Question

A) How many grams of solid silver nitrate would you need to prepare 150.0 mL of a 0.140 M AgNO3 solution? B) An experiment calls for you to use 100 mL of 0.30 M HNO3 solution. All you have available is a bottle of 3.8 M HNO3. How many milliliters of the 3.8 M HNO3 solution do you need to prepare the desired solution? C) How many milliliters of water do you need to prepare the desired solution?

Answer #1

A) How many grams of solid silver nitrate would you need to prepare 150.0 mL of a 0.140 M AgNO3 solution?

mol = MV = 0.14*150/1000 = 0.021 mol of Ag needed

mas s= mol*MW = 0.021*107.8682 = 2.265 g of Ag are neede

B) An experiment calls for you to use 100 mL of 0.30 M HNO3 solution. All you have available is a bottle of 3.8 M HNO3. How many milliliters of the 3.8 M HNO3 solution do you need to prepare the desired solution?

M1V1 = M2V2

3.8*V1 = 100*0.3

V1 = 100*0.3/3.8 = 7.89473 ml of acid (concnetrated)

C) How many milliliters of water do you need to prepare the desired solution?

VT = Vwater + Vacid

Vt = 100 and Vacid = 7.89473

then

Vwater= 100-7.89473 = 92.10527 ml

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