Here's the question: ---------- A base stock solution is prepared by dissolving both 1 gram of sodium hydroxide and 2 grams of potassium hydroxide in enough water to prepare 100 mL of solution. How many millimeters of this base stock solution are required to neutralize 100 mL of 0.50 M [tex]H_2SO_4 _(_a_q_)[/tex] ? ------------- This is what I have so far. Using Molarity * Volume = moles I get that there are 0.05 mol of [tex]H_2SO_4 _(_a_q_)[/tex] Here's where I get stuck. I've never dealt with a problem where the base is made up of 2 components instead of one (i.e. just lithium hydroxide not a combination of lithium hydroxide and aluminum hydroxide). As such I am unsure where to go with this. I think that I am going to need 0.1 mol of the base stock solution but that's about it. Any ideas where I can go from here?