Question

In: Chemistry

1) Calculate either [H3O ] or [OH

Solutions

Expert Solution

A) [OH]^- = 1.49 X 10 ^-7 M

[H3O]^+ x [OH]^- = 1 x 10^-14

[H3O]^+ = (1 x 10^-14) / [OH]^-

[H3O]^+ = (1 x 10^-14) / 1.49 X 10 ^-7

[H3O]^+ = 6.71 x 10^-8 M

-------------------------

B) [H3O]^+ = 7.81 X10^-9 M

[H3O]^+ x [OH]^- = 1 x 10^-14

[OH]^- = (1 x 10^-14) / [H3O]^+

[OH]^- = (1 x 10^-14) / (7.81 X10^-9)

[OH]^- = 1.28 x 10^-6

----------------------------------------------

C) [H3O]^+ = 0.000661 M = 6.61 x 10^-4 M

[H3O]^+ x [OH]^- = 1 x 10^-14

[OH]^- = (1 x 10^-14) / [H3O]^+

[OH]^- = (1 x 10^-14) / (6.61 x 10^-4)

[OH]^- = 1.51 x 10^-11 M

--------------------------------------------------------------------

pH = -log [H3O]^+

pH = -log ( 6.71 x 10^-8)

pH = 7.2

(As the pH is greater than 7, the solution is basic)

pH = -log [H3O]^+

pH = -log ( 7.81 X10^-9)

pH = 8.1

(As the pH is greater than 7, the solution is basic)

pH = -log [H3O]^+

pH = -log ( 6.61 x 10^-4)

pH = 3.2

(As the pH is less than 7, the solution is acidic)

Hence, solutions A and B are basic at 25 degree C

queen_honey_blossom answered 1 year ago

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