Concentration-of-solutions.pptx
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The document discusses different types of mixtures and solutions. It defines a homogeneous mixture or solution as a mixture that is uniform in composition throughout. Salt water is given as an example of a solution. A solution is defined as a homogeneous mixture of two or more substances, consisting of a solute dissolved in a solvent. The document then discusses various terms related to solutions, such as concentration, saturated vs unsaturated, and ways of measuring concentration including molarity and mass percent. Molarity is defined as moles of solute per liter of solution. Mass percent is the mass of solute divided by the total mass of the solution. Examples are provided for calculating molarity and mass percent.
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SOLUTIONS.pptx
solution, in chemistry, a homogenous mixture of two or more substances in relative amounts that can be varied continuously up to what is called the limit of solubility. The term solution is commonly applied to the liquid state of matter, but solutions of gases and solids are possible. Air, for example, is a solution consisting chiefly of oxygen and nitrogen with trace amounts of several other gases, and brass is a solution composed of copper and zinc.
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- 2. Mixtures – a review • Mixture: a combination of two or more substances that do not combine chemically, but remain the same individual substances; can be separated by physical means. • Two types: – Heterogeneous – Homogeneous
- 3. Heterogeneous Mixture • “Hetero” means “different” • Consists of visibly different substances or phases (solid, liquid, gas) • Can be separated by filtering • Example:
- 4. Homogeneous Mixture • “Homo” means the same • has the same uniform appearance and composition throughout; maintain one phase (solid, liquid, gas) • Commonly referred to as solutions • Example: Salt Water
- 14. Solution • Solution: a mixture of two or more substances that is identical throughout (homogeneous) • can be physically separated • composed of solutes and solvents the substance being dissolved the substance that dissolves the solute Iced Tea Mix (solute) Water (solvent) Iced Tea (solution) Salt water is considered a solution. How can it be physically separated?
- 15. Solution • The solvent is the largest part of the solution and the solute is the smallest part of the solution Chemistry-Borders IPC-Solutions-Borders S O L V E N T S O L U T E
- 16. Types of Solutions Gaseous solutions – air = Oxygen + Nitrogen Liquid solutions – drinks = mix + water Solid solutions – alloys = steel, brass, etc
- 17. Concentration • the amount of solute dissolved in a solvent at a given temperature •described as dilute if it has a low concentration of solute dissolved •described as concentrated if it has a high concentration of solute dissolved
- 18. Concentration •Unsaturated - has a less than the maximum concentration of solute dissolved •Saturated - has the maximum concentration of solute dissolved (can see solid in bottom of solution) •Supersaturated -contains more dissolved solute than normally possible (usually requires an increase in temperature followed by cooling)
- 19. Molarity (M)
- 20. Molarity • Molarity is the concentration of a solution expressed in moles of solute per Liter of solution. • Molarity is a conversion factor for calculations Molarity (M) = moles of solute Liters of solution
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- 22. 2. What is the molarity of a solution that was prepared by dissolving 82.0 g of CaCl2 in enough water to make 812 mL of solution? Chemistry-Borders IPC-Solutions-Borders
- 23. 3. What is the molarity of a solution that contains 5.5 g of HCl dissolved in enough water to make 250 mL of solution? Chemistry-Borders IPC-Solutions-Borders
- 25. Mass Percent • Solutions can also be represented as percent of solute in a specific mass of solution. • For a solid dissolved in water, you use percent by mass which is Mass Percent. • % by mass = mass solute x 100 mass of solution **Mass of solution = solute mass + solvent mass
- 26. Example 1 • If a solution that has a mass of 800.0 grams contains 20.0 grams of NaCl, what is the concentration using Percent by Mass? % by mass = mass solute x 100 mass of solution % by mass = 20.0g NaCl x 100 800.0g solution = 2.50% NaCl
- 27. Example 2 • If 10.0 grams of NaCl is dissolved in 90.0 grams of water, what is the concentration using Percent by Mass? % by mass = mass solute x 100 mass of solution % by mass = 10.0g NaCl x 100 = 10.0%NaCl 100.0g solution
- 28. Example 3 • How many grams of sodium bromide are in 200.0g of solution that is 15.0% sodium bromide by mass? % by mass = mass solute x 100 mass of solution % by mass = ? g NaBr x 100 = 15.0%NaBr 200.0g solution g NaBr = 200.0 x 15.0 100 = 30 g NaBr