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Measuring Concentration of Ions in Solution

Measuring Concentration of Ions in Solution. Molarity is ONE way to do this…we will learn others later in the year!!!. Molarity. Molarity (M) =Mole of solute/liter of solution What do we have to be careful about when solving for molarity? Is amount of solute given in moles?

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Measuring Concentration of Ions in Solution

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  1. Measuring Concentration of Ions in Solution Molarity is ONE way to do this…we will learn others later in the year!!!

  2. Molarity • Molarity (M) =Mole of solute/liter of solution • What do we have to be careful about when solving for molarity? • Is amount of solute given in moles? • Is volume of solution given in L? • How can we manipulate this equation and then solve for: grams of solute? mL of solution?

  3. To calculate molarity practice problem: • What is the molarity of a solution in which 27 g of NaCl is dissolved in 100 mL of water?

  4. To calculate volume practice problem: • What is the volume in mL of solution if you want to make a 0.5 M solution by adding 50 g of NaCl?

  5. To calculate mass practice problem: • If you are making a .33 molar NaCl solution with a 150 mL of NaCL, what mass in g of NaClmust you add?

  6. Dilutions • Often you start with a solution of a certain molarity and want to “dilute” that solution. Use the following equation: • M1V1 = M2V2 (M=molarity; V= volume)

  7. How to calculate new molarity if diluting a solution: • You have a 0.5 M solution with a volume of 400 mL. You dilute the solution with water to a final volume of 1000mL. What is the resulting molarity?

  8. How to determine how much of an original solution to add if you want a certain amount of a solution with a new molarity: • If you have a 0.4 M NaCl solution and you want to make 800 mL of a 0.25 M NaCl solution, how much of the original solution should you use?

  9. Ion concentration • Sometimes it is useful to know the concentration of ions found in a solution. • You must multiply the molarity of the solution by the number of the given cation or anion. • For a 0.5 M solution of MgCl2: • Mg +2 : [0.5 M] • 2 Cl-1 : 2 * [0.5 M] = [1.0 M]

  10. Stoichiometry • AgNO3 (aq) + NaCl (aq)  AgCl(s) + NaNO3 (aq) • If 50 mL of a 0.5 M silver nitrate solution is added to a solution of excess NaCl, how much precipitate can be produced? • How many mL of a 0.5 M NaCl solution would be needed to run this reaction with no waste?

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