Question

ph of aq. solution of 0.05M HCl

Answer 1

hello mate!....

➡️ given.....

0.05 M of HCL

$we \: know...... \\ \\ ph = - log \: (h {}^{ + } ) \\ \\ (h {}^{ + } ) = 0.05 \\ \\ then.... \\ \\ ph = - log(0.05) \\ \\ ph = 1.301$
HOPE IT HELPS U.....


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Answer 2

Given,

Molarity of HCl = 0.05M

To determine,

The pH of the HCl aqueous solution,

Solution,

The pH of the aqueous solution of HCl is 1.31

The numerical problem may be easily solved using the following strategy.

We already know that HCl is a powerful acid. As a result, it totally dissociates in an aqueous solution.

As a result, the concentrations of H⁺ and HCl are the same.

Now,

The pH of a solution = - log(H⁺)

where,

[H⁺] = [HCl] = 0.05M

Thus,

The pH of the aqueous solution of HCl = - log (0.05)

                                                                   = - (log (5) - log(100))

                                                                   = log(100) - log(5)

                                                                   = 2 - 0.69

                                                                   = 1.31

As a consequence, the pH of the aqueous solution of HCl is 1.31.