Question

Which of the following pairs of ionic compounds are BOTH expected to be insoluble in water?...

Which of the following pairs of ionic compounds are BOTH expected to be insoluble in water?

sodium acetate; calcium sulfate silver nitrate; silver chloride     silver chloride; barium sulfate magnesium chloride; potassium sulfate

A solution is prepared by dissolving 4.68 g of NaCl in enough water to produce 40.0 mL of solution. What is the molarity of NaCl for the solution?   

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Homework Answers

Answer #1

answer : silver chloride; barium sulfate

Explanation :

first group cations are soluble in water.

CH3COONa soluble and CaSO4 are in soluble in water

silver nitrate (AgNO3) is soluble and silver chloride( AgCl) in soluble.

BaSO4 is not soluble .

AgCl is not soluble.

2)

mass of NaCl = 4.68 g

moles of NaCl = 4.68 / 58.5 = 0.08

volume = 40.0 mL

Molarity = moles / volume

             = 0.08 / 0.040

Molarity of NaCl = 2.00 M

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