Properties of Solutions

Name: Properties of Solutions
Uploaded: 2017-12-21T01:56:31+00:00
Duration: PTM28S59
Channel: Carmel French
Description: Properties of Solutions

Properties of Solutions
Chapter 17 Web-site:

Properties of Solutions – ch. 17
1. Predict the relative solubility of the following: a. O2 in H20 vs. O2 in CCl4 b. CH3OH in H2O vs. CH3CH2CH2CH2OH in H2O c. AgCl(s) in H2O at 25°C vs. AgCl(s) in H2O at 45°C d. CO2(g) in C8H18 at 25°C vs. CO2(g) in C8H18 at 45°C e. N2(g) in C6H6(g)at 1 atm vs. N2(g) in C6H6(g)at 8 atm

Solubility ⇒ the maximum amount of solute that can dissolve in a given amount of solvent at any one T and P Solubility Considerations: 1. Polarity of solute and solvent ⇒ “like dissolves like” 2. Temperature ⇒ Substances are more soluble at high T’s if ΔSdiss > 0 (typical for solid solutes) and less soluble at high T’s if ΔSdiss < 0 (typical for gas solutes) 3. Pressure ⇒ gases are more soluble at high P’s (Henry’s Law is an example of Le Chatlier’s principle)

2. What is the molality of an aqueous solution that is 12.5% methanol by weight (molar mass of CH3OH is g/mol). Molality ⇒ m = nsolute kgsolvent

3. Calculate the molality and mole fraction of an aqueous solution that is 8 M NaCl, the density of the solution is 1.18 g/ml. Concentrations Variations Molarity ⇒ M = nsolute Lsolution Molality ⇒ m = nsolute kgsolvent Mole fraction ⇒ Xa = n𝑎 ntotal

4. Calculate the heat of hydration for the following ionic solids. a. KF b. RbF c. Compare the ion-dipole forces for K+ vs. Rb+ in H2O Compound Lattice Energy Heat of Solution KF -804 kJ/mol -15 kJ/mol RbF -768 kJ/mol -24 kJ/mol

5. A salt solution sits in an open beaker. Assuming constant temperature, the vapor pressure of the solution will… a. increases over time b. decreases over time c. stays the same over time d. We need to know which salt is in the solution to answer this e. We need to know the temperature and pressure to answer this

Colligative properties ⇒ the properties of a solution with a non-volatile solute relative to a pure solvent As the concentration of solute particles ↑ vapor pressure ↓ “depression” ⇒ Pa = Xa Pa° freezing point ↓ “depression” ⇒ ΔTf = - kf i m boiling point ↑ “elevation” ⇒ ΔTb = kb i m osmotic pressure ↑ ⇒ π = iMRT i = vant Hoff factor = moles of solute particles moles of solute

6. Rank the following aqueous solutions in order of increasing vapor pressure: a. 0.1 M C6H12O6 b. 0.1 M KBr c M Na2SO4 d M CH3COOH

7. Calculate the vapor pressure of a solution (in torr) made by dissolving 159 g of ethylene glycol (HOCH2CH2OH – 62.08g/mol) in 500 g of water at 27 °C. At 27 °C the vapor pressure of pure water is 26.7 torr.

8. Benzene (C6H6 – g/mol) and toluene (C7H8 – g/mol) form an ideal solution. What is the vapor pressure of a solution prepared by mixing 40 g of toluene with 15 g of benzene at 25 °C? At 25 °C the vapor pressures of pure toluene and pure benzene are 28 and 95 torr respectively. What is the mole fraction of the benzene in the vapor above the solution?

9. Pentane and hexane form an ideal solution. What composition of a pentane and hexane solution at 25 °C would give a vapor pressure of 350 torr? At 25 °C the vapor pressures of pure pentane and hexane are 511 torr and 150 torr respectively.

