2. Describe how to make up the following solution: 250.0 mL of a 0.0200M solutio

Question

2. Describe how to make up the following solution: 250.0 mL of a 0.0200M solution of AgNO. You are given solid AgNO, distilled water, and a 250 mL volumetric flask. Show your calculation for the required amount of AgNO. 3. Describe how to make up the following solution: 500.0 mL of a 2.50M solution of HNO,. volumetric flask. Show your calculation for the required amount of 6M HNO> You are given 6M HNO3, distilled water, and a 500 ml. 4. Calculate the molarity of a solution that is prepared by dissolving 0.453g KMnO, in enough water to give a 250.0 mL solution.

Explanation / Answer

1) molarity of AgNO3 = no. Of moles/vol in lts = 0.02 M

Vol of solution = 250ml = 250/1000= 0.25lts

0.02 = no. Of moles/0.25

No. Of moles = 0.25x0.02 = 0.05

0.05 = no. Of moles = wt of silver nitrate/mol mass of silver nitrate. = mass/169.87 = 0.05

Mass of silver nitrate for preparation 0.02M of 250ml solution = 0.05x169.87 = 8.4935 gms

2) molarity of initial .Molarity M1 = 2.5

Vol. Of initial solution V1 = 500 ml

Molarity of final solution M2 = 6 M

Vol of final solution V2 = V

M1V1 = M2 V2

2.5 x 500 = 6 x V

V = 208.34 ml of 6M HNO3

Remaining 291.66 ml of distilled water to make up 2.5 M HNO3 solution.

3) molarity of KMnO4 = no. Of moles of KMnO4/vol in lts

Vol in lts = 250 (ml)/1000 = 0.250 lts

No. Of moles of KMnO4 = wt taken/molar mass = 0.453/158.034 = 0.002866

Molarity = 0.002866/0.25 = 0.01146 M

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