Is the ionic compound CaCO3 soluble or insoluble, and does each of its ions tend to be soluble?
a. Both ions soluble b. Both ions insoluble c. Ions differ; soluble d. Ions differ; insoluble
Is the ionic compound NaNO3 soluble or insoluble, and does each of its ions tend to be soluble?
a. Both ions soluble b. Both ions insoluble c. Ions differ; soluble d. Ions differ; insoluble
Is the ionic compound AgBr soluble or insoluble, and does each of its ions tend to be soluble?
a. Both ions soluble b. Both ions insoluble c. Ions differ; soluble d. Ions differ; insoluble
Is the ionic compound (NH4)3PO4 soluble or insoluble, and does each of its ions tend to be soluble?
a. Both ions soluble b. Both ions insoluble c. Ions differ; soluble d. Ions differ; insoluble
Classify the solution properties of 1.0 M acetic acid.
a. Strong electrolyte b. Weak electrolyte c. Non-electrolyte d. Pure liquid
The Correct Answer and Explanation is :
1. Is the ionic compound CaCO₃ soluble or insoluble, and does each of its ions tend to be soluble?
Answer: d. Ions differ; insoluble
Explanation: Calcium carbonate (CaCO₃) is largely insoluble in water. The solubility of ionic compounds depends on the ability of their ions to dissociate in water. While calcium (Ca²⁺) ions are generally soluble in water (as seen in compounds like CaCl₂), carbonate (CO₃²⁻) ions tend to form insoluble salts with many cations, particularly calcium. Therefore, CaCO₃ is insoluble, but the ions individually (Ca²⁺ and CO₃²⁻) would typically be soluble if isolated in other compounds.
2. Is the ionic compound NaNO₃ soluble or insoluble, and does each of its ions tend to be soluble?
Answer: a. Both ions soluble
Explanation: Sodium nitrate (NaNO₃) is soluble in water. Sodium ions (Na⁺) and nitrate ions (NO₃⁻) both tend to be soluble in water. Sodium salts are generally soluble due to their low lattice energies, and nitrates are generally soluble in water, with very few exceptions. Therefore, NaNO₃ dissolves completely, with both Na⁺ and NO₃⁻ ions being soluble.
3. Is the ionic compound AgBr soluble or insoluble, and does each of its ions tend to be soluble?
Answer: c. Ions differ; soluble
Explanation: Silver bromide (AgBr) is insoluble in water. However, silver (Ag⁺) is generally soluble in many compounds, and bromide (Br⁻) is soluble in most salts except those formed with heavy metals like Ag⁺, Pb²⁺, and Hg₂²⁺. While Ag⁺ and Br⁻ tend to be soluble separately, their combination forms an insoluble salt (AgBr), due to the relatively low solubility product (Ksp) of AgBr.
4. Is the ionic compound (NH₄)₃PO₄ soluble or insoluble, and does each of its ions tend to be soluble?
Answer: a. Both ions soluble
Explanation: Ammonium phosphate ((NH₄)₃PO₄) is soluble in water. Ammonium (NH₄⁺) salts are typically soluble because ammonium is a weak acid and dissolves easily in water. Phosphate (PO₄³⁻), despite its tendency to form insoluble salts with many other cations (like calcium), remains soluble in combination with ammonium. Therefore, both ions in (NH₄)₃PO₄ are soluble.
5. Classify the solution properties of 1.0 M acetic acid.
Answer: b. Weak electrolyte
Explanation: Acetic acid (CH₃COOH) is a weak electrolyte. This means that it does not completely dissociate into ions when dissolved in water. Acetic acid only partially ionizes in water to form hydrogen ions (H⁺) and acetate ions (CH₃COO⁻), unlike strong electrolytes like hydrochloric acid (HCl), which dissociates completely. As a result, acetic acid is considered a weak electrolyte because it only partially conducts electricity due to its limited ionization in solution.