JokeJoke

• Why are chemists great for solving problems?

• They have all the solutions.

• Why are chemists great for solving problems?

• They have all the solutions.

Joke 2 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.

WILHELM CONRAD RÖNTGEN 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 1901.

• 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.

Labor to keep alivein your breast that

little spark of celestialfire called

CONSCIENCE.

Labor to keep alivein your breast that

little spark of celestialfire called

CONSCIENCE.

Acids and BasesAcids and Bases

Lesson 1Lesson 1

Solute Solute

• Substance being dissolved.• Substance being dissolved.

Solvent Solvent

• Substance doing the dissolving.

• Substance doing the dissolving.

Water: The Super SolventWater: 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.

Concentration Concentration

• The amount of solute per solvent.

• The amount of solute per solvent.

Dilute 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)

Concentrated 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.)

Unsaturated solution Unsaturated solution

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

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

Saturated solution Saturated solution

• Solution holds the maximum amount of solute under given conditions.

• Solution holds the maximum amount of solute under given conditions.

Supersaturated solution 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.

Aqueous Solution (aq) 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.

Molarity Molarity

• moles of solute / liter of solution.

• ( mol / L or M)

• moles of solute / liter of solution.

• ( mol / L or M)

Problem 1Problem 1

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

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

WorkWork

• First need to find the molar mass of Copper II Sulfate

• Mass = 159.62 g CuSO4

• Remember 1M can be written as 1 mol

1 L

• First need to find the molar mass of Copper II Sulfate

• Mass = 159.62 g CuSO4

• Remember 1M can be written as 1 mol

1 L

WorkWork

• 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

Work ContWork Cont

• Start with given

1mol CuSO4 159.62 g CuSO4 .1 L

1 L 1 mol CuSO4

Answer = Place 15.96 g CuSO4 in a flask and

add 100 ml of H20.

• Start with given

1mol CuSO4 159.62 g CuSO4 .1 L

1 L 1 mol CuSO4

Answer = Place 15.96 g CuSO4 in a flask and

add 100 ml of H20.

Problem 2Problem 2

• How would you prepare 1.0 L of a 0.15M sodium chloride solution?

• How would you prepare 1.0 L of a 0.15M sodium chloride solution?

WorkWork• First determine the molar mass of NaCl.

• Mass = 58.45 g NaCl

0.15 mol NaCl 58.45 g NaCl 1L 1 L 1 mol NaCl Answer = Put 8.77 g of NaCl in a flask

and add 1 L of H2O.

• First determine the molar mass of NaCl.

• Mass = 58.45 g NaCl

0.15 mol NaCl 58.45 g NaCl 1L 1 L 1 mol NaCl Answer = Put 8.77 g of NaCl in a flask

and add 1 L of H2O.

Problem 3Problem 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?

• 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?

WorkWork• First find the molar mass of

KCl

• KCl = 74.55 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 = 74.55 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).

WorkWork

32.0 g KCl 1 mol KCl .955 L 74.55 g KCl

Answer = .45 mol/L KCl or .45 M KCl

32.0 g KCl 1 mol KCl .955 L 74.55 g KCl

Answer = .45 mol/L KCl or .45 M KCl