Question

You are given a water-soluble compound \(\mathrm{X}\). Describe how you would determine whether it is an electrolyte or a non electrolyte. If it is an electrolyte, how would you determine whether it is strong or weak?

Short answer

Dissolve the compound in water and test for conductivity. If it conducts, it's an electrolyte; strong if conductivity is high, weak if low.

Step-by-step solution

Dissolve the Compound

Take a small quantity of the compound X and dissolve it in water to form an aqueous solution. This is essential to test its conductive properties.

Test Electrical Conductivity

Insert electrodes into the aqueous solution of compound X and connect them to a conductivity meter or a simple circuit with a light bulb. Observe whether the light bulb lights up or if the meter shows a reading, indicating the presence of electrical conductivity.

Determine Electrolyte or Nonelectrolyte

If the solution conducts electricity (bulb lights up or meter shows a reading), compound X is an electrolyte, as it allows the flow of ions. If no conductivity is observed, compound X is a nonelectrolyte, indicating it does not ionize in solution.

Test Conductivity Intensity for Electrolyte

If compound X is determined to be an electrolyte, observe the intensity of the bulb light or the magnitude of the conductivity reading. A strong light or high reading indicates a strong electrolyte, while a dim light or low reading suggests a weak electrolyte.

Confirm Strong or Weak Electrolyte

For further confirmation, use a multimeter to measure the precise conductivity in Siemens (S). Compare the value to known standards: high values indicate strong electrolytes and low values indicate weak electrolytes.

Key concepts

Aqueous Solution

An aqueous solution is formed when a substance, such as the compound \(\mathrm{X}\), is dissolved in water. This solution is crucial for testing the properties of the substance, especially its ability to conduct electricity. In a typical aqueous solution, water serves as the solvent, allowing molecules or ions of the solute to disperse evenly.

• The dissolution process depends on the nature of the solute and its interaction with water molecules.
• Polar substances, like many ionic compounds, dissolve readily, forming an aqueous solution.
• Non-polar substances may not dissolve in water, thus not forming a true aqueous solution.

For compound \(\mathrm{X}\), creating an aqueous solution is the first step in assessing whether it's an electrolyte or not. The presence of free ions in the solution indicates the potential for conductivity.

Conductivity Measurement

Conductivity measurement helps determine the electrical conductance of a substance dissolved in water. This is a key test for identifying electrolytes, as it directly reveals the ability of a solution to carry electric current.

• The setup typically involves inserting electrodes into the aqueous solution.
• Connecting these electrodes to a conductivity meter or a simple circuit gauge displays the level of electrical flow.
• A reading on the meter or a complete circuit illuminating a light bulb confirms the presence of ions in the solution.

A higher conductivity reading suggests more ions and hence stronger electrolytic nature. It gives an initial understanding of whether compound \(\mathrm{X}\) is a strong or weak electrolyte.

Strong and Weak Electrolytes

Understanding strong and weak electrolytes is essential to categorize the conductive nature of solution \(\mathrm{X}\). Once determined that a solution conducts electricity, we must further discern the level of its conductivity.

• Strong electrolytes are substances that completely dissociate into ions in solution. They exhibit high conductivity, lighting up bulbs brightly or showing high meter readings.
• Weak electrolytes only partially dissociate, resulting in fewer free ions. Consequently, they show lower conductivity; thus, bulbs glow dimly or meters read low.

This distinction is valuable in chemical processes where the strength of an electrolyte affects reaction rates and equilibria in aqueous solutions.

Ionization in Solution

Ionization in solution refers to the process by which molecules or compounds form ions upon dissolving in a solvent like water. It's the key mechanism by which compounds become electrolytes:

• When a strong electrolyte dissolves, it ionizes completely, releasing more ions into the solution, enabling better conductivity.
• Weak electrolytes, on the other hand, only partially ionize, resulting in fewer ions available to conduct electricity.

Evident in the conductivity test, the degree of ionization significantly influences the electrical behavior of the solution. Fully understanding ionization empowers learners to predict and manipulate the behavior of dissolved substances in various chemical contexts.