Beginner College Chemistry Questions, Need help

Thanks for the help if you happened to help me with my other two problems, now I've got a few more, and I need to know these well for the test coming up and I can't seem to figure them out. They're very similar as you'll see.

1)Average vinegar in the United States is around 6% (w/v). Convert this value to molarity.

2) There is a bottle of 3.7% (w/v) solution of sodium hypochlorite (m.w. = 74.44 g/mol) How many grams of sodium hypochlorite are present in 70.9mL of solution. What would the molarity of the solution be?

3) And lastly I'd just like to know how to convert a pH. For example 2.43 pH becomes [H+] 3.72 X 10^-3. I need to see the step to reach that point. Right now all I can do is convert from [H+] to pH but not the other way around. Hope this makes sense.

6% acetic acid = 6ml in 100g sample

density of acetic acid = 1.049g/ml
6 ml x 1.049g/ml = 6.294g acetic acid, C2H4O2
6.295g acetic acid in 93.706g water, density of water = 1g/ml so 6.295g acetic acid in 0.0937L
6.295g / 60g/mole = 0.105moles
0.105moles / 0.0937L = 1.12M

2. 3.7% w/v means that 3.7g NaClO is in a total of 100g
as the density of water = 1g/ml, the water has a mass of 96.3g and a volume of 96.3ml
3.7g / 74.45g/mole = 0.05moles NaClO
0.05moles / 0.0963L = 0.52M

3. 2.43 = pH so 10^-2.43 = [H+]
pH = -log[H+], you need to reverse the equation
inverse of the log = 10^-x