Chapter 17: Q102AE (page 733)
Would benzoic acid be more or less soluble in a 0.1-M solution than it is in water?
Benzoic acid will be more soluble in
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Erythrocytes are red blood cells containing hemoglobin. In a saline solution, they shrivel when the salt concentration is high and swell when the salt concentration is low. In a 250C aqueous solution of NaCl whose freezing point is -0.4060C, erythrocytes neither swell nor shrink. If we want to calculate the osmotic pressure under these conditions, what do we need to assume? Why? Estimate how good (or poor) of an assumption this is. Make this assumption and calculate the osmotic pressure of the solution inside erythrocytes.
A solid mixture contains MgCl2 (molar mass = 95.218g) and NaCl (molar mass= 58.443g). When 0.5000g of this solid is dissolved in enough water to form 1.000L of the solution, the osmotic pressure at 25C is observed to be 0.3950atm. What is the mass percent of MgCl2 in a solid? Assume ideal behavior for a solution.
Plants that thrive in salt water must have internal solutions (inside the plant cells) that are isotonic (same osmotic pressure) with the surrounding solution. A leaf of a saltwater plant is able to thrive in an aqueous salt solution that has a freezing point equal to . You would like to use this information to calculate the osmotic pressure of the solution in the cell.
a. In order to use the freezing-point depression to calculate osmotic pressure, what assumption must you make (in addition to the ideal behavior of the solutions, which we will assume)?
b. Under what conditions are the assumptions in part reasonable?
c. Solve for the osmotic pressure of the solution in the plant cell.
d. The plant leaf is placed in an aqueous salt solution that has a boiling point of 102.08C. What will happen to the plant cells in the leaf?
An aqueous antifreeze solution is 40.0% ethylene glycol () by mass. The density of the solution is . Calculate the molality, molarity, and mole fraction of the ethylene glycol.
Using KF as an example, write equations that refer to and Lattice energy was defined in chapter 13 as the reaction. K+(g)+F-(g) →KF(s). Show how would you utilize Hess’s law to calculate from and for KF, where = lattice energy,for KF, as for other soluble ionic compounds, is a relatively small number. How can this be sinceandare relatively large negative numbers?
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