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Chapter 13: Problem 40

(a) What is the mass percentage of iodine \(\left(\mathrm{I}_{2}\right)\) in a solution containing \(0.035 \mathrm{~mol} \mathrm{I}_{2}\) in \(125 \mathrm{~g}\) of \(\mathrm{CCl}_{4} ?\) (b) Seawater contains \(0.0079 \mathrm{~g} \mathrm{Sr}^{2+}\) per kilogram of water. What is the concentration of \(\mathrm{Sr}^{2+}\) measured in ppm?

Short Answer

Expert verified
(a) Mass percentage of iodine in the solution: Step 1: Mass of I₂ = \(0.035 \text{ mol} \times 253.8 \frac{\text{g}}{\text{mol}} = 8.883 \text{ g}\) Step 2: Total mass = 8.883 g I₂ + 125 g CCl₄ = 133.883 g Step 3: Mass percentage = \(\frac{8.883 \text{ g}}{133.883 \text{ g}} \times 100\% = 6.64 \% \) (b) Concentration of Sr²⁺ in seawater: Step 1: Mass of water = 1 kg × 1000 \( \frac{\text{g}}{\text{kg}} = 1000 \text{ g}\) Step 2: Concentration in ppm = \(\frac{0.0079 \text{ g Sr}^{2+}}{1000 \text{ g water}} \times 1,000,000 \ \text{ppm} = 7.9 \ \text{ppm}\)

Step by step solution

01

Calculate the mass of I₂

To find the mass of I₂, we will multiply the moles of I₂ given (0.035 mol) by the molar mass of I₂ (253.8 g/mol): Mass of I₂ = moles of I₂ × molar mass of I₂ Mass of I₂ = \(0.035 \text{ mol} \times 253.8 \frac{\text{g}}{\text{mol}}\)
02

Find the total mass of the solution

The total mass of the solution is the sum of the masses of I₂ and CCl₄ Total mass = mass of I₂ + mass of CCl₄
03

Calculate the mass percentage of I₂

Now, we will use the formula to find the mass percentage of I₂: Mass percentage = \(\frac{\text{mass of I₂}}{\text{total mass of solution}} \times 100\% \) (b) Concentration of Sr²⁺ in seawater
04

Convert mass of water to grams

First, we will convert the mass of water from kilograms to grams: Mass of water = 1 kg × 1000 \( \frac{\text{g}}{\text{kg}}\)
05

Calculate concentration in ppm

Now, to find the concentration of Sr²⁺ in ppm, use the formula: Concentration in ppm = \(\frac{\text{mass of Sr}^{2+}}{\text{total mass of water}} \times 1,000,000 \ \text{ppm}\)

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Most popular questions from this chapter

The solubility of \(\mathrm{Cr}\left(\mathrm{NO}_{3}\right)_{3} \cdot 9 \mathrm{H}_{2} \mathrm{O}\) in water is \(208 \mathrm{~g}\) per \(100 \mathrm{~g}\) of water at \(15^{\circ} \mathrm{C}\). A solution of \(\mathrm{Cr}\left(\mathrm{NO}_{3}\right)_{3} \cdot 9 \mathrm{H}_{2} \mathrm{O}\) in water at \(35^{\circ} \mathrm{C}\) is formed by dissolving \(324 \mathrm{~g}\) in \(100 \mathrm{~g}\) water. When this solution is slowly cooled to \(15^{\circ} \mathrm{C},\) no precipitate forms. (a) What term describes this solution? (b) What action might you take to initiate crystallization? Use molecular- level processes to explain how your suggested procedure works.

(a) What is the molality of a solution formed by dissolving \(1.12 \mathrm{~mol}\) of \(\mathrm{KCl}\) in \(16.0 \mathrm{~mol}\) of water? (b) How many grams of sulfur \(\left(\mathrm{S}_{8}\right)\) must be dissolved in \(100.0 \mathrm{~g}\) naphthalene \(\left(\mathrm{C}_{10} \mathrm{H}_{8}\right)\) to make a \(0.12 \mathrm{~m}\) solution?

Calculate the molality of each of the following solutions: (a) \(8.66 \mathrm{~g}\) benzene \(\left(\mathrm{C}_{6} \mathrm{H}_{6}\right)\) dissolved in \(23.6 \mathrm{~g}\) carbon tetrachloride \(\left(\mathrm{CCl}_{4}\right)\) (b) \(4.80 \mathrm{~g} \mathrm{NaCl}\) dissolved in \(0.350 \mathrm{~L}\) of water.

(a) Why is there no colloid in which both the dispersed substance and the dispersing substance are gases? (b) Michael Faraday first prepared ruby-red colloids of gold particles in water that were stable indefinitely. To the unaided eye these brightly colored colloids are not distinguishable from solutions. How could you determine whether a given colored preparation is a solution or colloid?

The osmotic pressure of a \(0.010 \mathrm{M}\) aqueous solution of \(\mathrm{CaCl}_{2}\) is found to be 0.674 atm at \(25^{\circ}\) C. (a) Calculate the van't Hoff factor, \(i\), for the solution. (b) How would you expect the value of \(i\) to change as the solution becomes more concentrated? Explain.
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