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Chapter 13: Problem 9

A saturated aqueous solution of \(\mathrm{NaBr}\) at \(20^{\circ} \mathrm{C}\) contains \(116 \mathrm{g} \mathrm{NaBr} / 100 \mathrm{g} \mathrm{H}_{2} \mathrm{O}\). Express this composition in the more conventional percent by mass, that is, as grams of NaBr per 100 grams of solution.

Short Answer

Expert verified
The composition of saturated aqueous solution of NaBr at 20°C is 53.70 % by mass, which means there are 53.70 grams of NaBr in every 100 grams of the total solution.

Step by step solution

01

Calculate total mass of the solution

According to the problem, we have 116 g of NaBr (solute) in every 100 g of water (solvent). To find out total mass of solution, we should add the mass of the solute to the mass of the solvent: 116 g (NaBr) + 100 g (H2O) = 216 g
02

Calculate percent by mass

Now, expressing the composition as grams of solute per 100 grams of solution (percent by mass), we find the percentage that the solute represents of the total. This can be found by using the formula: \[ ( \frac{mass \ of \ the \ solute}{mass \ of \ the \ solution} ) \times 100 \] Substituting in the values which we have: \( \frac{116 \ g}{216 \ g} \) x 100 = 53.70 %

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Most popular questions from this chapter

An aqueous solution is \(34.0 \% \mathrm{H}_{3} \mathrm{PO}_{4}\) by mass and has a density of \(1.209 \mathrm{g} / \mathrm{mL}\). What are the molarity and molality of this solution?

In a saturated solution at \(25^{\circ} \mathrm{C}\) and 1 bar, for the following solutes, which condition will increase solubility? (a) \(\operatorname{Ar}(g),\) decrease temperature; (b) \(\mathrm{NaCl}(\mathrm{s})\) increase pressure; (c) \(\mathrm{N}_{2}\), decrease pressure; (d) \(\mathrm{CO}_{2}\) increase volume.

The aqueous solubility of \(\mathrm{CO}_{2}\) at \(20^{\circ} \mathrm{C}\) and 1.00 atm is equivalent to \(87.8 \mathrm{mL} \mathrm{CO}_{2}(\mathrm{g}),\) measured at STP, per \(100 \mathrm{mL}\) of water. What is the molarity of \(\mathrm{CO}_{2}\) in water that is at \(20^{\circ} \mathrm{C}\) and saturated with air at 1.00 atm? The volume percent of \(\mathrm{CO}_{2}\) in air is \(0.0360 \% .\) Assume that the volume of the water does not change when it becomes saturated with air.

When the stems of cut flowers are held in concentrated \(\mathrm{NaCl}(\mathrm{aq}),\) the flowers wilt. In a similar solution a fresh cucumber shrivels up (becomes pickled). Explain the basis of these phenomena.

Calculate the mole fraction of the solute in the following aqueous solutions:(a) \(0.112 \mathrm{M} \mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\) \((d=1.006 \mathrm{g} / \mathrm{mL})\) (b) \(3.20 \%\) ethanol,by volume \((d=0.993 \mathrm{g} / \mathrm{mL}\) pure \(\left.\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}, d=0.789 \mathrm{g} / \mathrm{mL}\right)\).
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