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Joke Why are chemists great for solving problems? They have all the solutions. Why are chemists great for solving problems? They have all the solutions.

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Presentation on theme: "Joke Why are chemists great for solving problems? They have all the solutions. Why are chemists great for solving problems? They have all the solutions."— Presentation transcript:

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2 Joke Why are chemists great for solving problems? They have all the solutions. Why are chemists great for solving problems? They have all the solutions.

3 Joke 2 Teacher: What is the formula for water? Student: H, I, J, K, L, M, N, O Teacher: That’s not what I taught you. Student: But you said the formula for water was….H to O. Teacher: What is the formula for water? Student: H, I, J, K, L, M, N, O Teacher: That’s not what I taught you. Student: But you said the formula for water was….H to O.

4 WILHELM CONRAD RÖNTGEN Discovered X rays, a momentous event that instantly revolutionized the field of physics and medicine. For his discovery, Röntgen received the first Nobel Prize in physics in Discovered X rays, a momentous event that instantly revolutionized the field of physics and medicine. For his discovery, Röntgen received the first Nobel Prize in physics in 1901.

5 Labor to keep alive in your breast that little spark of celestial fire called CONSCIENCE.

6 Acids and Bases Lesson 1

7 Solute Substance being dissolved.

8 Solvent Substance doing the dissolving.

9 Water: The Super Solvent Water is such a versatile solvent that it is sometimes called the universal solvent. Most of the water on Earth is not pure, but rather is present in solutions. Water is such a versatile solvent that it is sometimes called the universal solvent. Most of the water on Earth is not pure, but rather is present in solutions.

10 Concentration The amount of solute per solvent.

11 Dilute To weaken the concentration. Solution contain small amount of solute. (Ex: dilute orange juice, tea) To weaken the concentration. Solution contain small amount of solute. (Ex: dilute orange juice, tea)

12 Concentrated Solution contains large amount of solute. (Ex: Orange juice in a can, strong tea.) Solution contains large amount of solute. (Ex: Orange juice in a can, strong tea.)

13 Unsaturated solution Amount of solute dissolved is less than the solution could hold.

14 Saturated solution Solution holds the maximum amount of solute under given conditions.

15 Supersaturated solution Solution contains more solute than the usual amount and are unstable. (Increasing the temp can increase the amount of solute in solution.) They cannot permanently hold the excess solute in solution and may release it suddenly. Solution contains more solute than the usual amount and are unstable. (Increasing the temp can increase the amount of solute in solution.) They cannot permanently hold the excess solute in solution and may release it suddenly.

16 Aqueous Solution (aq) A liquid solution to which water has been added to dilute the solution. Ex: Frozen O.J. adding the 3 cans of water. Mixing an acid or base to a certain molarity by adding water. A liquid solution to which water has been added to dilute the solution. Ex: Frozen O.J. adding the 3 cans of water. Mixing an acid or base to a certain molarity by adding water.

17 Molarity moles of solute / liter of solution. ( mol / L or M) moles of solute / liter of solution. ( mol / L or M)

18 Problem 1 How would you prepare 100 ml of 1 M of Copper II Sulfate?

19 Work First need to find the molar mass of Copper II Sulfate Mass = g CuSO 4 Remember 1M can be written as 1 mol 1 L First need to find the molar mass of Copper II Sulfate Mass = g CuSO 4 Remember 1M can be written as 1 mol 1 L

20 Work Convert 100 ml to L 100 ml 1 L 1000 ml Answer =.1 L Convert 100 ml to L 100 ml 1 L 1000 ml Answer =.1 L

21 Work Cont Start with given 1mol CuSO g CuSO 4.1 L 1 L 1 mol CuSO 4 Answer = Place g CuSO 4 in a flask and add 100 ml of H 2 0. Start with given 1mol CuSO g CuSO 4.1 L 1 L 1 mol CuSO 4 Answer = Place g CuSO 4 in a flask and add 100 ml of H 2 0.

22 Problem 2 How would you prepare 1.0 L of a 0.15M sodium chloride solution?

23 Work First determine the molar mass of NaCl. Mass = g NaCl 0.15 mol NaCl g NaCl 1L 1 L 1 mol NaCl Answer = Put 8.77 g of NaCl in a flask and add 1 L of H 2 O. First determine the molar mass of NaCl. Mass = g NaCl 0.15 mol NaCl g NaCl 1L 1 L 1 mol NaCl Answer = Put 8.77 g of NaCl in a flask and add 1 L of H 2 O.

24 Problem 3 You add 32.0 g of potassium chloride to a container and add enough water to bring the total solution volume to 955 mL. What is the molarity of this solution?

25 Work First find the molar mass of KCl KCl = g Convert ml to L Divide 955 ml by 1000 =.955 L Now place the amount of (g) given over the amount of volume give (L). First find the molar mass of KCl KCl = g Convert ml to L Divide 955 ml by 1000 =.955 L Now place the amount of (g) given over the amount of volume give (L).

26 Work 32.0 g KCl 1 mol KCl.955 L g KCl Answer =.45 mol/L KCl or.45 M KCl 32.0 g KCl 1 mol KCl.955 L g KCl Answer =.45 mol/L KCl or.45 M KCl


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