Question

Calculate the ph of a solution prepared by dilution 3.0 ml of 2.5 m hcl to a final volume of 100 ml with h2o.

Answer 1

The pH of the solution after dilution is 1.125.

HCl is hydrochloric acid. It is known by the name muriatic acid. It is among the strong acids. It has a pungent smell and is colorless. It has a molar mass of 36.4 g/mol. It's a common reagent used in pharmaceutical industries. It is also used in other industries such as textile, rubber, and metal.

The volume of HCl added to the solution = 3.0 ml

The molar concentration of HCl = 2.5 M

Let the molar concentration of the solution after dilution is x.

The volume of the diluted solution = 100 ml.

The molar concentration of the solution after dilution is,

$M _{1} V _{2} = M_{2} V _{2}$

$M_{2} = \frac{ M _{1} V _{2}}{V _{2} }$

$M_{2} = \frac{2.5 \times 3}{100}$

$= 0.075 \: M$

Thus, the molar concentration of the solution after dilution is 0.075 M.

The pH of the solution after the dilution is,

$[HCl] = [H ^{ + } ] = 0.075 \: M$

$pH = - log [H ^{ + } ]$

$pH = - log(0.075)$

$pH = 1.125$

Therefore, the pH of the solution after dilution is 1.125.

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