10. After substance A is mixed with substance B the solution feels hotter than before they were mixed. What deviation from Raoult’s Law (if any) would be expected for this solution? a. no deviation b. positive deviation – A and B form stronger forces than pure A and B c. positive deviation – A and B form weaker forces than pure A and B d. negative deviation – A and B form stronger forces than pure A and B e. negative deviation – A and B form weaker forces than pure A and B

Ideal vs. Non-Ideal Solutions a. ΔHsol’n ~ 0 ⇒ Ideal solution – the actual vapor pressures will agree with Raoult’s law b. ΔHsol’n > 0 ⇒ Non-Ideal solution – the forces in the solution are weaker than in the pure substances resulting in higher VPs than expected from Raoult’s Law c. ΔHsol’n < 0 ⇒ Non-Ideal solution – the forces in the solution are stronger than in the pure substances resulting in lower VPs than expected from Raoult’s Law

11. Predict if the following solutions will be ideal or non-ideal. What type of deviation from Raoult’s Law would you expect for the non-ideal solutions? a. carbon tetrachloride (CCl4) and dichloromethane (CH2Cl2) b. water and acetone (CH3COCH3) c. carbon tetrachloride and benzene (C6H6)

12. The vapor pressures of several solutions of water and butanol were determined at various compositions and the data is given below: a. Are the solutions of water and butanol ideal? b. Which of the above solutions would have the lowest boiling point? XH2O VP (torr) 0.00 47.0 0.27 52.5 0.58 58.3 0.72 46.9 1.00 40.2

13. Rank the following aqueous solutions by their boiling points, and freezing points. a M CH2O b M LiF c M (NH4)2SO4

14. Calculate the boiling point and freezing point of a solution made by dissolving 110 g of K3PO4 (212.3g/mol) in 800 mL of water at 1 atm. For water kb = 0.51 °Ckg/mol and kf = 1.86 °Ckg/mol.

15. Calculate the osmotic pressure of a solution made by dissolving 83 g of glucose (C6H12O6) in 100 mL of water at 30 °C.

Osmosis ⇒ the diffusion of water thru a semipermeable membrane Osmotic pressure (π )⇒ the minimum pressure that must be applied to keep osmosis from occurring ⇒ π= iMRT ⇒ as the concentration gradient ↑ π↑ Reverse osmosis ⇒ increasing the conc gradient by the movement of water thru a semipermeable membrane by applying a pressure that is > the osmotic pressure

16. A solution contains 3.75 g of a nonvolatile hydrocarbon in 95 g of acetone. The boiling points of pure acetone and the solution are 55.9 °C and 56.5 °C respectively. What is the molar mass of the hydrocarbon? For acetone the Kb = 1.71 °CKg/mol.

17. A solution that contains 29 g of non-volatile/non-ionizing solute in 126 g of water has a vapor pressure of torr at 100 °C. What is the molar mass of the solute?

Properties of Solutions – ch. 17 – Feldwinn
18. A solid mixture contains MgCl2 (molar mass= 𝑔 𝑚𝑜𝑙) and NaCl (molar mass = 𝑔 𝑚𝑜𝑙). When g of this solid is dissolved in enough water to form L of solution, the osmotic pressure at 25.0˚C is observed to be atm. What is the mass percent of MgCl2 in the solid? (Assume ideal behavior for the solution.)

Properties of Solutions – Answers
1. Predict the relative solubility of the following: a. O2 in H20 vs. O2 in CCl4 b. CH3OH in H2O vs. CH3CH2CH2CH2OH in H2O c. AgCl(s) in H2O at 25°C vs. AgCl(s) in H2O at 45°C d. CO2(g) in C8H18 at 25°C vs. CO2(g) in C8H18 at 45°C e. N2(g) in C6H6(g)at 1 atm vs. N2(g) in C6H6(g)at 8 atm 2. What is the molality of an aqueous solution that is 12.5% methanol by weight (molar mass of CH3OH is g/mol). molality = 𝑚𝑜𝑙𝑒𝑠 𝑠𝑜𝑙𝑢𝑡𝑒 𝑘𝑔 𝑜𝑓 𝑠𝑜𝑙𝑣𝑒𝑛𝑡 12.% ⇒ if there’s 100 g of solution 12.5 g of CH3OH and 87.5 g of water mole of CH3OH = 12.5 𝑔 𝑔/𝑚𝑜𝑙 = 0.39 mol ⇒ m= 0.39 𝑚𝑜𝑙 𝑘𝑔 = 4.46m

