1. If that is 0.1 molal, you must change molality to molarity (but I don't see a density listed) [or you can assume 0.1 m = 0.1 M and not make a significant difference).
CH3COOH ==> CH3COO^- + H^+
Set up an ICE chart, substitute into the expression for Ka = (H^+)(CH3COO^-)/(CH3COOH), and solve for (H^+)
2. HNO3 is a strong acid; therefore, H^+ = M
3. Here is a site you can read about degree of dissociation. Use that to calculate concn of ions, convert to the ion product and Kion from there.
http://www.pinkmonkey.com/studyguides/subjects/chem/chap12/c1212601.asp
Post your work if you get stuck.
1. calculate H+ ion concentrates in 0.10 m acetic acid solutions. Given that dissociation constant of acetic acid in water is 1.8 * 10^-5 ?
2. Calculate the concentration of H+ and OH- in a 0.05 m HNO3 solutions at 25^0c ?
3. The degree of dissociation of pure water at 18^0c is found to be 1.8 * 10^-9. Find the ionic product of water and its dissociation constant at 18^0c ?
1 answer
1 answer