Chapter 12: Problem 60
Why is the amount of energy associated with the solvation step of the dissolving process so critical to whether or not a solute will dissolve?
Chapter 12: Problem 60
Why is the amount of energy associated with the solvation step of the dissolving process so critical to whether or not a solute will dissolve?
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Get started for freeAt \(0.00{ }^{\circ} \mathrm{C}\) and sea level, dry air can be assumed to have a molar volume of \(22.414 \mathrm{~L}\). Given that air is \(21.0 \%\) by volume oxygen, what is the molar concentration of oxygen in the atmosphere at sea level at \(0.00^{\circ} \mathrm{C}\) ?
After \(50.0 \mathrm{~mL}\) of a \(0.250 \mathrm{M}\) solution of calcium nitrate is combined with \(100.0 \mathrm{~mL}\) of a \(0.835 \mathrm{M}\) solution of calcium nitrate, \((\) a) what is the molar concentration of \(\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}(a q)\) in the combined solution? Once in solution, the calcium nitrate exists not as intact calcium nitrate but rather as calcium ions and nitrate ions. What are the molar concentrations (b) of \(\mathrm{Ca}^{2+}(a q)\) in the combined solution and (c) of \(\mathrm{NO}_{3}^{-}(a q)\) in the combined solution?
You have \(45.0 \mathrm{~mL}\) of a \(0.250 \mathrm{M}\) solution of sucrose, \(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\) (a) How many moles of \(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\) are present in this solution? (b) How many grams of sucrose would you recover if you evaporated all of the water off of this solution? (c) A student says that if you did part (b) and recovered all of the evaporated water as a liquid, you would get \(45.0 \mathrm{~mL}\) of liquid water. Is this student correct? Explain.
Combustion analysis reveals vitamin \(\mathrm{C}\) to be \(40.9 \%\) by mass \(\mathrm{C}\) and \(4.58 \%\) by mass \(\mathrm{H}\). The only other element present is oxygen. A solution of \(19.40 \mathrm{~g}\) of vitamin \(\mathrm{C}\) in \(100.0 \mathrm{~g}\) of water freezes at \(22.05^{\circ} \mathrm{C}\). What is the molecular formula of vitamin \(C\) ?
Your assistant tells you he measured out \(116.886\) \(\mathrm{g}\) of \(\mathrm{NaCl}\) and then added exactly \(1.00 \mathrm{~L}\) of water to it to prepare a \(2.00 \mathrm{M}\) solution of \(\mathrm{NaCl}\). Do you fire him or give him a promotion? Explain.
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