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CALCULATING CONCENTRATION OF SOLUTIONS

CALCULATING CONCENTRATION OF SOLUTIONS. 1. Mass Percent = (mass of solute/mass of solution)100 2. Parts per million = (mass of solute/mass of solution)10 6 3. Mass/volume percent = (mass of solute/mL solution)100 4. Volume percent = (mL solute / mL solution)100

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CALCULATING CONCENTRATION OF SOLUTIONS

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  1. CALCULATING CONCENTRATION OF SOLUTIONS 1. Mass Percent = (mass of solute/mass of solution)100 2. Parts per million = (mass of solute/mass of solution)106 3. Mass/volume percent = (mass of solute/mL solution)100 4. Volume percent = (mL solute / mL solution)100 5. Molarity = moles solute / L solution

  2. CALCULATING CONCENTRATION OF SOLUTIONS • How many grams of a solution that is 32.7% by mass NaCl would contain 45.0 g of NaCl? Mass % = (mass of solute /mass of solution) 100 32.7 % = (45.0 g / x )100 x = 45.0 g / 0.327 x = mass of solution = 138 g

  3. CALCULATING CONCENTRATION OF SOLUTIONS • How much solute is present in 756.1 mL of a 14.7% (mass/volume) HCl solution? Mass/volume % = (masssolute/volumesolution) 100 14.7 % = (x / 756.1 mL )100 x = 0.147 (756.1 mL) x = mass of solute = 111g

  4. CALCULATING CONCENTRATION OF SOLUTIONS • A 350 mL sample of drinking water was analyzed and found to contain 0.0046 g of sulfate salts. Calculate the concentration of sulfate salts in this water sample? • Masswater = densitywater (Volumewater) = 1.00 g/mL (350 mL) = 350 g solution ppm = (masssolute/masssolution) 106 ppm = (0.0046g / 350 g ) 106 ppm = 13 ppm Use ppm for trace amounts of solute.

  5. PRACTICE PROBLEMS calculating the CONCENTRATION OF SOLUTIONS ___1. How many grams of a 45.0 % Mg(OH)2 solution can be made from 7.00 g of solid Mg(OH)2? ___2. How many kilograms of a 6.8% KC2H3O2 solution will contain 5.3 moles of KC2H3O2? ___3. If 134.5 g of a 25.0 % sucrose solution was prepared, how many grams of a 5.00% solution of sucrose would contain the same amount of sugar? 15.6 g 7.6 kg 673 g

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