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Chapter 13: Problem 39

(a) Calculate the mass percentage of \(\mathrm{NaNO}_{3}\) in a solution containing \(13.6 \mathrm{~g}\) of \(\mathrm{NaNO}_{3}\) in \(834 \mathrm{~g}\) of water. (b) An alloy contains \(2.86 \mathrm{~g}\) of chromium per $100 \mathrm{~kg}$ of alloy. What is the concentration of chromium in ppm?

Short Answer

Expert verified
The mass percentage of NaNO3 in the solution is 1.605%, and the concentration of chromium in the alloy is 28.6 ppm.

Step by step solution

01

Part (a) - Mass Percentage of NaNO3 in Solution

To calculate the mass percentage of NaNO3 in the solution, follow these steps: 1. Determine the mass of NaNO3: 13.6 g 2. Determine the mass of water: 834 g 3. Calculate the total mass of the solution: NaNO3 mass + water mass 4. Divide the mass of NaNO3 by the total mass of the solution. 5. Multiply the result by 100 to express it as a percentage. Let's calculate the mass percentage now: In this case, the mass of NaNO3 is 13.6 g, and the mass of water is 834 g. Total mass of the solution = 13.6 g (NaNO3) + 834 g (water) = 847.6 g Mass percentage of NaNO3 = \(\frac{13.6 \mathrm{~g}}{847.6 \mathrm{~g}}\) × 100
02

Part (a) - Calculate Mass Percentage

Now, calculate the mass percentage: Mass percentage of NaNO3 = \(\frac{13.6}{847.6}\) × 100 = 1.605 % Hence, the mass percentage of NaNO3 in the solution is 1.605%.
03

Part (b) - Chromium Concentration in Alloy

To calculate the concentration of chromium in the alloy in ppm, follow these steps: 1. Determine the mass of chromium: 2.86 g 2. Determine the mass of the alloy: 100 kg (convert to g) 3. Calculate the concentration of chromium in ppm. Let's calculate the concentration of chromium in ppm: In this case, the mass of chromium is 2.86 g and the mass of the alloy is 100 kg. Let's first convert the mass of alloy to g: Mass of the alloy = 100 kg × \(10^3 \mathrm{~g/kg}\) = 100,000 g Chromium concentration in ppm = \(\frac{2.86 \mathrm{~g}}{100,000 \mathrm{~g}}\) × \(10^6\)
04

Part (b) - Calculate Chromium Concentration

Now, calculate the chromium concentration in ppm: Chromium concentration in ppm = \(\frac{2.86}{100,000}\) × \(10^6\) = 28.6 ppm Hence, the concentration of chromium in the alloy is 28.6 ppm.

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Most popular questions from this chapter

Brass is a substitutional alloy consisting of a solution of copper and zinc. A particular sample of yellow brass consisting of \(65.0 \%\) Cu and \(35.0 \%\) Zn by mass has a density of \(8470 \mathrm{~kg} / \mathrm{m}^{3}\). (a) What is the molality of \(\mathrm{Zn}\) in the solid solution? (b) What is the molarity of \(Z n\) in the solution?

The normal boiling point of ethanol, $\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH},\( is \)78.4^{\circ} \mathrm{C}\(. When \)3.26 \mathrm{~g}$ of a soluble nonelectrolyte is dissolved in \(100.0 \mathrm{~g}\) of ethanol at that temperature, the vapor pressure of the solution is \(100 \mathrm{kPa}\). What is the molar mass of the solute?

A "canned heat" product used to warm buffet dishes consists of a homogeneous mixture of ethanol \(\left(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\right)\) and paraffin, which has an average formula of $\mathrm{C}_{24} \mathrm{H}_{50}\(. What mass of \)\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}$ should be added to \(620 \mathrm{~kg}\) of the paraffin to produce $1.07 \mathrm{kPa}\( of ethanol vapor pressure at \)35^{\circ} \mathrm{C}$ ? The vapor pressure of pure ethanol at \(35^{\circ} \mathrm{C}\) is \(13.3 \mathrm{kPa}\).

The density of acetonitrile \(\left(\mathrm{CH}_{3} \mathrm{CN}\right)\) is \(0.786 \mathrm{~g} / \mathrm{mL}\) and the density of methanol \(\left(\mathrm{CH}_{3} \mathrm{OH}\right)\) is $0.791 \mathrm{~g} / \mathrm{mL}\(. A solution is made by dissolving \)25.0 \mathrm{~mL}$ of \(\mathrm{CH}_{3} \mathrm{OH}\) in \(100 \mathrm{~mL}\) of $\mathrm{CH}_{3} \mathrm{CN}$ (a) What is the mole fraction of methanol in the solution? (b) What is the molality of the solution? (c) Assuming that the volumes are additive, what is the molarity of \(\mathrm{CH}_{3} \mathrm{OH}\) in the solution?

Which of the following in each pair is likely to be more soluble in water: (a) cyclohexane \(\left(\mathrm{C}_{6} \mathrm{H}_{12}\right)\) or glucose \(\left(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\right)\), (b) propionic acid \(\left(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{COOH}\right)\) or sodium propionate $\left(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{COONa}\right),(\mathbf{c}) \mathrm{HCl}$ or ethyl chloride \(\left(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{Cl}\right) ?\) Explain in each case.
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