Solution Stoichiometry (cont)

Ex. 100 ml of 0.250 M of Iron (II) Chlorine reacts with excess copper. How many grams of Iron are produced?

FeCl2 + Cu -> Fe + Cu Cl2

0.25 M x 0.1L x 1/1 x 55.8g = 1.40 g

• How many moles of Copper Chloride are produced?

0.25 M x 0.1L x 1/1 = 0.0250 mol of copper chloride

• Determine [CuCl2]

0.025 mol x 1/ 0.1 = 0.25 M of CuCl2

Ex. A beaker contains 100 ml of 1.5M HCl. Excess Zinc is added to the beaker. Determine how many leaders of hydrogen gas should be produced.

2 HCl + Zn -> ZnCl2 = H2

1.5M x 0.1L x 1/2 x 22.4L/mol = 1.7L of H2

• If 1.40L Hydrogen gas are actually produced what is the present yield?

1.4/1.7 x 100 = 82%

Ex. A 0.330 M solution of Ba(OH)2 reacts with 25 ml of 2.50M HCl. What volume of Ba(OH)2 is required for a complete reaction.

Ba(OH)2 + 2 HCl -> BaCl2 + 2 H20

2.50 M x 0.025 x 1/2 = 0.0313 mol of Ba(OH)2

 0.330M x 0.0313 mol = 0.095L or 95 ml

Ex. A 3.00g of piece of Iron is added to a beaker containing 100 ml of 0.750 M AgNO3, Determine the L.R.

Fe+ 3 AgNO3 - > Fe(NO3)3 + 3 Ag

0.750 M x 0.1 L x1/3 x 55.8 = 1.40g of Iron       Ag is L.R.

• How many grams of Ag are produced?

0.750 M x 0.1L x 3/3 x 107.9 = 8.09g

example of Titration