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Chapter 12: Problem 42

Which pairs of liquids will be soluble in each other? (a) \(\mathrm{H}_{2} \mathrm{O}\) and \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{3}\) (b) \(\mathrm{C}_{6} \mathrm{H}_{6}\) (benzene) and \(\mathrm{CCl}_{4}\) (c) \(\mathrm{H}_{2} \mathrm{O}\) and \(\mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{H}\)

Short Answer

Expert verified
Pairs (b) and (c) are soluble: (b) \(\mathrm{C}_{6} \mathrm{H}_{6}\) and \(\mathrm{CCl}_{4}\); (c) \(\mathrm{H}_{2} \mathrm{O}\) and \(\mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{H}\).

Step by step solution

01

Identify the polarity of each liquid

Determine whether each molecule is polar or non-polar. Polar molecules have an unequal distribution of electrons, while non-polar molecules have an equal distribution of electrons.
02

Analyze Solubility for Pair (a) \\(\mathrm{H}_{2} \mathrm{O}\\) and \\(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{3}\\)

Water \(\mathrm{H}_2\mathrm{O}\) is a polar molecule due to its bent shape and difference in electronegativity between hydrogen and oxygen. Butane (\(\mathrm{CH}_3\mathrm{CH}_2\mathrm{CH}_2\mathrm{CH}_3\)) is non-polar due to its symmetrical structure. Polar and non-polar liquids generally do not mix well because of the lack of interaction between different types of forces. Thus, these two will not be soluble in each other.
03

Analyze Solubility for Pair (b) \\(\mathrm{C}_{6} \mathrm{H}_{6}\\) and \\(\mathrm{CCl}_{4}\\)

Benzene (\(\mathrm{C}_6\mathrm{H}_6\)) and carbon tetrachloride (\(\mathrm{CCl}_4\)) are both non-polar molecules. Non-polar molecules generally mix well with one another because Van der Waals forces can act between them. Thus, these two liquids are soluble in each other.
04

Analyze Solubility for Pair (c) \\(\mathrm{H}_{2} \mathrm{O}\\) and \\(\mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{H}\\)

Water (\(\mathrm{H}_2\mathrm{O}\)) is polar, and acetic acid (\(\mathrm{CH}_3\mathrm{CO}_2\mathrm{H}\)) is also polar due to the presence of the hydroxyl group and the electronegative oxygen atoms. Polar-polar interactions facilitate solubility; thus, water and acetic acid are soluble in each other.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Molecular Polarity
Molecular polarity is a critical concept in understanding why certain substances mix while others don't. A molecule's polarity is determined by the difference in electronegativity between its atoms and the resulting arrangement of these atoms. In simple terms:
  • Polar molecules have an uneven distribution of charge due to differences in electronegativity.
  • Non-polar molecules have a more even charge distribution, often due to symmetry in their molecular structure.
Polarity affects molecular interactions. Polar molecules tend to have positive and negative ends (like tiny magnets) that allow them to interact with other polar substances. To determine if a molecule is polar, look at its geometric shape and the electronegativity of its atoms. A bent shape like in water (H鈧侽) usually indicates polarity, whereas a symmetrical shape typically indicates that the molecule is non-polar.
Polar and Non-Polar Interactions
The interactions between polar and non-polar molecules form the basis of solubility behavior. Polar molecules, due to their electrical charge separation, can engage in hydrogen bonding and dipole-dipole interactions. These strong interactions facilitate solubility between polar substances. For example:
  • Water ( H鈧侽 ) is polar, which allows it to mix well with other polar substances like acetic acid.
  • Non-polar molecules like butane ( C鈧凥鈧佲個 ) generally interact through weaker Van der Waals forces.
When mixing polar and non-polar substances, the mismatch in interactions generally means they do not mix well. This is why water and butane do not dissolve in each other. Mixing tends to occur more readily when similar interaction types align, such as polar-polar or non-polar-non-polar.
Solubility Rules
Solubility can often be predicted using simple rules based on molecular interactions:
  • "Like dissolves like": Typically, polar solvents dissolve polar solutes, and non-polar solvents dissolve non-polar solutes.
  • Solubility is enhanced when the intermolecular forces of the solute and solvent are similar in strength and type.
Applying these rules helps to understand experimental observations. For instance: - Water and acetic acid, both polar, dissolve in each other due to compatible hydrogen bonding. - Benzene and carbon tetrachloride, both non-polar, are soluble due to Van der Waals forces. Using these rules simplifies predicting solubility outcomes without needing complex calculations.
Chemical Structure Analysis
Assessing the chemical structure of a substance provides insights into its molecular properties and interactions. By examining a molecule's structure, one can predict its polarity and potential solubility:
  • Check for symmetry: Symmetrical molecules like carbon tetrachloride ( CCl鈧� ) are often non-polar.
  • Look for polar functional groups (e.g., -OH, NH鈧�): Presence of such groups can make a molecule polar, as seen in acetic acid ( CH鈧僀O鈧侶 ).
This analysis allows us to classify substances and predict their interactions. Understanding how the structure correlates with properties aids in predicting behaviors like solubility. For students, practicing chemical structure analysis can lead to better predictions of how molecules will behave in different environments.

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Most popular questions from this chapter

In the 1986 Lake Nyos disaster (see the chapter introduction), an estimated 90 billion kilograms of \(\mathrm{CO}_{2}\) was dissolved in the lake at the time. (a) What volume of gas is this at standard temperature and pressure? (b) A Assuming that this dissolved gas was in equilibrium with the normal partial pressure of \(\mathrm{CO}_{2}\) in the atmosphere \((0.038 \%\), or 0.29 torr \()\), use the Henry's law constant for \(\mathrm{CO}_{2}\) in water to estimate the volume of Lake Nyos.

A \(2.00 \%\) solution of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) in water freezes at \(-0.796^{\circ} \mathrm{C}\) (a) Calculate the van't Hoff factor, \(i\) (b) Which of the following best represents sulfuric acid in a dilute aqueous solution: \(\mathrm{H}_{2} \mathrm{SO}_{4}, \mathrm{H}^{+}+\mathrm{HSO}_{4}^{-}\), or \(2 \mathrm{H}^{+}+\mathrm{SO}_{4}^{2-} ?\)

Choose the solute of each pair that would be more soluble in water. Explain your answer. (a) \(\mathrm{NaOH}\) or \(\mathrm{CO}_{2}\) (b) \(\mathrm{TiCl}_{3}\) or \(\mathrm{CHCl}_{3}\) (c) \(\mathrm{C}_{3} \mathrm{H}_{8}\) or \(\mathrm{C}_{3} \mathrm{H}_{7} \mathrm{OH}\)

List and define the colligative properties, and give the units used for concentrations for each.

A 0.010 -molar solution of calcium chloride is separated from pure water by a semipermeable membrane at \(298 \mathrm{~K}\). In which direction does net transport of water occur across the membrane when the applied pressure on the solution is 500 torr? (Assume an ideal value for the van't Hoff factor. Calcium chloride is also used as a de-icer in wintry climates.)
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