The hydornium ion concentration in blood of three different patiens was:
Patient [H30+]
A 5.0 X 10^-8
B 3.1 X 10^-8
C 3.2 X 10^-8
What is the pH of each patient's blood? If the normal range is 7.30-7.50, which, if any, of these patient's have an abnormal blood pH?
pH = -log(H3O^+)
Plug and chug.
To find the pH of each patient's blood, we can use the formula:
pH = -log[H₃O⁺]
where [H₃O⁺] is the concentration of the hydronium ion.
Let's calculate the pH for each patient:
For Patient A:
[H₃O⁺] = 5.0 x 10⁻⁸
pH = -log(5.0 x 10⁻⁸)
To calculate the value, we take the negative logarithm of the concentration using base 10.
pH = -log(5.0 x 10⁻⁸) ≈ 7.3 (rounded to one decimal place)
For Patient B:
[H₃O⁺] = 3.1 x 10⁻⁸
pH = -log(3.1 x 10⁻⁸)
pH = -log(3.1 x 10⁻⁸) ≈ 7.5 (rounded to one decimal place)
For Patient C:
[H₃O⁺] = 3.2 x 10⁻⁸
pH = -log(3.2 x 10⁻⁸)
pH = -log(3.2 x 10⁻⁸) ≈ 7.5 (rounded to one decimal place)
Now, let's check if any of these pH values fall outside the normal range of 7.30-7.50:
Patient A has a pH of 7.3, which falls within the normal range.
Patient B has a pH of 7.5, which also falls within the normal range.
Patient C has a pH of 7.5, which is also within the normal range.
Therefore, none of these patients have an abnormal blood pH since their pH values fall within the normal range of 7.30-7.50.