chemistry

posted by .

Calculate the ph for ch3co2h,3% dissociated at a concentration of 0.02 mol dm-3.

• chemistry -

Use caps where needed. ch3co2h means nothing. I assume you meant to write CH3COOH. Let me call that HAc (H for the last H on the right, the acid H, and Ac for the rest of the molecule).
............3% = 0.03 dissociated
.............HAc ==> H^+ + Ac^-
initial.....0.02M....0.....0
change.....-6E-4....6E-4...6E-4
equil...0.0194.....6E-4....6E-4
(Note:6E-4 = 0.02*0.03
Then plug H^+ into pH = -log(H^+)

Similar Questions

1. Chemistry

Initially, 1.68 mol of PCl5(g) and 0.36 mol of PCl3(g) are in mixed in a 2.00 l container. It is later found that 1.44 mol of PCl5 are present when the system has reached equillibrium. Calculate the value of the equllibrium. This is …
2. Chemistry

Calculate the molar concentration of H+ ion of a solution that is 3.45×10-1 M in CH3CO2H and 1.62×10-3 M in the salt CH3CO2Li. CH3CO2H(aq) = CH3CO2-(aq) + H+(aq)
3. chemistry

Calculate the percent yield if 104 g of CH3CO2CH2CH3 is produced by the reaction of 111 g of CH3CO2H according to the following equation: CH3CO2H(l) + CH3CH2OH(l) ¨ CH3CO2CH2CH3(l) + H2O(l)
4. Chemistry

a 1.00-mol sample of phosphorus pentachloride placed in 10.0-L reaction flask and allowed to come to equilibrium at 250 degrees celsius; PCL5(g) = PCL3(g) Cl2(g) if the amount of chlorine in the equilibrium mixture is0.470 mol, calculate …
5. College Chemistry

The initial concentration for the compounds involved in the reaction shown were determined to be [CH4(g)] = 0.6616 mol/L, [H2O(g)] = 0.8127 mol/L, [CO(g)] = 0.9566 mol/L, [H2(g)] = 0.7688 mol/L. Calculate the value of the equilibrium …
6. chemistry

Calculate the [CH3CO2H] in a solution if it has a pH 3.21. CH3CO2H = CH3CO2- + H+
7. AP Chemistry

The equilibrium constant for thermal dissociation of F2 F2(g)<->2F(g) is 0.300. If initially 1.00 mol F2 is placed in a 1.00 L container, which of the following is the correct number of moles of F2 that have dissociated at equilibrium?
8. Chemistry

A buffer contains 0.50 mol CH3CO2H and 0.50 mol CH3CO2- diluted with water to 1.0 L. How many moles of NaOH are required to increase the pH of the buffer to 5.00?
9. chemistry

A 1.0 x 10-2 M solution of a weak acid is found to be 3.7% dissociated. Calculate Ka of this acid. I found the amount dissociated by (amount dissociated/initial conc)*100=3.7 Where do I go from here?
10. Chemsitry

What is the pH of the buffer solution that results when 58.50 g of sodium acetate (NaCH3CO2) (Formula Mass = 82.02 g mol-1) is added to 1 litre of 0.45 mol L-1 acetic acid (CH3CO2H) ?

More Similar Questions