Chapter 13: Problem 12
You are asked to prepare \(125.0 \mathrm{mL}\) of \(0.0321 \mathrm{M} \mathrm{AgNO}_{3}\) How many grams would you need of a sample known to be \(99.81 \% \mathrm{AgNO}_{3}\) by mass?
Chapter 13: Problem 12
You are asked to prepare \(125.0 \mathrm{mL}\) of \(0.0321 \mathrm{M} \mathrm{AgNO}_{3}\) How many grams would you need of a sample known to be \(99.81 \% \mathrm{AgNO}_{3}\) by mass?
All the tools & learning materials you need for study success - in one app.
Get started for freeCalculate the mole fraction of solute in the following aqueous solutions: (a) \(21.7 \% \mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH},\) by mass; (b) \(0.684 m \mathrm{CO}\left(\mathrm{NH}_{2}\right)_{2}\) (urea).
An important test for the purity of an organic compound is to measure its melting point. Usually, if the compound is not pure, it begins to melt at a lower temperature than the pure compound.(a) Why is this the case, rather than the melting point being higher in some cases and lower in others?(b) Are there any conditions under which the melting point of the impure compound is higher than that of the pure compound? Explain.
What is the molarity of \(\mathrm{CO}_{2}\) in a liter of ocean water at \(25^{\circ} \mathrm{C}\) that contains approximately \(280 \mathrm{ppm}\) of \(\mathrm{CO}_{2} ?\) The density of ocean water is \(1027 \mathrm{kg} / \mathrm{m}^{3}\).
A certain brine has \(3.87 \%\) NaCl by mass. A \(75.0 \mathrm{mL}\) sample weighs 76.9 g. How many liters of this solution should be evaporated to dryness to obtain \(725 \mathrm{kg}\) \(\mathrm{NaCl} \)?
Use the concentration of an isotonic saline solution, \(0.92 \% \mathrm{NaCl}(\mathrm{mass} / \text { volume }),\) to determine the osmotic pressure of blood at body temperature, \(37.0^{\circ} \mathrm{C}\). [Hint: Assume that \(\mathrm{NaCl}\) is completely dissociated in aqueous solutions.]
What do you think about this solution?
We value your feedback to improve our textbook solutions.