Solutions. Solutions. A solution is a homogeneous mixture of two or more components.

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1 Lecture 6 Solutions Solutions A solution is a homogeneous mixture of two or more components. The component whose phase is retained يسود) ) when the solution forms is called Solvent. If all components are in the same phase, the one in greatest amount will be the Solvent and other components are called Solutes. Solutions, in which water is the dissolving medium (solvent) are called aqueous solutions. The polarity in H 2 O is responsible of its great ability to dissolve several compounds. Prof. Ahmad Mahmoud Alakraa 1

Examples of solutions Solute Solvent Solution Example Gas Gas Gas Air, natural gas Gas Liquid Liquid O 2 in H 2 O, Soda Gas Solid Solid H 2 in Pt Liquid Gas Gas Moisture in air Liquid Liquid Liquid

2 Examples of solutions Solute Solvent Solution Example Gas Gas Gas Air, natural gas Gas Liquid Liquid O 2 in H 2 O, Soda Gas Solid Solid H 2 in Pt Liquid Gas Gas Moisture in air Liquid Liquid Liquid Alcohol in H 2 O Liquid Solid Solid Hg in Ag, Drops o f H 2 O in sugar Solid Gas Gas Dust in air Solid Liquid Liquid NaCl in H 2 O, sea water Solid Solid Solid Alloys (Brass, steel) Aqueous Solutions When water dissolves an ionic solid, the positive ends of the water molecules are attracted to the negatively charged anions and the negative ends are attracted to the positively charged cations. This process is called hydration. Ionic forces are replaced by stronger water ion interactions Prof. Ahmad Mahmoud Alakraa 2

3 Why do solutions form? Tendency to Randomness or Disordering This the only reason operating for gaseous solutions Solute/Solvent Attractions Like Dissolves Like Polar solvents dissolve polar substances. Ethanol, which is not ionic but polar, dissolves in H 2 O Non polar solvents dissolve non polar substances Heat of Solution H sol The amount of heat evolved or absorbed when one mole of a solute dissolves in a solvent at constant pressure to make a dilute solution Steps involved in forming a solution Separation of solute (H 1 ) and solvent (H 2 ) particles This needs energy (+veh), i.e., Endothermic Attraction of solute and solvents particles This releases energy (H 3 is ve), i.e., Exothermic H sol = H 1 +H 2 + H 3 If H 1 + H 2 =H 3 (in value but opposite signs), H sol =0 ideal solution almost equal attraction forces between solute/solute, solvent/solvent, and solute/solvent) If H 1 + H 2 H 3,H sol 0 Non ideal solution Prof. Ahmad Mahmoud Alakraa 3

4 Energy (heat) of solution When do solutions form? H sol = H 1 +H 2 + H 3 large +Ve or Ve Small +Ve or Ve Solutions does not form Dissolution of a solute in a solvent to form a solution does not involve a chemical transformation. Solutions form Prof. Ahmad Mahmoud Alakraa 4

5 Exothermic Process Endothermic Process Prof. Ahmad Mahmoud Alakraa 5

6 Potential Energy Diagrams Nature of solutes and Solvents Why oil is insoluble in water? Oil: a mixture of non polar molecules having only the weak London dispersion forces, i.e., H 1 is small +Ve Water: is a polar solvent having the relatively strong H bonding, i.e., H 2 is large +Ve OilWater interaction: is almost negligible, i.e., H 3 is small Ve H sol = H 1 +H 2 + H 3 = large +Ve Solution does notform Prof. Ahmad Mahmoud Alakraa 6

Nature of solutes and Solvents Why NaCl is soluble in water? NaCl: is an ionic solid having the strong ionic bond, i.e., H 1 is large +Ve Water: is a polar solvent having the relatively strong H bonding, i.

7 Nature of solutes and Solvents Why NaCl is soluble in water? NaCl: is an ionic solid having the strong ionic bond, i.e., H 1 is large +Ve Water: is a polar solvent having the relatively strong H bonding, i.e., H 2 is large +Ve NaClWater interaction: is strong, i.e., H 3 is large Ve H sol = H 1 +H 2 + H 3 = small +Ve +3.9 kj mol 1 A Solution forms Nature of solutes and Solvents Prof. Ahmad Mahmoud Alakraa 7

8 Nature of solutes and Solvents Polar solvents don't dissolve nonpolar solutes Polar solvents dissolve polar solutes Strong Electrolytes Substances that are completely ionized (i.e., conduct electricity efficiently) when they are dissolved in water. Examples include soluble salts, strong acids, and strong bases. Prof. Ahmad Mahmoud Alakraa 8

Examples include weak acids (acetic acid) and weak bases (ammonia). HC2H3O2( aq.

