Question

Calculate the pH of a solution with [H3O+] = 1.0 x 10-8 M please explain

Calculate the pH of a solution with [H3O+] = 1.0 x 10-8 M

please explain

Homework Answers

Answer #1

Given [H3O+] = 1.010 -8 M

We know that pH = -log [H3O+]

                         = -log(1.010 -8 )

                        = -[log1.0+ log 10 -8 )                 Since Log AB = log A + Log B

                       = - log 1.0 -(-8log 10 )                 Since log Ax = x log A

                       = 0 + (8x1)

                      = 8      

which is abuse since pH of an acidic solution should not exceeds 7

Sine the [H3O+] concentration is very weak

Total But the [H3O+]total = [H3O+] from the acid + [H3O+] from water

                               = 1.010 -8 M + 1.010 -7 M

                                 = 1.010 -7 (0.1+1)

                          = 1.1 10 -7 M

So pH = -log [H3O+]total

         = -log(1.110 -7 )

         = -[log1.1+ log 10 -7 )

         = - log 1.1 +7 log 10

         = -0.04 + 7

         = 6.96

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