Question

Which of the following statements is(are) true? For the false statements, correct them. a. A concentrated solution in water will always contain a strong or weak electrolyte. b. A strong electrolyte will break up into ions when dissolved in water. c. An acid is a strong electrolyte. d. All ionic compounds are strong electrolytes in water

Short answer

a. True b. True c. False; corrected statement: An acid can be either a strong or a weak electrolyte. d. False; corrected statement: Some ionic compounds are strong electrolytes in water, while others can be weak electrolytes or have limited solubility.

Step-by-step solution

Statement a: A concentrated solution in water will always contain a strong or weak electrolyte.

This statement is true. A concentrated solution in water implies a high concentration of solute molecules, which can be strong or weak electrolytes. Strong electrolytes ionize completely in water, while weak electrolytes only partially ionize.

Statement b: A strong electrolyte will break up into ions when dissolved in water.

This statement is true. A strong electrolyte is a compound that dissociates completely into its constituent ions when it is dissolved in water. This results in a solution containing a high concentration of mobile ions, which can effectively carry an electric current.

Statement c: An acid is a strong electrolyte.

This statement is false. Some acids, such as hydrochloric acid (HCl) and sulfuric acid (H2SO4), are strong electrolytes because they dissociate completely into ions. However, not all acids are strong electrolytes. For example, acetic acid (CH3COOH) and other weak acids only partially dissociate, meaning they are weak electrolytes. The corrected statement should be: An acid can be either a strong or a weak electrolyte.

Statement d: All ionic compounds are strong electrolytes in water.

This statement is false. While many ionic compounds are strong electrolytes, some ionic compounds can have limited solubility in water or dissociate only partially, thus behaving as weak electrolytes. The corrected statement should be: Some ionic compounds are strong electrolytes in water, while others can be weak electrolytes or have limited solubility.

Key concepts

Strong Electrolytes

Strong electrolytes are substances that completely dissociate into ions in water, allowing them to conduct electricity very well. When you dissolve a strong electrolyte in water, every single molecule breaks apart to form charged particles. This complete breakdown makes the solution highly conductive.

• Examples of strong electrolytes include salts like sodium chloride (NaCl) and acids such as hydrochloric acid (HCl).

Strong electrolytes are essential in many chemical processes where electrical conductivity is required. Understanding the nature of strong electrolytes helps in predicting the behavior of chemical reactions in aqueous solutions.

Weak Electrolytes

Unlike strong electrolytes, weak electrolytes only partially dissociate into ions in water, resulting in a solution that conducts electricity poorly. In a solution with a weak electrolyte, not all of the material is converted into ions. This means that there are fewer charged particles in the solution, which reduces its ability to conduct electricity compared to strong electrolytes.

• An example of a weak electrolyte is acetic acid (CH\(_3\)COOH), a component of vinegar.

Recognizing weak electrolytes is crucial for understanding the dynamics of equilibrium in chemical solutions, especially involving weak acids and bases.

Ionic Compounds

Ionic compounds are composed of positive and negative ions held together by strong electrostatic forces known as ionic bonds. When they dissolve in water, they break into their respective ions, making them electrolytes. However, not all ionic compounds are strong electrolytes. Their solubility varies, and some may not dissolve completely, behaving like weak electrolytes in solution.

• For instance, while sodium chloride (NaCl) is a strong electrolyte, calcium sulfate (CaSO\(_4\)) has low solubility and therefore can act as a weak electrolyte.

Understanding the nature of ionic compounds and their behavior in water is fundamental in various applications, from designing chemical reactions to analyzing complex biological systems.