Explain Acid Base Equilibrium

Question 1: The molar concentration of OH^– ions in a certain solution is 1.04 x 10^-5 mol L^-1. Calculate the pOH and then the pH of the solution.

Question 2: Death occurs if the pH of human blood plasma changes by more than about ±0.4 from its normal value of about pH = 7.4, the “safe” range is from neutral to slightly alkaline. What is the corresponding range of molar concentrations of hydrogen ions for which human life can be sustained?

Solution 1:

[OH^–] = 1.04 x 10^-5 mol L^-1

pOH = – log ₁₀ (1.04 x 10^-5) = 4.98

pH + pOH = 14.00

pH = 14.00 – 4.98 = 9.02

Solution 2:

Maximum pH = 7.8	7.8 = -log₁₀[H⁺]_max	[H⁺]_max = 10^-7.8
Maximum pH = 7.0	7.0 = -log₁₀[H⁺]_max	[H⁺]_max = 10^-7.0

From the definition of a logarithm we have [H⁺] = 10^-7.8 . The easiest way of solving this on your calculator is to use “shift-log” (which is 10^x) then type —7.8 then equals. Take care to use “shift-log” = 10^x not “shift-In” = e^x.

[H ⁺]_MAX = 1.58 x 10^-8 mol L^-1

[H ⁺]_MIN = 1.00 x 10^-7 mol L^-1

Human blood covers only a small range of proton concentrations. Here all explanation based on Acid Base Equilibrium.