Solution Concentrations

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Presentation transcript:

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 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

Molarity Number of moles of solute per liter of solution

Perform the following calculations… 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?

Preparing Solutions by Dilution 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…

Perform the following calculation 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)

Perform the following calculations… 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?

Perform the following calculations… 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?