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Chapter 13: Problem 23

How do the solubilities of most ionic compounds in water change with temperature?

Short Answer

Expert verified
The solubilities of most ionic compounds in water increase with temperature.

Step by step solution

01

Understanding Solubility

Solubility refers to the maximum amount of a substance (solute), that can dissolve in a particular solvent at a given temperature to form a homogeneous solution.
02

Solubility of Ionic Compounds

Ionic compounds are made up of positive and negative ions held together by electrostatic forces. When these compounds are mixed with water, the water molecules, being polar, surround the ions and pull them away from the compound, causing the compound to dissolve.
03

Effect of Temperature on Solubility

The solubility of most substances typically increases with an increase in temperature. The increased temperature provides more kinetic energy to the water molecules, which makes it easier for them to break apart the ionic bonds and dissolve the compound. Therefore, more of the ionic compound can be dissolved at higher temperatures.

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Most popular questions from this chapter

The molar mass of benzoic acid \(\left(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COOH}\right)\) determined by measuring the freezing-point depression in benzene is twice that expected for the molecular formula, \(\mathrm{C}_{7} \mathrm{H}_{6} \mathrm{O}_{2}\). Explain this apparent anomaly.

The alcohol content of hard liquor is normally given in terms of the "proof," which is defined as twice the percentage by volume of ethanol \(\left(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\right)\) present. Calculate the number of grams of alcohol present in \(1.00 \mathrm{~L}\) of 75 proof gin. The density of ethanol is \(0.798 \mathrm{~g} / \mathrm{mL}\)

Describe the factors that affect the solubility of a solid in a liquid. What does it mean to say that two liquids are miscible?

A mixture of ethanol and 1 -propanol behaves ideally at \(36^{\circ} \mathrm{C}\) and is in equilibrium with its vapor. If the mole fraction of ethanol in the solution is \(0.62,\) calculate its mole fraction in the vapor phase at this temperature. (The vapor pressures of pure ethanol and 1 -propanol at \(36^{\circ} \mathrm{C}\) are \(108 \mathrm{mmHg}\) and 40.0 \(\mathrm{mmHg}\), respectively.)

The solubility of \(\mathrm{KNO}_{3}\) is \(155 \mathrm{~g}\) per \(100 \mathrm{~g}\) of water at \(75^{\circ} \mathrm{C}\) and \(38.0 \mathrm{~g}\) at \(25^{\circ} \mathrm{C}\). What mass (in grams) of \(\mathrm{KNO}_{3}\) will crystallize out of solution if exactly \(100 \mathrm{~g}\) of its saturated solution at \(75^{\circ} \mathrm{C}\) are cooled to \(25^{\circ} \mathrm{C} ?\)
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