I'm going crazy over this question that I can't complete
The question reads: You prepare a "stock" solution by dissolving 50.0 grams of potassium chloride (KCl) in enough water to make 250mL of solution. If you place 100mL this stock into a beaker and then add (another) 50mL of water to it, what is the resulting molarity?
I figure that I need to find the molarity of the "stock" solution:
My work: Molar Mass of KCl = 74.55g/mol
50g/74.55 = .67moles
250mLx1l/1000mL = .25L ----> 1000/250 = 4
4x.67/.25L = 2.68mol/L
I can't figure out where to go after that. Do I plug the 2.68mol/L to a different equation?