AP Chemistry - Solution Molarity Worksheet 1. Suppose you prepare a 0.200 M salt solution in a 250-mL volumetric flask and then accidentally spill some of it. What happens to the concentration of the solution in the bottle? 2. Calculate the number of grams of each solute that has to be taken to make each of the following solution. (a) 250 mL of 0.100 M NaCl (b) 100 mL of 0.440 M C6H12O6 (glucose) (c) 500 mL of 0.500 M H2O2 3. How much solute, in grams, is needed to make each of the following solutions? (a) 250 mL of 0.00100 M Na2SO4 (b) 100 mL of 0.250 M Na2CO3 (c) 500 mL of 0.400 M NaOH 4. What is the molarity of pure water? 5. Concentrated ammonia contains 26 grams NH3 per 100 mL of solution. What is its molarity? 6. What is the molarity of a solution of sodium chloride that contains 26.00 g NaCl/100.0 mL solution? 7. What is the molarity of a solution prepared by disoolving 17.1 grams of ordinary sugar (C12H22O11) in enough water to make 0.500 L of solution? 8. What is the molarity of a solution made by dissolving 10.0 grams of NaOH in 0.200 L of water? 9. Calculate the molarity of a solution containing 5.0 mg of BaCl2 per mL of solution. 10. Calculate the grams of silver nitrate needed to prepare 0.500 L of a 0.100 M solution. 11. Calculate the grams of BaCl2 needed to prepare 200 mL of a 0.500 M solution. 12. The following questions refer to a 0.20 M solution of BaCl2. The molecular mass of BaCl2 is 208.23 g/mole. a) Calculate the moles of BaCl2 in 2.00 mL of solution. b) Calculate the mg and grams of BaCl2 in 2.00 mL of the solution. c) Calculate the volume in mL that contains 5.0 moles of BaCl2. d) Calculate the volume in mL that contains 41.6 mg of BaCl2. 13. Calculate a) the volume of 2.0 M CaCl2 that must be used to prepare 1200 mL of 0.80 M CaCl2 b) the volume of water that must be added. 14. Calculate the molarity of these solutions: a) 1.00 L containing 119 grams of KCl b) 2.00 L containing 223.5 grams of CuBr2 c) 0.250 L containing 13.35 grams of aluminum chloride d) 0.150 L containing 13.0 grams cobalt(II) chloride e) 0.250 L containing 4.33 grams of chromium(III) iodide 15. How many moles of NaOH are contained in a) 1.0 litre of a 1.0 M solution? b) 0.50 L of a 1.0 M solution? c) 0.50 L of a 0.50 M solution? d) 0.125 L of a 0.50 M solution? e) 5.0 x 10-2 L of a 5.0 x 10-3 M solution 16. Calculate the mass of solute needed to make these solutions: a) 1.0 L of 1.0 M sodium hydroxide b) 0.500 L of 2.00 M calcium nitrate c) 2.0 L of 0.50 M potassium bromide d) 0.200 L of 0.75 M zinc chloride e) 0.125 L of 2.40 M ammonium chloride 17. What mass of solute is required to prepare the volume of each of these solutions? a) 500 mL of 3 M CaCl2? b) 750 mL of 2.0 M H2SO4? c) 5.0 L of 0.50 M H2C2O4? d) 0.125 L of 8.00 M HC2H3O2? e) 5.0 x 104 mL of 0.10 M KBr? f) 1.0 x 10-3 L of 1.0 x 10-3 M NH4Cl? g) 150 mL of 0.50 M ZnCl2? 18. Tell how to prepare a solution of HNO3 which contains 0.1 mmol per mL from a 6 M stock solution of HNO3 19. Fifty mL of 0.50 M HCl is mixed with 30 mL of 0.28 M HCl. Calculate the molarity of the resulting mixture. 20. Two litres of 6.0 M HNO3 is added to 1.0 L of 2.0 M HNO3. What is the concentration of HNO3 in the mixture? 21. Calculate the volume of 12 M HCl that must be added to 2.5 L of 1.0 M HCl in order to obtain 15 L of 1.0 M HCl. 22. 50.0 mL of an aqueous NaCl solution yielded 1.25 grams NaCl on evaporation. What was the molarity of the original solution. 23. Calculate the molarity of a solution prepared by dissolving 54.5 grams of Na2CO3.10H2O in enough water to give the resulting solution a volume of 2.4 L. 24. What volume of 2.00 mol/L HNO3 is needed to yield 10.00 grams of HNO3? 25. Give directions for preparing 500 mL of 0.050 mol/L KMnO4. 26. Give directions for preparing 250 mL of 0.500 mol/L CuSO4 using CuSO4.5H2O as solute.