Solution Concentration. Solute Solvent Concentration Molarity Molality ph

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1 Solution Concentration Solute Solvent Concentration Molarity Molality ph

2 Lets Review Mixture: A mixture is a chemical substance which is a homogeneous or heterogeneous association without chemical bonding of elements and/or compounds in varying proportions and that retain their own individual properties and makeup. Remember that you can see the parts

3 Zado, B. (2005). Lets Review Solution: A solution is a homogenous mixture of two or more substances in a single physical state. Remember that you cannot see the parts

4 How do we put it all together? mixtures heterogeneous homogeneous solutions electrolytes Aqueous solutions

5 How would you describe this picture?

6 Concentrated vs. Dilute In the tea example, the dark colored tea, is referred to strong tea, in chemistry we would say it is a concentrated solution of tea The lighter colored tea, would be referred to as weak tea, in chemistry we would say it is a dilute solution

7 What are Solutions? One compound is dissolved in another Solute substance being dissolved (tea) Solvent substance doing the dissolving (water)

8 In the tea example A concentrated solution a relatively large amount of solute (tea) is dissolved in the solvent (water) Concentration of solvent is High A dilute solution relatively little tea is dissolved in water Concentration of solvent low

9 Definitions Solutions can be classified as saturated or unsaturated. A saturated solution contains the maximum quantity of solute that dissolves at that temperature. An unsaturated solution contains less than the maximum amount of solute that can dissolve at a particular temperature

10 What makes up a solution? Solute: the substance being dissolved Solvent: the substance doing the dissolving Name the solute and solvent: solution solute(s) solvent Ocean water Coca-cola salt Sugar, carbon dioxide water water Humid air Water vapor air

11 Supersaturated Saturated Unsaturated

12

13 The Dead Sea The Dead Sea receives water from several streams but has no outflow The water is evaporated which concentrates the salt Uninhabitable for fishes but nearly impossible for swimmers to sink!

14 Human Blood The blood in our bodies has a certain concentration of salt This salt solution must be carefully matched

15 Molarity

16 Concentration of Solute The amount of solute in a solution is given by its concentration. Molarity (M) = moles solute liters of solution

17 PROBLEM: Dissolve 5.00 g of NiCl 2 6 H 2 O in enough water to make 250 ml of solution. Calculate the Molarity. Step 1: Calculate the # of moles of NiCl 2 6H 2 O 5.00 g 1 mol g = mol Step 2: Calculate Molarity mol L = M [NiCl 2 6 H 2 O ] = M

18 Find the Molarity If you have 1.0L of sodium chloride solution and 8.8g of sodium chloride What is the Molarity? 8.8gNaCl 1mol NaCl = 0.15mol/L NaCl or 0.15M gNaCl 1.0 L solution

19 Find mass from Molarity What mass of sucrose,c 12 H 22 O 11 must be dissolved to make 460mL of 1.10M solution? Find: Mass C 12 H 22 O 11 Given: 460mL of 1.10M solution

20 Find mass from Molarity Molar mass of sucrose = g/mol 460mL soln 1L 1.10mol C 12 H 22 O g C 12 H 22 O 11 = mL 1L solution 1mol C 12 H 22 O g C 12 H 22 O 11

21 Use Molarity to make Solutions We can use Molarity to prepare solutions

22 Making Solutions How would you prepare 2.50L of a 0.800M solution of Potassium Nitrate? Find: mass of KNO 3 Given: 2.50L of 0.800M KNO 3

23 KNO 3 Molar mass: g/mol 2.50L soln mol KNO g KNO 3 = 1 1L soln. 1mol KNO 3 202g KNO 3 To make this solution, dissolve 202g KNO 3 in 2.50L of solution.

24 Dilution To dilute a solution means to add more solvent without the addition of more solute If the amount of solute is unchanged then: Moles before dilution = Moles after dilution

25 Dilution continued Molarity = moles of solute equals the molarity times volume M = mol/l or mol = MV Moles before dilution = Moles after dilution Then: M 1 V 1 = M 2 V 2 1 = before dilution 2 = after dilution

26 Dilution Example 53.4mL of a 1.50M solution of NaCl is on hand, but you need some 0.800M solution. How many ml of 0.800M can you make? Find: V 2 or ml of 0.800M solution Given: M 1 = 1.50M, M 2 = 0.800M V 1 = 53.4mL

27 Dilution Example M 1 V 1 = M 2 V 2 Rearrange our equation to get find by itself V 2 = M 1 V 1 M 2 V 2 = (1.50mol/L)(53.4ml) = 100mL (0.800mol/L)

28 Another Example How many ml must be added to 500.mL of 6.00M NaOH to make a solution that is 2.75M? Find: Final Volume Given: M 1 = 6.00M M 2 = 2.75M V 1 = 500mL

29 Dilutions V 2 = M 1 V 1 M 2 V 2 = (6.00M) (500.ml) = 1090 ml (2.75M) ml added = V 2 V 1 ml added = 590. ml

30 Molality

31 Two Other Concentration Units MOLALITY, m m of solution = mol solute kilograms solvent % by mass % by mass = grams solute grams solution

32 Calculating Concentrations Dissolve 62.1 g (1.00 mol) of ethylene glycol in Calculate molality 250. g of H 2 O. Calculate m & % of ethylene glycol (by mass). conc (molality) = 1.00 mol glycol kg H 2 O 4.00 molal Calculate weight % %glycol = 62.1 g 62.1 g g x 100% = 19.9%

33 Try this molality problem 25.0 g of NaCl is dissolved in ml of water. Find the molality (m) of the resulting solution. m = mol solute / kg solvent 25 g NaCl 1 mol NaCl 58.5 g NaCl = mol NaCl Since the density of water is 1 g/ml, 5000 ml = 5000 g, which is 5 kg mol NaCl 5 kg water = m salt water

34 Review & Recap: Qualitative Descriptors Concentrated Dilute Saturated Unsaturated Supersaturated Quantitative Descriptors Molarity mols solute Liters solution Molality mols solute kg solvent Mole Fraction mols part total moles

35 Molarity, Molality, and Mole Fraction Ex. 1) How many grams of potassium chloride (KCl) are needed to prepare L of a 1.50 M solution of potassium chloride in water?

36 Molarity, Molality, and Mole Fraction Ex. 2) What is the molality of a solid solution containing 0.125g of chromium and 81.3 g of iron?

37 Molarity, Molality, and Mole Fraction Ex. 3) A gas mixture contains 45.6 g of carbon monoxide and 899 g of carbon dioxide. What is the mole fraction of carbon monoxide?

38 Molarity, Molality, and Mole Fraction Ex. 4) A gas mixture contains the following gases with the mole fractions indicated: NH 3 (0.214), Cl 2 (0.452), NH 2 Cl (0.118), and N 2 (0.175). The mixture also contains HCl gas. What is the mole fraction of HCl gas?

39 ph

40 ph Equations ph = -log[h + ] poh = -log[oh - ] ph + poh = 14 Acidic <7 Basic >7 7 = Neutral [H + ] = 10 -ph [OH - ] = 10 -poh

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