If a liquid has hydrogen ion concentration of [H^+] moles per liter, its pH = -l

Question

If a liquid has hydrogen ion concentration of [H^+] moles per liter, its pH = -log[H^+]. The pH of surface ocean water in 1751 is estimated to have been 8.25. Compute the hydrogen ion concentration of surface ocean water in 1751. The acidity of the ocean has increased since then. In 1994 the hydrogen ion concentration was about 7.23336 times 10^-9 moles per liter. By how much did the pH drop since 1751? Would it be accurate to say that the "acidity" of the world's oceans (the concentration [H^+]) increased about 28.6%? Explain why or why not.

Explanation / Answer

a)
pH = -log [H+]
8.25 = -log [H+]
[H+] = 5.62341*10^-9 M

Answer: 5.62341*10^-9 M

b)
pH = -log [H+]
= -log (7.23336*10^-9)
= 8.14
Answer: 8.14

increase in H+ =(7.23336 - 5.62341)*10^-9 *100/ (5.62341*10^-9)
= 28.6 %

Answer: Yes it is accurate

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