Using words, explain how you would prepare 0.75L of the 0.12 M aqueous solution of AgNO3 in the laboratory, starting with deionized water and solid AgNO3. In your response, refer to the mass of AgNOs that you calculated in part (e)

Question

Using words, explain how you would prepare 0.75L of the 0.12 M aqueous solution of AgNO3 in the laboratory, starting with deionized water and solid AgNO3. In your response, refer to the mass of AgNOs that you calculated in part (e)

The mass I calculate in part e is 15g of AgNO3

Answer 1

I don't know what part (e) was about; however, you need about 15.3 g AgNO3. So here is what I would do to prepare 0.75 L of 0.12 M AgNO3. I don't know how that is to figure in to your part e response so I'll leave that for you to handle.

mols needed = M x L = 0.12 x 0.75 = o.09
grams needed = mols x molar mass = 0.09 moles x 170 g/mol = 15.3 g.
Transfer 15.3 g AgNO3 to a 750 mL volumetric flask, add some DI water, swirl to dissolve all of the AgNO3, add DI water to the mark on the volumetric flask, stopper, mix thoroughly, label. done.