How does the polarity of water contribute to its ability to dissolve so many substances?

• A. Water's polarity allows it to form covalent bonds with many substances.
• B. Natural water has a pH of approximately 5.6, which is slightly acidic. Acids can dissolve more substances than bases can.
• C. Because it is polar, water forms ionic bonds with the ions in substances such as NaCl (salt).
• D. Because it is polar, water's negatively charged oxygen atoms and positively charged hydrogen atoms are attracted to positively and negatively charged ions and molecules.

Answer: (D)

Verified step by step guidance

1. Understand the concept of polarity: Water is a polar molecule, meaning it has a partial positive charge on one side (hydrogen atoms) and a partial negative charge on the other side (oxygen atom). This is due to the difference in electronegativity between hydrogen and oxygen.
2. Recognize how polarity affects interactions: The polarity of water allows it to interact with other charged particles. The positive side of water molecules (hydrogen) is attracted to negatively charged ions or molecules, while the negative side (oxygen) is attracted to positively charged ions or molecules.
3. Explore the process of dissolution: When a substance like NaCl (salt) is added to water, the polar water molecules surround the individual Na⁺ and Cl⁻ ions. The negative oxygen ends of water molecules are attracted to Na⁺ ions, and the positive hydrogen ends are attracted to Cl⁻ ions.
4. Consider the role of hydrogen bonding: Water's ability to dissolve substances is also enhanced by hydrogen bonding, where the hydrogen atoms of one water molecule are attracted to the oxygen atoms of another, creating a network that can surround and separate solute particles.
5. Summarize the effect of water's polarity: The combination of water's polarity and its ability to form hydrogen bonds makes it an excellent solvent, capable of dissolving a wide range of ionic and polar substances by surrounding and interacting with their charged components.