9 Weak Electrolytes Substances that exhibit a small degree of ionization in water (i.e., conduct only a small current). They produce relatively few ions when dissolved in water. Examples include weak acids (acetic acid) and weak bases (ammonia). HC2H3O2( aq.) H2O( l) H3O ( aq) C2H3O2 ( aq) Nonelectrolytes Substances that dissolve in water but do not produce any ions (i.e., non conductors for electricity). Examples include ethanol and glucose Prof. Ahmad Mahmoud Alakraa 9

10 Composition of Solutions Mass of a solute per mass of solventor solution Mole fraction and Mole percent, Mass fraction and Mass percent, Molality Mass of a solute per Volume of solution Molarity Normality Mole fraction Theratiooftheno.ofmolesofagiven component in a solution to the total no. of moles of all components Unitless X A n A n B n n C A... n X i 1 Mole Percent is the mole fraction multiplied by 100 Z Prof. Ahmad Mahmoud Alakraa 10

11 Mass fraction The ratio of the mass of a given component in a solution to the total mass of all components ma ( mass fraction) A m m m... m Unitless A ( mass fraction) 1 Mass Percent is the mass fraction multiplied by 100 A solution labeled 0.9 % NaCl means 0.9 g NaCl is dissolved in 99.1 g H 2 O or 100 g of solution B i C Z Molality (Molal concentration) The no. of moles of solute dissolved in 1 kg of solvent nsolute m mass of solvent (kg) m w Mwt solute solute 1000 w ( g) solvent n solute : moles of solute Mwt solute : molar mass of solute W solute : mass of solute W solvent : mass of solvent Prof. Ahmad Mahmoud Alakraa 11

12 w Molarity (Molar concentration) The no. of moles of solute dissolved in 1 liter of solution nsolute wsolute M Volume of solution ( L) Mwt V ( L) n solute : no. of moles of solute Mwt solute : molar mass of solute W solute : mass of solute V : Volume of solution in liter solute solute ( g) M( mol / L) Mwt ( g / mol) V ( L) solute Normality The number of equivalents of solute per liter of solution mass No. Equivalent Equivalent mass wsolute Eq.wt solute solute solute (g) (g / equivalent ) The definition of the equivalent mass and equivalent depends on the reaction taking place in the solution. Prof. Ahmad Mahmoud Alakraa 12

13 Acid base reactions Equivalent mass An equivalent is the mass of acid or base that can furnish or accept exactly 1 mole of protons (H + ions). Acid/Base Eq.wt No of Mwt, g/mol Equivalent mass molar mass replacable H or OH M/N relationship HCl M = 1N H 2 SO /2 = 49 1M = 2N NaOH M = 1N Ca(OH) /2 = 37 1M = 2N Equivalent mass Oxidation reduction reactions The equivalent is defined as the quantity of oxidizing or reducing agent that can accept or furnish 1 mole of electrons. 2 MnO4 8H 5e Mn 4H2O For example, MnO 4 reacts in acidic solution absorbing five electrons to produce Mn 2+ : Equivalent mass of KMnO molar mass 158 g g Prof. Ahmad Mahmoud Alakraa 13

14 Equivalent mass Salts reactions Equivalent mass of a salt molar mass no.of ions its valency NaCl: Eq. wt = MWt/1 Na 3 PO 4 : Eq.Wt = Mwt / 3 Normality N no. equivalentssolute Volume of solution ( L) w Eq. wt solute solute V ( L) w n solute : no. of moles of solute Eq.wt solute : Equivalent mass of solute W solute : mass of solute V: Volume of solution in liter solute ( g) N (equivelents/l) Eq. wt solute (g/equivalents) V ( L) Prof. Ahmad Mahmoud Alakraa 14

15 Exercise A solution is prepared by mixing 1.00 g ethanol (C 2 H 5 OH) with g water to give a final volume of 101 ml. Calculate the molarity, mass percent, mole fraction, and molality of ethanol in this solution. Solution wsolute M Mwtsolute V ( L) 1.0 g g mol 101 ml M molar mass of ethanol = g/mol ml L mol/l mass percent of ethanol m % m ethanol ethanol m water 100 nethanol Xethanol nethanol nwater 1.0 g g mol 1.0 g g g mol 18.0 g mol Prof. Ahmad Mahmoud Alakraa 15

wethanol m Mwte tanol 1.0 g 46.07 g mol 1000 wwater ( g) 1000 0. 217 mol kg 1 100.0 ( g) 1 0.

