How Do You Make A Buffer Solution Of 150Mm Nacl, 10Mm Cacl2 And 25Mm Tris?
The trick here is that you want the FINAL solution to be 150mM NaCl 10mM CaCl2 25mM Tris Molarity = moles / Litres of solution or (milliMolarity = millimoles / litres of solution) If you prepare 5 ml of 150mM NaCl, then add an extra 10 ml to get a total of 15 ml then you have diluted your NaCl 3x and your 15 ml final solution will be 50mM NaCl The same applies to each of the other solutions, you will have diluted them all 3x The other thing to remember is that if you add 5 ml of one solution to 5 ml of another solution you will not always get 10 ml final volume. This is because of itermolecular attractions between the molecules of the solutions. For some solutions, you may end up with a larger volume then you wanted, for others a smaller volume. But you cannot assume that adding 5 ml of each solution will give you 15 ml. When preparing solutions you always add the amount of reagent you need to add in a smaller volume then you require, then, once everything is added and dissolved (disso
