HCl Solution Concentration and pH

The video tutorial explains how to calculate the pH of a solution prepared by diluting a tenth molar HCl solution from 25 mL to 100 mL. It covers determining the number of moles of HCl, converting units, calculating the final molarity, and using this to find the pH. The process is explained systematically to aid understanding of similar problems.

What is the initial volume of the HCl solution used in the problem?

• 50 mL

• 25 mL

• 100 mL

• 10 mL

What is the concentration of the initial HCl solution before dilution?

• 1 M

• 0.01 M

• 0.1 M

• 0.001 M

How many moles of HCl are present in the initial 25 mL solution?

• 2.5 x 10^-3 moles

• 2.5 x 10^-2 moles

• 2.5 x 10^-4 moles

• 2.5 x 10^-1 moles

What is the concentration of HCl after the solution is diluted to 100 mL?

• 0.025 M

• 0.25 M

• 0.05 M

• 0.0025 M

What happens to HCl when it is added to water?

• It partially dissociates into ions.

• It forms a precipitate.

• It completely dissociates into H3O+ and Cl- ions.

• It remains as HCl molecules.

What is the formula used to calculate the pH of a solution?

• pH = -log[H3O+]

• pH = log[HCl]

• pH = log[H3O+]

• pH = -log[OH-]

What is the final pH of the solution after dilution?

• 2.6

• 1.6

• 0.6

• 3.6