Textbook Question
A solution contains 32 g of KNO3 per 100.0 g of water at 25 °C. Is the solution unsaturated, saturated, or supersaturated? (Use Figure 13.11.)
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Ch.13 - Solutions
Chapter 13, Problem 45
Why do some laboratory procedures involving oxygen-sensitive reactants or products call for using water that has been boiled and then cooled?
Verified step by step guidance1
Understand that oxygen-sensitive reactants or products can react with dissolved oxygen in water, which can affect the outcome of the experiment.
Recognize that boiling water helps to remove dissolved gases, including oxygen, by driving them out of the solution due to the increased temperature and decreased solubility of gases.
After boiling, allow the water to cool in a closed container to prevent reabsorption of oxygen from the air as it cools down.
Use the cooled, deoxygenated water in the laboratory procedure to minimize the risk of unwanted reactions with oxygen-sensitive substances.
Consider the importance of using deoxygenated water in experiments where the presence of oxygen could lead to oxidation or other side reactions that could interfere with the results.
Related Practice
Textbook Question
A KNO3 solution containing 45 g of KNO3 per 100.0 g of water is cooled from 40 °C to 0 °C. What happens during cooling? (Use Figure 13.11.)
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Textbook Question
A KCl solution containing 42 g of KCl per 100.0 g of water is
cooled from 60 °C to 0 °C. What happens during cooling? (Use
Figure 13.11.)
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Open Question
Why do fish die when placed in a tank filled with water that has been boiled and then cooled?
Open Question
Scuba divers breathing air at increased pressure can suffer from nitrogen narcosis—a condition resembling drunkenness—when the partial pressure of nitrogen exceeds about 4 atm. What property of gas-water solutions causes this to happen? How can a diver reverse this effect?
Textbook Question
Scuba divers breathing air at increased pressure can suffer from oxygen toxicity—too much oxygen in their bloodstream— when the partial pressure of oxygen exceeds about 1.4 atm. What happens to the amount of oxygen in a diver's bloodstream when he or she breathes oxygen at elevated pressures? How can this be reversed?
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