1. General Terms a. concentratedLots of solute dissolved in the solvent b. diluteLittle solute in the solvent 2. Specific terms a. Percent by mass Describes.

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1. General Terms a. concentratedLots of solute dissolved in the solvent b. diluteLittle solute in the solvent 2. Specific terms a. Percent by mass Describes the mass of solute in the mass of the solution Mass of solute Mass of solution X 100

Examples 1. What is the percent mass of a solution if g of solution contains 30.0 g of NaCl? 2. If we add 25.0 g of KCl to 80.0 g of water, what is the percent by mass of the solution? 3. If we want to make a 20.0% solution by mass, how much KBr must we add to make 45 g of solution? Mass of solute Mass of solution X X % To get the mass of the solution, we must add solute + solvent! Mass of solute Mass of solution X X % Mass of solute Mass of solution X 100 X 45 X g20.0 =

b. Parts per million (ppm) Used for very small concentrations. % = parts per hundred Ppm = parts per million Mass of solute Mass of solution X 1,000, ppm NH 3 10 g of NH 3 for every 1,000,000 g of solution Example 1. We determined that the air contains g of CO 2 for every 5,000.0 g of air. What is the concentration in ppm? 2. The legal amount of methyl isocyanate is ppm. How many grams of this chemical can we find in 3300 g of air? Mass of solute Mass of solution X 1,000,000 Mass of solute Mass of solution X 1,000, ,000 X 1,000, ppm X 3300 X 1,000, g0.020= 6.6 x g

c. Molarity Specific measurement of concentration Moles of solute dissolved in one liter of solution 6.0 M HCl6.0 moles of HCl dissolved in H 2 O to make one liter Formula Molarity (M) = moles of solute liters of solution

Remember, check to see if you have moles or grams, and if you are using liters or milliliters. Molarity Practice A. What is the molarity of a solution if we add 8.00 moles of LiCl to 2.00 L of water? M = moles liters M = 8.00 moles 2.00 L M = 4.00 M B. If we have g of HCl dissolved to make 2.00 L of solution, what is the molarity? Must change g to moles first! g x (36.46 g/mole) moles M = moles liters M = moles 2.00 L M = 6.85 M

C. If we have g of HCl in ml of solution, what is the molarity? Must change ml in to L! g x (36.46 g/mole) mole ml = L M = moles liters M = moles L M = M

M – moles liters M = 1.00 moles 2.50 L