ration of each of Part A sodium bromide, NaBr(s), a strong electrolyte Express your answer as a chemical equation including phases. = AE ? NaBr(s) +H, O(1)+Na+ (aq) + Br- (aq) You have already submitted this answer. Enter a new answer No credit lost. Try again Submit Previous Answers Request Answer Part B lactic acid, HC,H,O,(s), a woak electrolyte Express your answer as a chemical equation including phases. Submit Request Answer – Part dextrose(D-glucose), C6H1206(s), a nonelectrolyte Express your answer as a chemical equation including phases. Submit Request Answer Provide Feedback
The Correct Answer and Explanation is:
Here are the correct chemical equations for the dissolution of each compound, followed by a detailed explanation.
Part A: Sodium bromide (NaBr), a strong electrolyte
Chemical Equation: NaBr(s)→Na+(aq)+Br−(aq)\text{NaBr(s)} \rightarrow \text{Na}^+(aq) + \text{Br}^-(aq)
Explanation:
Sodium bromide is an ionic compound composed of sodium ions (Na⁺) and bromide ions (Br⁻). It is classified as a strong electrolyte, which means it completely dissociates into its ions when dissolved in water. The process of dissociation doesn’t involve a reversible reaction; all the NaBr units separate into free-moving ions in the aqueous solution. This is why NaBr is good at conducting electricity in solution—it provides a high concentration of ions. The water (H₂O) isn’t explicitly included in the reaction equation as a reactant because it’s the medium, not a reactant, but it facilitates the dissociation.
Part B: Lactic acid (HC₃H₅O₃), a weak electrolyte
Chemical Equation: HC3H5O3(s)⇌H+(aq)+C3H5O3−(aq)\text{HC}_3\text{H}_5\text{O}_3(s) \rightleftharpoons \text{H}^+(aq) + \text{C}_3\text{H}_5\text{O}_3^-(aq)
Explanation:
Lactic acid is a weak electrolyte, meaning it only partially ionizes in aqueous solution. The equation shows a reversible reaction using a double arrow (⇌), indicating that an equilibrium is established between the undissociated lactic acid and its ions. Only a small fraction of lactic acid molecules donate protons (H⁺) to form lactate ions (C₃H₅O₃⁻), so the concentration of free ions in solution is relatively low. This incomplete ionization is why weak electrolytes conduct electricity poorly compared to strong electrolytes.
Part C: Dextrose (D-glucose, C₆H₁₂O₆), a nonelectrolyte
Chemical Equation: C6H12O6(s)→C6H12O6(aq)\text{C}_6\text{H}_{12}\text{O}_6(s) \rightarrow \text{C}_6\text{H}_{12}\text{O}_6(aq)
Explanation:
Dextrose (or glucose) is a nonelectrolyte, which means it dissolves in water without ionizing. The solid sugar simply dissolves as intact, neutral molecules, so it does not produce ions in solution. As a result, glucose solutions do not conduct electricity. In the chemical equation, the phase changes from solid (s) to aqueous (aq), indicating it has dissolved, but no chemical reaction has occurred—only a physical process. The molecules remain unchanged, and water simply acts as a solvent.
Summary Table
| Substance | Type of Electrolyte | Chemical Equation |
|---|---|---|
| NaBr | Strong electrolyte | NaBr(s) → Na⁺(aq) + Br⁻(aq) |
| HC₃H₅O₃ | Weak electrolyte | HC₃H₅O₃(s) ⇌ H⁺(aq) + C₃H₅O₃⁻(aq) |
| C₆H₁₂O₆ | Nonelectrolyte | C₆H₁₂O₆(s) → C₆H₁₂O₆(aq) |
These equations demonstrate how the nature of the solute (ionic, molecular, strong/weak acid/base) determines the type of dissolution or ionization process in water.
