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Chapter 13: Problem 35

(a) Calculate the mass percentage of \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) in a solution containing \(10.6 \mathrm{~g} \mathrm{Na}_{2} \mathrm{SO}_{4}\) in \(483 \mathrm{~g}\) water. (b) An ore contains \(2.86 \mathrm{~g}\) of silver per ton of ore. What is the concentration of silver in ppm?

Short Answer

Expert verified
(a) The mass percentage of Na2SO4 in the solution is 2.15 %. (b) The concentration of silver in the ore is 2.86 ppm.

Step by step solution

01

Calculate the total mass of the Na2SO4 solution

The solution contains 10.6 g of Na2SO4 dissolved in 483 g of water. To find the total mass of the solution, we add the masses of the solute (Na2SO4) and the solvent (water). Total mass of the solution = Mass of Na2SO4 + Mass of water Total mass = 10.6 g + 483 g Total mass = 493.6 g
02

Calculate the mass percentage of Na2SO4

Now that we know the total mass of the solution, we can calculate the mass percentage of Na2SO4. The mass percentage is the mass of the solute divided by the total mass of the solution, multiplied by 100. Mass percentage of Na2SO4 = (Mass of Na2SO4 / Total mass of the solution) x 100 Mass percentage = (10.6 g / 493.6 g) x 100 Mass percentage = (0.0215) x 100 Mass percentage = 2.15 % (a) The mass percentage of Na2SO4 in the solution is 2.15 %.
03

Convert the mass of silver per ton of ore to grams

In the second part of the exercise, we are given that there are 2.86 g of silver in one ton of ore. Since we will need to express the concentration of silver in ppm, we should first convert the mass of silver to grams. One ton is equal to 1,000,000 grams. Mass of silver = 2.86 g Mass of ore = 1 ton = 1,000,000 g
04

Calculate the concentration of silver in ppm

Now that we have the mass of silver and the mass of ore in grams, we can easily calculate the concentration of silver in ppm. Silver concentration in ppm = (Mass of silver / Mass of ore) x 1,000,000 Silver concentration in ppm = (2.86 g / 1,000,000 g) x 1,000,000 Silver concentration in ppm = 2.86 ppm (b) The concentration of silver in the ore is 2.86 ppm.

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Most popular questions from this chapter

A saturated solution of sucrose \(\left(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\right)\) is made by dissolving excess table sugar in a flask of water. There are \(50 \mathrm{~g}\) of undissolved sucrose crystals at the bottom of the flask in contact with the saturated solution. The flask is stoppered and set aside. A year later a single large crystal of mass \(50 \mathrm{~g}\) is at the bottom of the flask. Explain how this experiment provides evidence for a dynamic equilibrium between the saturated solution and the undissolved solute.

Indicate the principal type of solute-solvent interaction in each of the following solutions, and rank the solutions from weakest to strongest solute- solvent interaction: (a) KCl in water, (b) \(\mathrm{CH}_{2} \mathrm{Cl}_{2}\) in benzene \(\left(\mathrm{C}_{6} \mathrm{H}_{6}\right)\), (c) methanol \(\left(\mathrm{CH}_{3} \mathrm{OH}\right)\) in water.

A sulfuric acid solution containing \(571.6 \mathrm{~g}\) of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) per Jiter of solution has a density of \(1.329 \mathrm{~g} / \mathrm{cm}^{3}\). Calculate (a) the mass percentage, (b) the mole fraction, (c) the molality, (d) the molarity of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) in this solution.

Describe how you would prepare each of the following aqueous solutions: (a) \(1.50 \mathrm{~L}\) of \(0.110 \mathrm{M}\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}\) solution, starting with solid \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4} ;\) (b) \(120 \mathrm{~g}\) of a solution that is \(0.65 \mathrm{~m}\) in \(\mathrm{Na}_{2} \mathrm{CO}_{3}\), starting with the solid solute; (c) \(1.20 \mathrm{~L}\) of a solution that is \(15.0 \% \mathrm{~Pb}\left(\mathrm{NO}_{3}\right)_{2}\) by mass (the density of the solution is \(1.16 \mathrm{~g} / \mathrm{mL}\) ), starting with solid solute; (d) a \(0.50 \mathrm{M}\) solution of \(\mathrm{HCl}\) that would just neutralize \(5.5 \mathrm{~g}\) of \(\mathrm{Ba}(\mathrm{OH})_{2}\) starting with \(6.0\) M HCl.

Explain how each of the following factors helps determine the stability or instability of a colloidal dispersion: (a) particulate mass, (b) hydrophobic character, (c) charges on colloidal particles.
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