AP Chemistry - Molarity and Solution Creation 1. The maximum concentration of salt in water at 0oC is 31.6 g/100 mL.  What mass of salt can be dissolved in 250 mL of solution? 2. To prepare for an experiment using flame tests, a student requires 100 mL of 0.10 mol/L solutions of each of the following substances.  Calculate the required mass of each solid. a)   NaCl b)   KCl c)   CaCl2 3. An experiment is planned to study the chemistry of a home water-softening process.  The brine (sdoium chloride solution) used in this process has a concentration of 25 g/100 mL.  What is the molar concentration of this solution? 4. What volume of 0.055 mol/L glucose solution found in a plant contains 2.0 grams of glucose,  C6H12O6(aq)? 5. In a quantitative analysis for sulfate ions in a water treatment plant, a technician needs 100 mL of 0.125 mol/L barium nitriate solution.  What mass of pure barium nitriate is required? 6. A chemical analysis of silver uses 100 mL of a 0.155 mol/L solution of potassium thiocyanate, KSCN.  Write a complete, specific procedure for preparing the solution from the solid.  Include all the necessary calculations and precautions. 7. Calculate the molar concentration of the following: a)    0.35 mole of copper(II) nitrate is dissolved in water to make 50 mL of solution b)    10.0 grams of sodium hydroxide is dissolved in water to make 2.00 L of solution. c)    A sample of tap water contains 16 ppm of magnesium ions. 8. Standard solutions of sodium oxalate, Na2C2O4(aq), are used in a variety of chmeical analyses.  What mass of sodium oxalate is required to prepare 250.0 mL of 0.375 mol/L solution? 9. What is a standard solution, and why is such as solution necessary? 10. Standard solutions of potassium hydrogen tartrate, KHC4H4O6(aq), are used in chemical analyses to determine the concentration of bases such as sodium hydroxide. a)     Calculate the mass of potassium hydrogen tartrate that is needed to be measured to prepare 100.0 mL of a  0.150 M  standard solution. b)    Write a complete procedeure for the preparation of this standard solution, including specific quantities and equipment. 11. Calculate the number of grams of each solute that has to be taken to make each of the following solutions. 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 12. What is the molarity of pure water? Concentrated ammonia contains 26 grams NH3 per 100 mL of solution.  What is its molarity? 14. What is the molarity of a solution prepared by dissolving 17.1 grams of ordinary sugar (C12H22O11) in enough water to make 0.500 L of solution? 15. What is the molarity of a solution made by dissolving 10.0 grams of NaOH in 0.200 L of water? 16. Calculate the molarity of a solution containing 5.0 mg of BaCl2 per mL of solution. 17. Calculate the grams of silver nitriate needed to prepare 0.500 L of a 0.100 M solution. 18. Calcualte the grams of BaCl2 needed to prepare 200 mL of a 0.500 M solution. 19. 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 20. 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 of cobalt(II) chloride e)   0.250 L containing 4.33 grams of chromium(III) iodide 21. What mass of solute is required to prepare the indicated 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 22. Fifty mL of 0.50 M HCl is mixed with 30 mL of 0.28 M HCl.  Claculate the molarity of the resulting mixture.