Chapter 10: Problem 56
What is the osmotic pressure of a \(0.135 \mathrm{M}\) solution of \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) at \(20^{\circ} \mathrm{C} ?\) (Assume complete dissociation.)
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The freezing point of a \(0.21 m\) aqueous solution of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) is \(-0.796^{\circ} \mathrm{C}\) (a) What is i? (b) Is the solution made up primarily of (i) \(\mathrm{H}_{2} \mathrm{SO}_{4}\) molecules only? (ii) \(\mathrm{H}^{+}\) and \(\mathrm{HSO}_{4}^{-}\) ions? (iii) \(2 \mathrm{H}^{+}\) and \(1 \mathrm{SO}_{4}^{2-}\) ions?
The Henry's law constant for the solubility of radon in water at \(30^{\circ} \mathrm{C}\) is \(9.57 \times 10^{-6} \mathrm{M} / \mathrm{mm} \mathrm{Hg} .\) Radon is present with other gases in a sample taken from an aquifer at \(30^{\circ} \mathrm{C}\). Radon has a mole fraction of \(2.7 \times 10^{-6}\) in the gaseous mixture. The gaseous mixture is shaken with water at a total pressure of 28 atm. Calculate the concentration of radon in the water. Express your answers using the following concentration units. (a) molarity (b) ppm (Assume that the water sample has a density of \(1.00 \mathrm{~g} / \mathrm{mL} .)\)
Consider an aqueous solution of urea, \(\left(\mathrm{CO}\left(\mathrm{NH}_{2}\right)_{2}\right)\) at \(26^{\circ} \mathrm{C} .\) Its vapor pressure is \(21.15 \mathrm{~mm} \mathrm{Hg}\) (vapor pressure of pure \(\left.\mathrm{H}_{2} \mathrm{O}=25.21 \mathrm{~mm} \mathrm{Hg}\right)\). How would you prepare \(250.0 \mathrm{~mL}\) of this solution \((d=1.06 \mathrm{~g} / \mathrm{mL}) ?\)
Lead is a poisonous metal that especially affects children because children retain a larger fraction of lead than adults do. To date, there is no "safe" concentration of lead in blood. Research shows that \(100 \mu \mathrm{g} / \mathrm{L}\) ( 2 significant figures) of lead in the blood of young children can cause delayed cognitive development. How many moles of lead per liter in a child's blood does \(100 \mu \mathrm{g} \mathrm{b} / \mathrm{L}\) represent? How many ppm? Assume the density of blood is \(1.00 \mathrm{~g} / \mathrm{mL}\)
When \(13.66 \mathrm{~g}\) of lactic acid, \(\mathrm{C}_{3} \mathrm{H}_{6} \mathrm{O}_{3},\) are mixed with \(115 \mathrm{~g}\) of stearic acid, the mixture freezes at \(62.7^{\circ} \mathrm{C}\). The freezing point of pure stearic acid is \(69.4^{\circ} \mathrm{C}\). What is the freezing point constant of stearic acid?
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