16 wethanol m Mwte tanol 1.0 g g mol 1000 wwater ( g) mol kg ( g) m Exercise molar mass of sulfuric acid= 98 g/mol The electrolyte in automobile lead storage batteries is a 3.75 M sulfuric acid solution that has a density of g/ml. Calculate the mass percent, molality, and normality of the sulfuric acid? Solution d = g/ml = 1230 g/l means we have 1230 g solution (H 2 SO 4 +H 2 O) in every liter of solution (H 2 SO 4 + H 2 O) Molarity of H 2 SO 4 =3.75M means we have 3.75 mole (368 g) ofh 2 SO 4 in every liter of solution (H 2 SO 4 + H 2 O) Prof. Ahmad Mahmoud Alakraa 16

17 1L Solution 1230 g H 2 SO 4 + H 2 O 368 g H 2 SO 4 mass of water in1l solution g mass percent of ethanol msulfuric acid 100 msulfuric acid mwater % N w m Mwt 368 g 98 g mol sufuric acid sufuric acid 1000 wwater ( g) ( g) 1 M equivalents per liter m ( N) Prof. Ahmad Mahmoud Alakraa 17

18 Solubility The mass of solute necessary to form a saturated solution with a given mass of solvent at a specific temperature. Its unit is usually expressed in g solute/100 g solvent or in mole solute/g solvent. A saturated solution: is a solution containing the maximum amount of solute soluble in a definite amount of solvent at a given temperature (equilibrium concentration) Supersaturated solutions A supersaturated solution: is a solution containing more solutes than the equilibrium amount. It is unstable and tends to move towards saturation under proper conditions Unsaturated solution Saturated solution Supersaturated solution Prof. Ahmad Mahmoud Alakraa 18

19 Solubility and equilibrium In saturated solutions, a dynamic equilibrium exists between the undissolved solute and the soluble solute in solution Solute undissolved Solute Factors affecting solubility Temperature Pressure Concentration Nature of solutes and solvents dissolved Effect of Temp. on the Solubility of a gas in a liquid At constant pressure, the solubility of gases in liquids always decreases with T. The reasons are complicated where a very close competition exists between the two parameters responsible for solution formation (randomness and attractions) Prof. Ahmad Mahmoud Alakraa 19

20 Effect of Temp. on the Solubility of solids and liquids in liquids Solute undissolved Solute dissolved If equilibrium is distorted by any factor, the equilibrium will shift toward the direction restoring equilibrium (Le Chatelier Principle) For endothermic reactions Solute undissolved heat Solute dissolved Increasing temperature shifts the reaction to right increasing the solubility of the solute Effect of Temp. on the Solubility of solids and liquids in liquids For exothermic reactions Solute undissolved Solute dissolved heat Increasing temperature shifts the reaction to left lowering thesolubility ofthesolute Prof. Ahmad Mahmoud Alakraa 20

21 Effect of Pressure on the Solubility of gases Pressure has a significant effect in case of gaseous solutes since liquids and solids are incompressible Carbonated beverages, for example, are always bottled at high pressures of carbon dioxide to ensure a high concentration of carbon dioxide in the liquid. The fizzing that occurs when you open a can of soda results from the escape of gaseous carbon dioxide, because under these conditions the pressure of CO 2 above the solution is now much lower than that used in the bottling process. Effect of Pressure on the Solubility of gases Consider a closed container that is partially filled with a solution (gas in liquid) Gas Solvent Solution The gas molecules are entering and leaving the solution at the same rate. If P is suddenly increased, the number of gas molecules per unit volume increases, and the gas enters the solution at a higher rate than it leaves. As the concentration of dissolved gas increases, the rate of the escape of the gas also increases until a new equilibrium is reached, where the solution contains more dissolved gas than before. Prof. Ahmad Mahmoud Alakraa 21

Effect of Pressure on the Solubility of gases Pressure increase new equilibrium with higher solubility Henry s law The amount of a gas dissolved in a solution is directly proportional to the pressure

22 Effect of Pressure on the Solubility of gases Pressure increase new equilibrium with higher solubility Henry s law The amount of a gas dissolved in a solution is directly proportional to the pressure of the gas above the solution. C kp C: concentration of the dissolved gas, K: a constant characteristic of a particular solution, P: the partial pressure of the gaseous solute above the solution. Prof. Ahmad Mahmoud Alakraa 22

23 Henry s law Henry s law is obeyed most accurately for dilute solutions of gases that do not dissociate in or react with the solvent. For example, Henry s law is obeyed by oxygen gas in water, but it does not correctly represent the behavior of gaseous hydrogen chloride in water because of the dissociation reaction HCl H 2 O H ( aq) Cl ( aq ) Exercise Solution A certain soft drink is bottled so that a bottle at 25 C contains CO 2 gas at a pressure of 5.0 atm over the liquid. Assuming that the partial pressure of CO 2 in the atmosphere is atm, calculate the equilibrium concentrations of CO 2 in the soda both before and after the bottle is opened. The Henry s law constant for CO2 in aqueous solution is mol/l. atm at 25 C. Before Opening 2 C kp ( mol / L. atm) (5.0 atm) 0.16 mol / L After Opening C kp ( mol / L. atm) (4.010 atm) mol / L Note the large change in concentration of CO 2. This is why soda goes flat after being open for a while. Prof. Ahmad Mahmoud Alakraa 23

