Reference no: EM131430361

1. The sulfur dioxide present in air is responsible for the "acid rain" phenomenon.  One can calculate its concentration by titrating against a standard permanganate solution as follows:

5 SO₂   +   2 MnO₄^-1   +   2 H₂O   →   5 SO₄^-2   +   2 Mn⁺²   +   4 H⁺

How many grams of SO₂ are present in a sample if 7.37 mL of a 0.00800 M KMnO₄ solution is needed for the titration?  Answer  9.45 x 10^-3 grams

2. Calculate the molarity of (a) 6.57 g of methanol (CH₃OH) in 150. mL of solution and (b) 10.4 g of calcium chloride in 220. mL of solution.  Answers  (a) 1.37 M  (b) 0.426 M

3. Water is added to 25.0 mL of a 0.866 M KNO₃ solution until the final volume is exactly 500. mL. What is the concentration of the final solution?  Answer  0.0433 M

4. A 1.00 mL solution of a radioactive sample exhibiting 1.00 x 10⁹ counts per minute is placed in a tank containing water, and the tank's water is stirred until the radioactivity is completely distributed.  A 1.00 mL sample of the water is then removed and found to exhibit 5.00 x 10² counts per minute.  What is the volume of the water in liters?  Answer 2000 liters

5. Calculate the volume of 0.150 M HCl needed to completely neutralize 25.00 mL of 0.125 M NaOH.  Answer  20.8 mL