Open Question
The Henry’s law constant for helium gas in water at 30 °C is 3.7 * 10^-4 M/atm and the constant for N2 at 30 °C is 6.0 * 10^-4 M/atm. If the two gases are each present at 1.5 atm pressure, calculate the solubility of each gas.
Ch.13 - Properties of Solutions
Chapter 13, Problem 39b
(b) An ore contains 2.86 g of silver per ton of ore. What is the concentration of silver in ppm?
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Parts Per Million (ppm)
Parts per million (ppm) is a unit of measurement used to express very dilute concentrations of substances. It indicates how many parts of a substance are present in one million parts of a solution or mixture. For example, 1 ppm means 1 part of solute in 1,000,000 parts of solution, making it a useful measure for trace elements in ores or environmental samples.
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Guided course
01:38
Parts per Million (ppm)
Conversion of Mass to ppm
To convert a mass concentration to ppm, the mass of the substance is divided by the total mass of the solution or mixture, then multiplied by 1,000,000. In this case, since the ore contains silver, the total mass is considered in terms of grams per ton, where 1 ton equals 1,000,000 grams, facilitating the conversion to ppm.
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04:12Energy to Mass Conversion
Understanding Ore Composition
Ore composition refers to the specific elements and their concentrations found within a mineral deposit. In this context, knowing the amount of silver in the ore allows for calculations of its economic viability and extraction potential. Understanding the composition is crucial for mining and metallurgy, as it influences processing methods and costs.
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04:19Matter Composition
Related Practice
Open Question
The partial pressure of O2 in air at sea level is 0.21 atm. Using the data in Table 13.1, together with Henry’s law, calculate the molar concentration of O2 in the surface water of a mountain lake saturated with air at 20 °C and an atmospheric pressure of 650 torr.
Textbook Question
(a) Calculate the mass percentage of Na2SO4 in a solution containing 10.6 g of Na2SO4 in 483 g of water.
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Open Question
A solution is made containing 14.6 g of CH3OH in 184 g of H2O. Calculate (a) the mole fraction of CH3OH.
Textbook Question
A solution is made containing 20.8 g of phenol (C6H5OH) in 425 g of ethanol (CH3CH2OH). Calculate (a) the mole fraction of phenol,
Textbook Question
A solution is made containing 20.8 g of phenol (C6H5OH) in 425 g of ethanol (CH3CH2OH). Calculate (c) the molality of phenol.
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