1. 150 ml of a 0.27 M solution of HCl contains _________moles of H⁺ ions. (ans .0405 )

Do this problem three ways: a) by using unit conversion factors b) by using an equation (M=n/V) c) by setting up a proportion.

More difficult: H₂SO₄ instead of HCl. or Reverse calculation.

2. a) 87.3 g of C₆H₆ equal ________ moles. As above do this problem three ways. (n=wt/MW)

b) 87.3 g of C₆H₆ contains ________ moles of C 

3. a) 3.6 g of CH3OH in 340 g of water = _____ molal

b) 256 mL of 0.358 M HBr = _____ moles of HBr

c) 12 g of C₃H₆O in 75 g CH₄O = _____ mole fraction of C₃H₆O

4. Classify each of the following as a non-electrolyte or electrolyte in water. For each electrolyte give the formula of the ions formed.

a) benzene - C₆H₆ b) H₂SO₄ c) CH₃F d) NaCl e) KNO₃ answer to b:electrolyte 2 H⁺ + SO₄^-2

5. Describe the bonding in Na₂SO₄ . Which bonds are ionic and which are covalent? How does this effect its structure when it is dissolved in water? When 0.2 mols of Na₂SO₄ is dissolved in 500 mL, what is the molarity of Na₂SO₄ in solution? What is the molarity of sulfate ions in solution? What is the molarity of sodium ions in solution? (answer to last question is 0.8 M)

6. A solution is prepared by dissolving 45.0 g of glucose (C₆H₁₂O₆, MW = 180) in water to make 400 mL of solution. The concentration of the solution is ________ M.

Do this problem three ways.

7. Find the molality of a 10.0% by weight NaOH solution. (F.W. of NaOH = 40.0 g/mol)

a) 10.0 m b) 0.25 m c) 2.78 m d) 1.42 m e) 2.78 x 10^-3 m

 8. Which of the following +1 ions is the least reactive: and : Cl⁺ Ar⁺ K⁺ Ca⁺ (ans K⁺)

Give your reason for selecting it.

9.  Define each of the following: electrolyte solution, ionic solution, ionic compound, non-electrolyte, weak electrolyte, strong electrolyte.