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Anon25 [30]
3 years ago
14

The normal range of the pH of blood is between 7.35 and 7.45; variations beyond this range have significant health implications.

Calculate the hydrogen ion concentrations [H+ ] associated with these pH values. Express your answers in molarity to two significant figures.
Chemistry
1 answer:
patriot [66]3 years ago
8 0

Answer:

The hydrogen ion concentrations associated with these pH value 7.35 is 4.5\times 10^{-8} M

The hydrogen ion concentrations associated with these pH value 7.45 is 3.6\times 10^{-8} M.

Explanation:

To calculate the pH of the solution, we use the equation:

pH=-\log[H^+]

We are given:

1) pH = 7.35

Putting values in above equation, we get:

7.35=-\log[H^+]

[H^+]=4.467\times 10^{-8} M\approx 4.5\times 10^{-8} M

The hydrogen ion concentrations associated with these pH value 7.35 is 4.5\times 10^{-8} M

2) pH = 7.45

Putting values in above equation, we get:

7.45=-\log[H^+]

[H^+]=3.548\times 10^{-8}M \approx 3.6\times 10^{-8} M

The hydrogen ion concentrations associated with these pH value 7.45 is 3.6\times 10^{-8} M.

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