The ph of 0.001dm3 of hcl is?

Question: The ph of 0.001dm3 of hcl is?

The pH of a solution is a measure of its acidity, defined as the negative logarithm (base 10) of the hydrogen ion concentration ([H+]) in moles per liter (M). The pH scale ranges from 0 to 14, with a pH of 7 considered neutral, pH less than 7 considered acidic, and pH greater than 7 considered basic or alkaline.

To determine the pH of a solution of HCl with a volume of 0.001 dm3 (or 1 mL), we need to know the concentration of HCl in the solution. Let's assume that the concentration of HCl is x mol/dm3. 

The balanced chemical equation for the dissociation of HCl in water is:

HCl + H2O ⇌ H3O+ + Cl-

This means that in aqueous solution, HCl dissociates into H+ ions and Cl- ions. Since HCl is a strong acid, it dissociates completely in water, so the concentration of H+ ions in the solution is equal to the concentration of HCl.

Using the definition of pH, we can write:

pH = -log[H+]

Substituting [H+] with the concentration of HCl, we get:

pH = -log(x)

We can use the fact that the solution contains 0.001 dm3 (or 1 mL) of HCl to relate the concentration to the amount of HCl in moles:

x mol/dm3 = moles of HCl / volume of solution in dm3

Since the volume of solution is 0.001 dm3 and the molarity of HCl is x mol/dm3, the number of moles of HCl in the solution is:

moles of HCl = x mol/dm3 x 0.001 dm3 = 0.001 x mol

Therefore, the concentration of H+ ions in the solution is also 0.001 x mol/dm3.

Substituting this value into the pH equation, we get:

pH = -log(0.001 x)

Taking the negative logarithm of 0.001 x, we get:

pH = -log(0.001) - log(x)

pH = 3 - log(x)

So the pH of the HCl solution with a volume of 0.001 dm3 and a concentration of x mol/dm3 is 3 - log(x).

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