Answer In 60 Words Or More: Explain Why Some Substances Are

Answer In 60 Words Or Moreexplain Why Some Substances Are Soluble In

Some substances are soluble in water because of the principle "like dissolves like," meaning polar substances dissolve best in polar solvents, and nonpolar substances dissolve in nonpolar solvents. Water, being polar, dissolves ionic compounds like salt (NaCl) and polar molecules like sugar but not nonpolar molecules such as oil. Solubility depends on intermolecular forces and polarity.

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Solubility is fundamentally driven by the nature of intermolecular interactions between solute and solvent. Water's polarity allows it to effectively surround and interact with ionic compounds and polar molecules, leading to their dissolution. Conversely, nonpolar substances such as oils or fats lack the necessary polarity to interact favorably with water, resulting in low solubility. For example, table salt (NaCl) dissolves readily in water because of ionic interactions, whereas substances like wax are insoluble due to their nonpolar characteristics.\n

The concept "like dissolves like" emphasizes that solvents and solutes with similar polarity tend to be compatible. Polar solutes like ethanol or sugar dissolve well in water, a polar solvent, while nonpolar solvents like hexane dissolve nonpolar substances such as greasy oils. This principle extends beyond water, where solvents like benzene or toluene efficiently dissolve nonpolar compounds, illustrating the importance of intermolecular forces in solubility behavior.

Electrolytes are substances that produce ions when dissolved in water, enabling the solution to conduct electricity. Strong electrolytes, such as sodium chloride (NaCl) or potassium iodide (KI), dissociate completely into their ions, resulting in high electrical conductivity. Weak electrolytes, like acetic acid or ammonia, dissociate partially, leading to lower conductivity. The degree of ionization directly influences the strength of conduction.

The solubility of electrolytes relates to their ionization ability in water. For instance, NaCl dissolves readily and dissociates completely, making it a strong electrolyte and a good conductor. In contrast, calcium carbonate (CaCO₃) is poorly soluble and behaves as a weak electrolyte, providing limited ions in solution. Factors like temperature, ionic charge, and lattice energy influence solubility and electrolyte strength. Understanding these principles aids in applications like battery design, water treatment, and drug delivery systems.

References

• Atkins, P., & de Paula, J. (2014). Physical Chemistry (10th ed.). Oxford University Press.
• Chang, R., & Goldsby, K. (2016). Chemistry (12th ed.). McGraw-Hill Education.
• Laidler, K. J. (1993). Chemical Kinetics. Harper & Row.
• Petrucci, R. H., Herring, F. G., Madura, J. D., & Bissonnette, C. (2017). General Chemistry: Principles & Modern Applications. Pearson.
• Moore, J. W., & Stanitski, C. L. (2017). Chemistry: The Molecular Nature of Matter and Change. Cengage Learning.
• Chang, R. (2018). Chemistry. McGraw-Hill Education.
• Organ, M. (2010). Principles of Chemistry. Oxford University Press.
• Harris, D. C. (2015). Quantitative Chemical Analysis. W. H. Freeman and Company.
• McMurry, J. (2013). Organic Chemistry. Brooks Cole.
• Zumdahl, S. S., & Zumdahl, S. A. (2017). Chemistry. Cengage Learning.