the following is correct
a) The H^+ in the numerator includes only the H+ that comes from the ionization of the HC2H3O2.
b) The H+ in the numerator in includes both the H+ that comes from the ionization of the HC2H3O2 and from the ionization of the HCl.© BrainMass Inc. brainmass.com October 25, 2018, 8:29 am ad1c9bdddf
Q1. NH4+ -----> NH3 + H+
[NH4+] = 0.20mol / 0.4L = 0.5M
If' x' is the change in concentration, then
Ka = 1 x 10^(-14) / Kb = [NH3][H+] / [NH4+] => 5.56 x 10^-10 = x^2/ (0.5 -x)
Hence 2.78 x 10^-10 - 5.56 x 10^-10x = ...
Three equilibrium problems that deal with finding out unknown concentrations are solved without using the Henderson-Hasselbach equation.
Determine pH of a Solution: Henderson HasselBach Equations
Using a ICE table (initial change equilibrium)
a) Calculate the pH of solution that is 0.175M in acidic acid(HC2H3O2) ans 0.110Min potassium Acetate(KC2H302)
b) Perform same calculation using the Henderson HasselBach equations to determine pH of the solutionView Full Posting Details