Final answer:
Solubility in water is determined by the substance's chemical and physical properties, intermolecular forces, and the principle that 'like dissolves like'. This can have significant implications in fields like medicine and environmental science.
Step-by-step explanation:
The solubility of a compound in water is greatly influenced by the compound's chemical and physical properties, such as molecular structure, polarity, and intermolecular forces. In general, substances that exhibit hydrogen bonding or dipole-dipole forces have greater water solubility than those with only London dispersion forces. Ionic compounds, due to their charged nature, are often quite soluble in polar solvents like water. The temperature and pressure can also affect the solubility of gases, with gas solubility typically increasing with increased pressure and decreasing with increased temperature.
Regarding solubility trends, the principle "like dissolves like" is often useful. This means that polar solutes are more likely to dissolve in polar solvents, while nonpolar solutes favor nonpolar solvents. For example, NaCl, a polar ionic compound, is highly soluble in water but not in nonpolar oil. Conversely, nonpolar wax dissolves in nonpolar hexane but not in polar water.
Selecting the more soluble member in a pair of compounds can have significant practical implications. For instance, in medical applications, the solubility of a drug in bodily fluids affects its bioavailability. In environmental chemistry, the solubility of pollutants in water can influence their distribution and impact on ecosystems. Understanding these factors is essential for effective application and management of chemical substances.