A primary standard solution of silver nitrate solution is made by dissolving 12.

Question

A primary standard solution of silver nitrate solution is made by dissolving 12.25 g of solid AgNO_3 (FW = 169.87 g/mol) into 1.00 L solution. How many mL of this solution will react with 0.1197 g BaCl_2.2H_2O (FW = 244.263 g/mol)? 13.6 6.80 3.40 27.2 Calculate the concentration of Co^2+ in a solution that is prepared by mixing 1.50 millimoles Co^2+ and 2.50 millimoles EDTA into 1000 mL of solution that has been buffered to a pH of 3.0. (K_f for CoY^2- = 2.0 times 10^16, alpha 4 = 3.30 times 10^-11) 7.5 times 10^-17 M 2.3 times 10^-6 M 0.0015 M 4.1 times 10^-9 M

Explanation / Answer

80. Write down the balanced chemical equation for the reaction as

2 AgNO3 (aq) + BaCl2.2H2O -------> 2 AgCl (s) + Ba(NO3)2 (aq) + 2 H2O (l)

Moles of BaCl2.2H2O reacted = (mass of BaCl2.2H2O)/(F.W. of BaCl2.2H2O) = (0.1197 g)/(244.263 g/mol) = 4.900*10-4 mol.

Moles AgNO3 reacted = (4.900*10-4 mol BaCl2.2H2O)*(2 mole AgNO3/1 mole BaCl2.2H2O) = 9.800*10-4 mole.

Now, we simply need to find the volume of the solution which will contain 9.800*10-4 mole AgNO3.

Moles of AgNO3 in the solution = (12.25 g)/(169.87 g/mol) = 0.07211 mole.

Since the volume of the solution is 1.00 L, the molar concentration of (0.07211 mole)/(1.00 L) = 0.07211 M.

Let x mL of 0.07211 M solution be taken. Therefore,

(x mL)*(1 L/1000 mL)*(0.07211 mol/L) = 9.800*10-4

===> 7.211*10-5x = 9.800*10-4

===> x = (9.800*10-4)/(7.211*10-5) = 13.59 13.6

The volume of solution required is 13.6 mL (ans).

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