Use the given values of Ka to arrange the following acids in order of decreasing percent dissociation? Estimate [H3O+] in a 1.7 M solution of each acid. Having a difficult time trying to figure this out. Please help, Thank you.
Acid Formula Ka
Formic HCO2H 1.8×10−4
Hydrocyanic HCN 4.9×10−10
Perchloric HClO4 very large
Hypobromous HOBr 2.0×10−9
Part 1.
Use the given values of Ka to arrange the following acids in order of decreasing acid strength.
Use the given values of Ka to arrange the following acids in order of decreasing percent dissociation
Part 2.
Estimate [H3O+] in a 1.7 M solution of each acid.
[H3O+]formic, [H3O+]hydrocyanic, [H3O+]perchloric, [H3O+]hypobromous = ?
Acid Formula Ka
Formic HCO2H 1.8×10−4
Hydrocyanic HCN 4.9×10−10
Perchloric HClO4 very large
Hypobromous HOBr 2.0×10−9
Part 1.
Use the given values of Ka to arrange the following acids in order of decreasing acid strength.
Use the given values of Ka to arrange the following acids in order of decreasing percent dissociation
Part 2.
Estimate [H3O+] in a 1.7 M solution of each acid.
[H3O+]formic, [H3O+]hydrocyanic, [H3O+]perchloric, [H3O+]hypobromous = ?
1 Answer
Explanation:
And clearly, given this expression, STRONGER acids, i.e. those acids for which the equilibrium lies to the RIGHT as we face the page, have inherently high
You have got
We will solve the equilibrium concentrations for formic acid (of course the strong acid is stoichiometric in
...and if we let
So
So