arufel AP Chemistry Aqueous Solutions and Reactions l Aqueous Solutions l Daily

Question

arufel AP Chemistry Aqueous Solutions and Reactions l Aqueous Solutions l Daily Ops A solution is prepared by adding 34.71 g of solid KNO, to 382.48 mL of 3.56 M Mg(No2 What is the molarity of nitrate ion in the final solution? Assume moles are additive and that the volume of the final solution is 382 48 mL. Include the unit M in your answer. Round to two decimal places. Answer: Check A sample volume of 2100.5 mL of a 1.5 M soluble ionic compound, represented by the formula A,B. contains moles of the 'A ion. Check

Explanation / Answer

mol of NO3- from KNO3 = mass/MW = 34.71/101.1032 = 0.34331 mol

mol of NO3- from Mg(NO3)2 = 2*MV* = 2(3.56)(0.38248) = 2.7232 mol

total NO3- = 0.34331 + 2.7232 = 3.06651 mol of NO3-

Vtotal = 0.38248 L

[NO3-] = 3.06651 / 0.38248 = 8.017 M

Q2

1 mol of A3B --> 3 mol of A+ ion

mol = MV = (1.5*2.1005) = 3.15075 mol of A3B

mol of A+ = 3.15075*3 = 9.45225 mol of A+ ion

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