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CHEM 115 HW 5
Course: CHEM 162 162, Spring 2011School: Washington
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pointsAll 1.1/1 Submissions NotesQuestion: ZumChemP6 17.E.014. Calculate the sodium ion concentration when 65.0 mL of 3.2 M sodium carbonate is added to 25.0 mL of 1.6 M sodium bicarbonate. M 2.1/1 pointsAll Submissions NotesQuestion: ZumChemP6 17.E.018. A bottle of wine contains 12.5% ethanol by volume. The density of ethanol (C2H5OH) is 0.789 g/cm . Calculate the concentration of ethanol in wine in terms...
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pointsAll 1.1/1 Submissions NotesQuestion: ZumChemP6 17.E.014.
Calculate the sodium ion concentration when 65.0 mL of 3.2 M sodium carbonate is added to 25.0 mL of 1.6 M sodium bicarbonate. M
2.1/1 pointsAll Submissions NotesQuestion: ZumChemP6 17.E.018.
A bottle of wine contains 12.5% ethanol by volume. The density of ethanol (C2H5OH) is 0.789 g/cm . Calculate the concentration of ethanol in wine in terms of mass percent and molality. mass percent molality m
3
3.1.5/1.5 pointsAll Submissions NotesQuestion: ZumChemP6 17.E.026.
(a) Use the following data to calculate the enthalpy of hydration for calcium chloride and calcium iodide.
calcium chloride calcium iodide attracted to water? iodide chloride kJ
kJ
(b) Based on your answers to part (a), which ion, Cl or I , is more strongly
*Lattice energy was defined in Chapter 8 as the energy change for the process M (g) + X (g)
+
MX(s).
4.1.5/1.5 pointsAll Submissions NotesQuestion: ZumChemP6 17.E.028.
Which ion in each of the following pairs would you expect to be more strongly hydrated?
(a) Mg2+ Na+ (b) Be Mg (c) Fe3+ Fe2+ (d) F Br (e) Cl ClO4 (f) ClO4 SO42 5.1.5/1.5 pointsAll Submissions NotesQuestion: ZumChemP6 17.E.030. Why? Why?
2+ 2+
Why? Why? Why? Why?
Which solvent, water or carbon tetrachloride, would you choose to dissolve each of the following? (a) CH2=CH2 (b) SF2 (c) CO2
6.1/1 pointsAll Submissions NotesQuestion: ZumChemP6 17.E.035.
The solubility of nitrogen in water is 8.21 10 mol/L at 0C when the N2 pressure above water is 0.790 atm. Calculate the Henry's law constant for N2 in units of Latm/mol for Henry's law in the form P = kC, where C is the gas concentration in mol/L. atm/mol Calculate the solubility of N2 in water when the partial pressure of nitrogen above water is 1.20 atm at 0C. mol/L
4
7.1/1 pointsAll Submissions NotesQuestion: ZumChemP6 17.E.038.
Glycerin (C3H8O3) is a nonvolatile liquid. What is the vapor pressure of a
solution made by adding 103 g of glycerin to 358 mL of H2O at 39.8C? The vapor pressure of pure water at 39.8C is 54.74 torr and its density is 0.992 g/cm . torr
3
8.1/1 pointsAll Submissions NotesQuestion: ZumChemP6 17.E.040.
Which of the following will have the lowest total vapor pressure at 25C? pure water (vapor pressure = 23.8 torr at 25C) a solution of glucose in water with C6H12O6 = 0.01 a solution of methanol in water with CH3OH = 0.2 (Consider the vapor pressure of both methanol [143 torr at 25C] and water.) a solution of sodium chloride in water with NaCl = 0.01
9.1/1 pointsAll Submissions NotesQuestion: ZumChemP6 17.E.042.
A solution is prepared by mixing 0.0234 mol CH2Cl2 and 0.0339 mol CH2Br2 at 25C. Assuming the solution is ideal, calculate the composition of the vapor (in terms of mole fractions) at 25C. At 25C, the vapor of pressures pure CH2Cl2 and pure CH2Br2 are 133 and 11.4 torr, respectively.
V CH2Cl2
V CH2Br2
10.1/1 pointsAll Submissions NotesQuestion: ZumChemP6 17.E.057.
A solution is prepared by dissolving 21.0 g of urea [(NH2)2CO], in 119.0 g of water. Calculate the boiling point of the solution. Urea is a nonelectrolyte. C
11.1/1 pointsAll Submissions NotesQuestion: ZumChemP6 17.E.060.
The freezing point of tbutanol is 25.50C and Kf is 9.1Ckg/mol. Usually t butanol absorbs water on exposure to air. If the freezing point of a 10.0 g sample of tbutanol is 24.59C, how many grams of water are present in the sample? g
12./1 pointsNotesQuestion: ZumChemP6 17.E.062.
If the human eye has an osmotic pressure of 8.09 atm at 25C, what concentration of solute particles in water will provide an isotonic eyedrop solution (a solution with equal osmotic pressure)? M
13./1 pointsNotesQuestion: ZumChemP6 17.E.064.
An aqueous solution of 10.00 g of catalase, an enzyme found in the liver, has a volume of 1.00 L at 27C. The solution's osmotic pressure at 27C is found to be 0.745 torr. Calculate the molar mass of catalase.
14.1.5/1.5 pointsAll Submissions NotesQuestion: ZumChemP6 17.E.075.
g/mol
Consider the following solutions. 0.010 m Na3PO4 in water 0.020 m CaBr2 in water 0.020 m KCl in water 0.020 m HF in water (HF is a weak acid.) (a) Assuming complete dissociation of the soluble salts, which solution(s) would have the same boiling point as 0.040 m C6H12O6 in water? (C6H12O6 is a nonelectrolyte.) (Select all that apply.) Na3PO4 in water CaBr2 in water KCl in water HF in water (b) Which solution would have the highest vapor pressure at 28C? Na3PO4 in water CaBr2 in water KCl in water HF in water (c) Which solution would have the largest freezingpoint depression? Na3PO4 in water CaBr2 in water KCl in water HF in water
15.1/1 pointsAll Submissions NotesQuestion: ZumChemP6 17.E.076.
From the following choices choose the one with the following.
pure water solution of C12H22O11 (m = 0.01) in water solution of NaCl (m = 0.01) in water solution of CaCl2 (m = 0.01) in water
(a) highest freezing point (b) lowest freezing point (c) highest boiling point (d) lowest boiling point (e) highest osmotic pressure 16./1 pointsNotesQuestion: ZumChemP6 17.E.080.
Calculate the freezing point and the boiling point of each of the following aqueous solutions. (Assume complete dissociation.) (a) 0.026 m MgCl2 freezing point boiling point C C (b) 0.026 m FeCl3 freezing point C boiling point C
17./1 pointsNotesQuestion: ZumChemP6 17.E.083.
A 0.660 g sample of a compound is dissolved in enough water to form 280.0 mL of solution. This solution has an osmotic pressure of 1.80 atm at 25C. If each molecule of the solute dissociates into two particles (in this solvent), what is the molar mass of this solute? g/mol
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