Lead Compounds and Electrolyte Properties

The video tutorial explores whether lead(II) chloride (PbCl2) is an electrolyte or non-electrolyte. It begins by explaining the nature of electrolytes, which dissolve in water to produce ions that conduct electricity. The solubility of PbCl2 is examined, revealing it is slightly soluble, leading to limited ion formation. Consequently, PbCl2 is classified as a weak electrolyte due to its minimal ion presence in water, resulting in low conductivity.

What is the primary characteristic of an electrolyte?

• It remains solid in water.

• It does not conduct electricity.

• It produces ions in solution.

• It dissolves in non-polar substances.

Why should one be cautious with lead compounds in terms of solubility?

• They are always highly soluble.

• They are often insoluble.

• They never dissolve in water.

• They are non-polar substances.

What does the solubility table indicate about PbCl2?

• It is highly soluble.

• It is insoluble.

• It is slightly soluble.

• It does not dissolve at all.

What ions are formed when PbCl2 dissociates in water?

• Pb+ and Cl2-

• Pb3+ and Cl3-

• Pb2+ and Cl-

• Pb4+ and Cl4-

Why is PbCl2 considered a weak electrolyte?

• It produces a small number of ions.

• It is highly conductive.

• It produces a large number of ions.

• It does not produce any ions.

What is the charge on the lead ion when PbCl2 dissociates?

• 1+

• 2+

• 3+

• 4+

What is the final conclusion about PbCl2 in the video?

• It is a strong electrolyte.

• It is a non-electrolyte.

• It does not dissolve in water.

• It is a weak electrolyte.