(Analysis) a. You found a 125.0 ml contaminated water sample in the lab. This so

Question

(Analysis) a. You found a 125.0 ml contaminated water sample in the lab. This solution is known to contain Silver Nitrate (AgNO,). Determine the original Molarity of silver ions (Ag) in the contaminated sample if it took 7.25 ml of a 0.25 M Barium Chloride (BaCl:) solution to precipitate ALL the silver ions as silver chloride (AgCI). b. You need to do another cleanup job, but this time the BaCla solution needed should be more dilute. Show your calculations and DESCRIBE the steps for how you will make 35.0 ml of a 0.2 M Bal: solution starting from the original solution in part a.

Explanation / Answer

(a)

Balanced equation:

2 Ag+ (aq.) + BaCl2 (aq.) ---------------> 2 AgCl (s) + Ba2+ (aq.)

Useful formula,

M1 V1 / n1 = M2 V2 / n2

M1 * 125.0 / 2 = 0.25 * 7.25 / 1

M1 = Molarity of silver ions = 0.029 M

(b)

Useful formula to calculate molarity of dilute solution,

M1V1 = M2V2

0.25 * V1 = 0.20 * 35.0

V1 = 28 mL

So, take 28 mL of 0.25 M solution and dilute it to 35 mL of total volume to get 0.20 M of solution.

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