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Chapter 11: Problem 82
A 0.15 -g sample of a purified protein is dissolved in water to give 2.0 \(\mathrm{mL}\) of solution. The osmotic pressure is found to be 18.6 torr at \(25^{\circ} \mathrm{C}\) . Calculate the protein's molar mass.
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Calculate the normality of each of the following solutions. a. 0.250\(M \mathrm{HCl}\) b. 0.105\(M \mathrm{H}_{2} \mathrm{SO}_{4}\) c. \(5.3 \times 10^{-2} M \mathrm{H}_{3} \mathrm{PO}_{4}\) d. 0.134 \(\mathrm{M} \mathrm{NaOH}\) e. 0.00521 \(\mathrm{M} \mathrm{Ca}(\mathrm{OH})_{2}\) What is the equivalent mass for each of the acids or bases listed above?
In some regions of the southwest United States, the water is very hard. For example, in Las Cruces, New Mexico, the tap water contains about 560$\mu \mathrm{g}$ of dissolved solids per milliliter. Reverse osmosis units are marketed in this area to soften water. A typical unit exerts a pressure of 8.0 atm and can produce 45 \(\mathrm{L}\) water per day. a. Assuming all of the dissolved solids are \(\mathrm{MgCO}_{3}\) and assuming a temperature of \(27^{\circ} \mathrm{C},\) what total volume of water must be processed to produce 45 L pure water? b. Would the same system work for purifying seawater? (Assume seawater is 0.60\(M \mathrm{NaCl.} )\)
In order for sodium chloride to dissolve in water, a small amount of energy must be added during solution formation. This is not energetically favorable. Why is NaCl so soluble in water?
Consider the following solutions: 0.010\(m \mathrm{Na}_{3} \mathrm{PO}_{4}\) in water 0.020 \(m \mathrm{CaBr}_{2}\) in water 0.020 \(m \mathrm{KCl}\) in water 0.020 \(m \mathrm{HF}\) in water \((\mathrm{HF} \text { is a weak acid.) }\) a. Assuming complete dissociation of the soluble salts, which solution(s) would have the same boiling point as 0.040 $\mathrm{m} \mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\( in water? \)\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}$ is a nonelectrolyte. b. Which solution would have the highest vapor pressure at $28^{\circ} \mathrm{C} ?$ c. Which solution would have the largest freezing-point depression?
A typical IV used in hospitals is dextrose 5\(\%\) in water (called D5W). This solution is injected into veins through an IV to replace lost fluids and to provide carbohydrates. Injectable medicines are also delivered to the body using the D5W IV. D5W contains 5.0 g dextrose monohydrate $\left(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6} \cdot \mathrm{H}_{2} \mathrm{O}\right)\( per 100.0 \)\mathrm{mL}$ of solution. Assuming a density of 1.01 \(\mathrm{g} / \mathrm{cm}^{3}\) , calculate the molarity and molality of D5W.
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