Problem 2
Using concentration as a conversion factor, how many moles of solute are in \(844 \mathrm{~mL}\) of \(2.09 \mathrm{M}\) \(\mathrm{MgSO}_{4} ?\)
Problem 2
Define saturated, unsaturated, and supersaturated.
Problem 2
\(\mathrm{NaCl}\) is often used in winter to melt ice on roads and sidewalks, but calcium chloride \(\left(\mathrm{CaCl}_{2}\right)\) is also used. Which would be better (on a mole-by-mole basis), and why?
Problem 2
What quantity remains constant when you dilute a solution?
Problem 3
What is the molarity of a solution made by dissolving \(13.4 \mathrm{~g}\) of \(\mathrm{NaNO}_{3}\) in \(345 \mathrm{~mL}\) of solution?
Problem 3
A solution is prepared by combining \(2.09 \mathrm{~g}\) of \(\mathrm{CO}_{2}\) and \(35.5 \mathrm{~g}\) of \(\mathrm{H}_{2} \mathrm{O} .\) Identify the solute and solvent.
Problem 3
If \(45.0 \mathrm{~g}\) of \(\mathrm{C}_{6} \mathrm{H}_{6}\) and \(60.0 \mathrm{~g}\) of \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{CH}_{3}\) are mixed together, what is the mole fraction of each component?
Problem 3
Using concentration as a conversion factor, how many liters are needed to provide 0.822 mol of NaBr from a 0.665 M solution?
Problem 3
A \(1.88 \mathrm{M}\) solution of \(\mathrm{NaCl}\) has an initial volume of \(34.5 \mathrm{~mL}\). What is the final concentration of the solution if it is diluted to \(134 \mathrm{~mL} ?\)
Problem 4
A \(0.664 \mathrm{M}\) solution of \(\mathrm{NaCl}\) has an initial volume of \(2.55 \mathrm{~L}\). What is the final concentration of the solution if it is diluted to \(3.88 \mathrm{L?}\)