24 Effect of structure on the Solubility Solubility is favored if the solute and solvent have similar polarities. Since it is the molecular structure that determines polarity, there should be a definite connection between structure and solubility. Effect of structure on the Solubility soluble in nonpolar materials such as body fat hydrophobic (water fearing) water soluble hydrophilic (water loving) Prof. Ahmad Mahmoud Alakraa 24

25 Vapor pressures of solutions Think Why? We add antifreeze to water in a car s cooling system to prevent freezing in winter and boiling in summer. We also melt ice on sidewalks and streets by spreading salt. The answer is simply because of the solute s effect on the solvent s properties Colligative properties Properties that depend only on the number (concentration) of solute particles in a solution and do not depend on the identity of the solute. Consider two aqueous solutions of the same concentration; one containing glucose and the other containing urea. The impact of solute on the solvent s properties is the same for both solutions. Prof. Ahmad Mahmoud Alakraa 25

Colligative properties Vapor pressure lowering Boiling point elevation Freezing point depression Osmotic pressure generating Vapor pressure Lowering The dissolution of a nonvolatile solute in a

26 Colligative properties Vapor pressure lowering Boiling point elevation Freezing point depression Osmotic pressure generating Vapor pressure Lowering The dissolution of a nonvolatile solute in a solvent decreases the number of solvent molecules per unit volume. It should proportionately lower the escaping tendency of the solvent molecules. Pure Solvent Solution Prof. Ahmad Mahmoud Alakraa 26

27 Raoult's law The change in vapor pressure is proportional to the quantity of the dissolved solute. P solution X solvent P o solvent P solution : the vapor pressure of the solution (impure solvent) X solvent : the mole fraction of the solvent P 0 solvent : is the vapor pressure of the pure solvent. Exercise Calculate the expected vapor pressure at 25 C for a solution prepared by dissolving g common table sugar (sucrose, molar mass g/mol) in cm 3 of water. At 25 C, the density of water is g/cm 3 and the vapor pressure is torr g Answer Number of moles of sucrose mol g / mol cm g/cm Number of moles of H2O mol 18 g / mol o Psolution X solvent Psolvent torr torr Prof. Ahmad Mahmoud Alakraa 27

28 Ideal (liquid liquid) solutions Both liquids are volatile Obey Raoult s Law P T P A P B X A P o A X B P o B Ideal (liquid liquid) solutions Prof. Ahmad Mahmoud Alakraa 28

29 Ideal (liquid liquid) solutions Ideal (liquid liquid) solutions Prof. Ahmad Mahmoud Alakraa 29

30 Ideal (liquid liquid) solutions Ideal (liquid liquid) solutions Prof. Ahmad Mahmoud Alakraa 30

31 Ideal (liquid liquid) solutions Non Ideal solutions Both liquids are volatile Disobey (deviate from) Raoult s Law Prof. Ahmad Mahmoud Alakraa 31

32 Non Ideal solutions Non Ideal solutions Prof. Ahmad Mahmoud Alakraa 32

33 Negative Deviation Positive Deviation Prof. Ahmad Mahmoud Alakraa 33

34 Ideal/Non ideal behavior no deviation Ideal solution ve deviation Strong solutesolvent Interactions +ve deviation Weak solutesolvent Interactions Exercise A solution is prepared by mixing 5.81 g acetone (M.wt. = 58.1 g/mol) and 11.9 g chloroform (M.wt. = g/mol). At 35 o C this solution has a total v.p. of 260 torr. Is this an ideal solution? The v.p. of pure acetone and pure chloroform at 35 o C are 345 and 293 torr, respectively. P T P A P B X A P o A X B P o B ve deviation > Prof. Ahmad Mahmoud Alakraa 34

11/4/2017. General Chemistry CHEM 101 (3+1+0) Dr. Mohamed El-Newehy. Chapter 4 Physical Properties of Solutions

11/4/2017. General Chemistry CHEM 101 (3+1+0) Dr. Mohamed El-Newehy. Chapter 4 Physical Properties of Solutions General Chemistry CHEM 11 (3+1+) Dr. Mohamed El-Newehy http://fac.ksu.edu.sa/melnewehy Chapter 4 Physical Properties of Solutions 1 Types of Solutions A solution is a homogenous mixture of 2 or more substances.