3. Calculate the molality and mole fraction of an aqueous solution that is 8 M NaCl, the density of the solution is 1.18 g/ml. (molar mass of NaCl is g/mol) molality = 𝑚𝑜𝑙𝑒𝑠 𝑠𝑜𝑙𝑢𝑡𝑒 𝑘𝑔 𝑜𝑓 𝑠𝑜𝑙𝑣𝑒𝑛𝑡 and mole fraction = 𝑚𝑜𝑙𝑒𝑠 𝑁𝑎𝐶𝑙 𝑡𝑜𝑡𝑎𝑙 𝑚𝑜𝑙𝑒𝑠 8 M NaCl ⇒ 8 moles of NaCl per 1 L of solution (8 mol NaCl)(58.44 g/mol) = g NaCl (1 L of sol’n)(1000mL/L)(1.18 g/L) = 1180 g of sol’n – 467.5g = g of water 𝑔 𝑤𝑎𝑡𝑒𝑟 𝑔/𝑚𝑜𝑙 = 39.5 mol water molality = 8 𝑚𝑜𝑙 𝑘𝑔 = 11.2 m mole fraction= 8 𝑚𝑜𝑙𝑒𝑠 𝑁𝑎𝐶𝑙 𝑡𝑜𝑡𝑎𝑙 𝑚𝑜𝑙𝑒𝑠 = 0.168

4. Calculate the heat of hydration for the following ionic solids. a. KF b. RbF c. Compare the ion-dipole forces for K+ vs. Rb+ in H2O ΔHhydration = ΔHLE + ΔHsol’n KF ⇒ ΔHhydration = (-804kJ/mol) + (-15kJ/mol) = -819kJ/mol RbF ⇒ ΔHhydration = (-768kJ/mol) + (-24kJ/mol) = -792kJ/mol Since both species have fluoride we can compare the ion-dipole forces of K+ vs. Rb+ ⇒ the more negative the heat of hydration the stronger the force ⇒ K+ has the stronger ion-dipole force ⇒ this makes sense since K+ is smaller and can form shorter/stronger bonds with water

5. A salt solution sits in an open beaker. Assuming constant temperature, the vapor pressure of the solution will… b. decreases over time as water evaporates away the concentration of the salt increases causing the VP to decrease 6. Rank the following aqueous solutions in order of increasing vapor pressure: a. 0.1 M C6H12O6 ⇒ i=1 b. 0.1 M KBr ⇒ i=2 c M Na2SO4 ⇒ i=3 d M CH3COOH ⇒ i=1 as (conc)x(i) ↑ VP ↓ b < c < a < d

7. Calculate the vapor pressure of a solution (in torr) made by dissolving 159 g of ethylene glycol (HOCH2CH2OH – 62.08g/mol) in 500 g of water at 27 °C. At 27 °C the vapor pressure of pure water is 26.7 torr. (159g)/(62.08g/mol) = 2.6 mol HOCH2CH2OH (500g)/(18.02g/mol) = 27.7 mol water Pwater = (27.7mol/30.3mol)(26.7torr) = 24.4torr Relative FP or VP => b < c < a < d Relative BP or OP => b > c > a > d

8. Toluene and benzene form an ideal solution. What is the vapor pressure of a solution prepared by mixing 40 g of toluene with 15 g of benzene at 25 °C? At 25 °C the vapor pressures of pure toluene and pure benzene are 28 and 95 torr respectively. (40g)/(92.15g/mol) = 0.43 mol toluene (15g)/(78.12g/mol) = 0.19 mol benzene Ptoluene = (0.43 mol/0.62 mol)(28 torr) = 19.6 torr Pbenzene = (0.19 mol/0.62 mol)(95 torr) = 29.1 torr Psolution = 48.7 torr

9. Pentane and hexane form an ideal solution. What composition of a pentane and hexane solution at 25 °C would give a vapor pressure of 350 torr? At 25 °C the vapor pressures of pure pentane and hexane are 511 torr and 150 torr respectively. Ptotal = Ppentane + Phexane Ptotal = XpPp° + XhPh° Since Xp + Xh = 1 => Xp = 1 – Xh Ptotal = (1 – Xh) Pp° + XhPh° 350 torr = (1 – Xh)(511 torr) + Xh(150 torr) Xh = 0.45 => Xp = 0.55

10. After substance A is mixed with substance B the solution feels hotter than before they were mixed. What deviation from Raoult’s Law (if any) would be expected for this solution? d. negative deviation – A and B form stronger forces than pure A and B A hotter solution means that the heat of solution was exothermic – the heat given off is due to forming strong forces

