Number of Chloride in 100ml of 0.01M HCL Solution

To determine the number of chloride ions present in 100ml of a 0.01M HCl solution, we need to consider the stoichiometry of the reaction and the concept of molarity.

1. Understanding Molarity
Molarity (M) is a measure of the concentration of a solution, defined as the number of moles of solute dissolved per liter of solution. It is calculated using the formula:

Molarity (M) = Moles of solute / Volume of solution (in liters)

2. Stoichiometry of the Reaction
The balanced chemical equation for the dissociation of hydrochloric acid (HCl) in water is:

HCl → H+ + Cl-

From this equation, we can see that for every molecule of HCl that dissociates, one chloride ion (Cl-) is produced.

3. Calculation
Given that the concentration of the HCl solution is 0.01M, this means that there are 0.01 moles of HCl in 1 liter of solution.

To find the number of moles of HCl in 100ml (0.1L) of the solution, we can use the molarity formula:

Molarity (M) = Moles of solute / Volume of solution (in liters)

0.01M = Moles of HCl / 0.1L

Moles of HCl = 0.01M * 0.1L = 0.001 moles

Since the stoichiometry of the reaction tells us that there is one chloride ion (Cl-) for every molecule of HCl, the number of chloride ions in the solution is also 0.001 moles.

Finally, we can use Avogadro's number (6.023 × 10^23) to convert the number of moles to the number of chloride ions:

Number of chloride ions = 0.001 moles * 6.023 × 10^23 ions/mole = 6.023 × 10^20 ions

Answer:
The number of chloride ions in 100ml of a 0.01M HCl solution is 6.023 × 10^20 ions.

Note:
The given options A) 6.023× 10^23 and B) 6.023 × 10^24 are incorrect. The correct answer is 6.023 × 10^20 ions.

It shall be 6.023×10^20