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# Solution Concentrations - PowerPoint PPT Presentation

Solution Concentrations. Different ways of representing how much stuff is contained in a solution. Solution Components . Solution: a homogeneous mixture of two or more substances in a single phase

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## PowerPoint Slideshow about 'Solution Concentrations' - lucita

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### Solution Concentrations

Different ways of representing how much stuff is contained in a solution

• Solution: a homogeneous mixture of two or more substances in a single phase

• Atoms, molecules, or ions are thoroughly mixed so that the substance has a consistent composition and properties

• Solute: The substance being dissolved

• USUALLY the smaller amount

• The particles of solute are so small that they can not be seen

• Solvent: The substance doing the dissolving

Some Commonly Used Ways of Representing Concentration

• Molality

• Moles of solute per kilogram of solvent

• Percent by Volume

• Percent by Mass

• Parts per Million

• Parts per Billion

• Parts per Trillion

• Number of moles of solute per liter of solution

• What is the molarity of a solution prepared by dissolving 37.94 g of potassium hydroxide to produce a 500.0 mL solution?

• What is the molarity of a 3500.0 mL solution that contains 141.6 g of citric acid (C3H5O(COOH)3)?

• How much sodium hydroxide would be needed to produce 750.0 mL of a 6.00 M solution?

• How many grams of K2Cr2O7 are needed to make 250.0 mL of a 0.125M solution?

• In many cases, solutions are sold in high concentrations and diluted with distilled water (or other solvents) to produce a solution with a desired concentration

• Any ideas why?

• When this is the case, the number of moles is the quantity that will determine the volumes needed…

• Calculate the amount of a 12.0 M hydrochloric acid solution (HCl) that is needed to produce 500.0 mL of a 2.00 M HCl solution.

• Determine the moles of solute required for the desired solution

• Use the SAME NUMBER OF MOLES to calculate the volume of the concentrated solution that would provide this amount

• Make up the volume difference with distilled water (or other specified solvent, if you are actually making the solution)

• What volume of a 6.77 M nitric acid (HNO3) solution to produce a 250.0 mL of a 1.50 M solution?

• What is the molarity of a solution that is made by diluting 50.00 ml of a 4.74 M HCl solution to 250.0 mL?

• How much final solution would be made by adding water to 1.19 mL of a 8.00 M acetic acid solution (CH3COOH) to produce a final molarity of 1.50 M?

• What is the final molarity of an ammonium chloride solution produced by diluting 50.00 mL of a 3.79 M solution to 2.00 L?

• A 3.8 M solution of iron (II) sulfate is diluted to eight times its original volume. What is the new molarity of the solution?