# Chemistry

a) Calculate [H3O^+] in a 0.15M solution of benzonic acid, HC7H5O2(aq) having K of 6.4x10^-5.

b) Calculate the per cent ionization of the HC7H5O2.

I got..

A) 0.16M but i did it again and got 7.2M so i'm very stuck as to the very different answers i got.

B) 12.4% ionization.

1. 👍 0
2. 👎 0
3. 👁 109
1. If you missed A you probably missed B.
Call benzoic acid HB, then
................HB ==> H^+ + B^-
initial........0.15....0......0
change..........-x......x.....x.
equil........0.15-x.....x......x

K = (H^+)(B^-)/(HB)
Substitute and solve for x.

%ion = [(H^+)/0.15]*100 = ?

1. 👍 0
2. 👎 0
posted by DrBob222

## Similar Questions

1. ### chem 12

a) Calculate [H3O^+] in a 0.15M solution of benzonic acid, HC7H5O2(aq) having K of 6.4x10^-5. b) Calculate the per cent ionization of the HC7H5O2. I got.. Kb = [HC7H5O3][OH]/HC7H5O2 6.3x10^-5 x Kb =1.0x10^-14 Kb =

asked by Sarah on October 11, 2011
2. ### chemistry 12

Calculate [H3O^-] in a 0.15M solution of benzoic acid, HC7H5O2(aq) having a Ka of 6.4 x 10^-5 I got. 6.4x10^-5=(x)(x)/0.15 6.4x10^-5= x^2/0.15 6.4x10^-5 x 0.15 = x^2 square root of 9.6x10^-6 = square root of x^2 x= 0.003098 The pH

asked by shelly on October 13, 2011
3. ### Chemistry

Calculate the [H3O+] and pH of each polyprotic acid solution. (b) 0.116 M H3C6H5O7 I did part (a) just fine, but for some reason can't figure (b) out. Can someone help me with just the [H3O+] part to get me started? I already got

asked by DeeDee on April 6, 2013
4. ### chemistry

What is the [C7H5O2−] in a solution which is 0.1283 M in HC7H5O2 and 0.1364 M in HBr? HC7H5O2(aq) + H2O(l) « C7H5O2−(aq) + H3O+(aq) Ka = 6.5000e-5

asked by Andy on May 6, 2014
5. ### chemistry

1)A solution has a [OH-] of 5.2 x 10-4. What is the [H3O+] in the solution? 2) A 0.25 M solution of a monoprotic acid, HA, has a pH of 2.54. What is Ka for this acid? The dissociation of HA is: HA + H2O H3O+ + A- (Hint: write the

asked by nicki on December 9, 2012
6. ### AP Chemistry

A buffer solution contains .4mol of formic acid, HCOOH and a .6mol of sodium formate, HCOONa, in 1L of solution. Ka of formic acid is 1.8 x 10^-4. a) calculate pH b) if 100ml of this buffer solution is diluted to a volume of 1L

asked by Jessie on April 25, 2010
7. ### Chemistry

Just two more to check, thanks! 1) The pH of a 1.25 M solution of unknown monoprotic acid is 5.43. Determine the value of Ka for this acid. HX H+ + X-. (I obtain 1.0 x 10^-11) 2) Calculate the pH of a solution which is 0.73 M

asked by Amanda on May 1, 2014
8. ### Chemistry

1. Calculate the pH of a buffer solution that contains 0.32 M benzoic acid (C6H5CO2H) and 0.17 M sodium benzoate (C6H5COONa). [Ka = 6.5 × 10-5 for benzoic acid] Round your answer to two places past the decimal. 2. A solution is

asked by Erin on April 8, 2013
9. ### Chemistry

1. Calculate the pH of a buffer solution that contains 0.32 M benzoic acid (C6H5CO2H) and 0.17 M sodium benzoate (C6H5COONa). [Ka = 6.5 × 10-5 for benzoic acid] Round your answer to two places past the decimal. 2. A solution is

asked by Erin on April 8, 2013
10. ### Chemistry

find the concentration of h3o in a .86mol/l solution of the weak acid H2O2 (kA=2.4x10-12)

asked by Buck on May 31, 2016

More Similar Questions