11. Predict if the following solutions will be ideal or non-ideal. What type of deviation from Raoult’s Law would you expect for the non-ideal solutions? a. carbon tetrachloride (CCl4) and dichloromethane (CH2Cl2) non-ideal with positive deviations - CCl4 has LDF whereas CH2Cl2 is polar and has dipole-dipole in addition to the LDF – upon mixing the CH2Cl2 will be unable to have as many dipole-dipole forces and therefore weaker b. water and acetone (CH3COCH3) non-ideal with negative deviations – water is polar and can H-Bond however acetone is polar but can’t H-Bond with itself but can H-Bond with water – therefore the forces in solution are stronger c. carbon tetrachloride and benzene (C6H6) ideal - both are non-polar and will have LDFs when pure and in solution

12. The vapor pressures of several solutions of water and butanol were determined at various compositions and the data is given below: a. are the solutions of water and butanol ideal? No – since the VP’s of some of the solutions are outside of the range of pure water and pure butanol – since they are outside on the high side the solution will have positive deviations b. which of the above solutions would have the lowest boiling point? Highest VP will result in the lowest BP => XH2O = 0.58 XH2O VP (torr) 0.00 47.0 0.27 52.5 0.58 58.3 0.72 46.9 1.00 40.2

13. Rank the following aqueous solutions by their boiling points, and freezing points. a M CH2O b M LiF c M (NH4)2SO4 as (conc)x(i) ↑ FP ↓ and BP ↑ Relative FP => b < c < a Relative BP => a < c < b

14. Calculate the boiling point and freezing point of a solution made by dissolving 110 g of K3PO4 (212.3g/mol) in 800 mL of water at 1 atm. For water kb = 0.51 °Ckg/mol and kf = 1.86 °Ckg/mol. (110 g K3PO4)/(212.3g/mol) = 0.52 mol K3PO4 m = 0.52 mol/0.8 kg = 0.65m ΔTf = -(0.65 mol/kg)(4)(1.86 °Ckg/mol) = -4.8°C ΔTb = (0.65 mol/kg)(4)(0.51°Ckg/mol) = 1.3°C Since pure water has a FP = 0°C and BP = 100°C then the solution will have a FP = -4.8°C and BP = 101.3°C

15. A solution contains 3.75 g of a nonvolatile hydrocarbon in 95 g of acetone. The boiling points of pure acetone and the solution are 55.9 °C and 56.5 °C respectively. What is the molar mass of the hydrocarbon? For acetone the Kb = 1.71 °CKg/mol. molar mass = g/mol => given grams and you can get moles from ΔTb = kb i m => mol = ΔTb kgsolvent/ kb i mol = (56.5 °C – 55.9 °C)(0.095kg)/(1.71°CKg/mol)(1) mol = 0.056 molar mass = 3.75g/0.056mol = 66.8g/mol

16. Calculate the osmotic pressure of a solution made by dissolving 83 g of glucose (C6H12O6) in 100 mL of water at 30 °C. π = iMRT π = (1)((83g/180g/mol)/(01.L))( atmL/molK)(303K) π = 115 atm

17. A solution that contains 29 g of non-volatile/non-ionizing solute in 126 g of water has a vapor pressure of torr at 100 °C. What is the molar mass of the solute? molar mass = g/mol => given grams and you can get moles from Pwater = XwaterPwater° => nsolute = (nwPw°/Pw) – (nw) => nsolute = (126g/18g/mol)(760torr)/(723.4torr) – (126g/18g/mol) nsolute = moles molar mass = 29g/0.354mol = 82 g/mol

18. A solid mixture contains MgCl2 (molar mass= 𝑔 𝑚𝑜𝑙) and NaCl (molar mass = 𝑔 𝑚𝑜𝑙). When g of this solid is dissolved in enough water to form L of solution, the osmotic pressure at 25.0˚C is observed to be atm. What is the mass percent of MgCl2 in the solid? If you have X g of MgCl2 then there’s 0.50 g – X g of NaCl moles of MgCl2 = X/ = X moles of NaCl = (0.5 – X)/ = – X π = iMRT = (iM (for MgCl2)+iM (for NaCl))RT = (3(0.0105X/1) + 2(( – X)/1)( )(298) X = g % MgCl2 = (0.352g/0.5g)(100) = 70.4%

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