In order to mix up chemicals in the right amounts (so we get the right amount out of the reaction), we have to figure out how much of a chemical to put in in the first place. Sometimes chemists have this problem: they need for example 2.0 L of 1.5 M solution of Na2CO3 (sodium carbonate). They find a bottle of Na2CO3 on the shelf, some distilled water, and a 2.00L flask. How much Na2CO3 do they put in the flask with the water?


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2 Responses to “Molarity And Preparation Of Solutions”

  1. No, not really. it’s going to depend on how much water you add to the pitcher and also how much your cabbage holds onto before extracting it.

  2. youngsurrender says:

    Do you have to know how many moles are the basic solution (cabbage juice) to know how concentrated the firsts solution (the base) will be? Sorry if that sounded confusing. I just started this chemistry section. Thanks!