A solution of vinegar is 5.10% by mass acetic acid in water. Assuming the density of the solution is 1.00g/ml

A solution of vinegar is 5.10% by mass acetic acid in water. Assuming the density of the solution is 1.00g/ml, what is the pH?

A hint was given saying that the mm of acetic acid is 60.05 g/mol and ka= 1.8 x 10^-5

I am kind of confused and where to start. I know I need to get the molarity..but I dunno where to start and where to go from there.

Any help is greatly appreciated!!

Thanks for your time!!

Hello

If the density of the solution is 1 g/mL, then is the mass of 1 L = 1000 g, and 5,1 % of this mass is
51 g.
And 51 g/L are 51/60,05 moles/L = 0,8493 moles/L = 0,8493 M.

Calculate the pH by
pH = 1/2*(pKa - log(c_Hac))
pH = 1/2(4,744 - log(0,8493)
pH = 1/2(4,744 +0,0709)
pH = 1/2(4,8149)
pH = 2,407

Regards