None At a certain temperature the vapor pressure of pure acetic acid (HCH3CO2) is measured to be 403. mmHg. Suppose asolution is prepared by mixing 60.6 g of acetic acid and 64.0 gof acetone((CH3)2CO).Calculate the partial pressure of acetic acid vapor above this solution. Be sure your answer has the correct number ofsignificant digits.Note for advanced students: you may assume the solution is ideal.

Step 1: Determine the number of moles of acetic acid. Note that the molar mass of acetic acid is…

Answered: At a certain temperature the vapor…

Introductory Chemistry For Today

8th Edition

ISBN:9781285644561

Author:Seager

Publisher:Seager

Chapter7: Solutions And Colloids

Section: Chapter Questions

Problem 7.86E

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6-21 Are mixtures of gases true solutions or heterogeneous mixtures? Explain.
6-111 As noted in Section 6-8C, the amount of external pressure that must be applied to a more concentrated solution to stop the passage of solvent molecules across a semipermeable membrane is known as the osmotic pressure The osmotic pressure obeys a law similar in form to the ideal gas law (discussed in Section 5-4), where Substituting for pressure and solving for osmotic pressures gives the following equation: RT MRT, where M is the concentration or molarity of the solution. (a) Determine the osmotic pressure at 25°C of a 0.0020 M sucrose (C12H22O11) solution. (b) Seawater contains 3.4 g of salts for every liter of solution. Assuming the solute consists entirely of NaCl (and complete dissociation of the NaCI salt), calculate the osmotic pressure of seawater at 25°C. (c) The average osmotic pressure of blood is 7.7 atm at 25°C. What concentration of glucose (C6H12O6) will be isotonic with blood? (d) Lysozyme is an enzyme that breaks bacterial cell walls. A solution containing 0.150 g of this enzyme in 210. mL of solution has an osmotic pressure of 0.953 torr at 25°C. What is the molar mass of lysozyme? (e) The osmotic pressure of an aqueous solution of a certain protein was measured in order to determine the protein's molar mass. The solution contained 3.50 mg of protein dissolved in sufficient water to form 5.00 mL of solution. The osmotic pressure of the solution at 25°C was found to be 1.54 torr. Calculate the molar mass of the protein.
6-60 Predict which of these covalent compounds is soluble in water. (a) C2H6 (b) CH3OH (c) HF (d) NH3 (e) CCI4
Instead of using NaCl to melt the ice on your sidewalk you decide to use CaCl2. If you add 35.0 g of CaCl2 to 150. g of water, what is the freezing point of the solution? (Assume i = 2.7 for CaCl2.)
The solubility of lead nitrate at 100C is 140.0 g/100 g water. A solution at 100C consists of 57.0 g of lead nitrate in 64.0 g of water. When the solution is cooled 10C to 25.0 g of lead nitrate crystallize out. What is the solubility of lead nitrate in g/100 g water at 10C?
In the 1986 Lake Nyos disaster (see the chapter introduction), an estimated 90 billion kilograms of CO2 was dissolved in the lake at the time. (a) What volume of gas is this at standard temperature and pressure? (b) Assuming that this dissolved gas was in equilibrium with the normal partial pressure of CO2 in the atmosphere (0.038%, or 0.29 torr), use the Henrys law constant for CO2 in water to estimate the volume of Lake Nyos.
Samples of each of the substances listed below are dissolved in 125 g of water. Which of the solutions has the highest boiling point? (a) 3.0 g sucrose, C12H22O11 (b) 1.0 g glycerol, C3H3(OH)3 (c) 1.0 g propylene glycol, C3H6(OH)2 (d) 2.0 g glucose, C6H12(OH)2
A certain liquid X has a normal freezing point of 0.90°C and a freezing point depression constant Kf=6.96·°C·kgmol−1.A solution is prepared by dissolving some barium hydroxide (Ba(OH)2) in 900.g of X. This solution freezes at−3.7°C. Calculate the mass of Ba(OH)2 that was dissolved. Round your answer to 2 significant digits.
A certain liquid X has a normal freezing point of −4.40°C and a freezing point depression constant =Kf2.42·°C·kgmol−1 .Calculate the freezing point of a solution made of 24. g of barium hydroxide ( BaOH2 ) dissolved in 500.g of X . Round you answer to 2 significant digits.
A certain liquid X has a normal freezing point of 7.10°C and a freezing point depression constant =Kf3.27·°C·kgmol−1. A solution is prepared by dissolving some ammonium chloride (NH4Cl) in 700.g of X. This solution freezes at 6.4°C. Calculate the mass of NH4Cl that was dissolved. Round your answer to 1 significant digit. __g
A certain liquid X has a normal freezing point of 3.00°C and a freezing point depression constant Kf=6.96·°C·kgmol−1. Calculate the freezing point of a solution made of 80.7 g of benzamide (C7H7NO) dissolved in 900.g of X. Round your answer to 3 significant digits.
- 1 A certain liquid X has a normal freezing point of –1.00 °C and a freezing point depression constant K,=2.88 °C·kg•mol *. A solution is prepared by dissolving some zinc chloride (ZnCl,) in 350. g of X. This solution freezes at -2.1 °C. Calculate the mass of ZNC1, that was dissolved. Be sure your answer is rounded to the correct number of significiant digits. alo 18.2 g Ar х10

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