The ion product Of D2O is 1.35x 10^-15 at 25 degrees C. For a solution to be acidic the PDF must be what?
A distribution curve shows how the fractions of non ionized acid and its conjugate base vary as a function of Ph. The curves of the plot of [CH3COOH] vs. Ph and [CH3COO-] vs. Ph will intersect at a Ph of what? I need to show work
To determine the acidity of a solution, we can use the concept of pH, which is a measure of the concentration of hydrogen ions (H+) in a solution. The pH scale ranges from 0 to 14, where pH values below 7 indicate acidity, pH 7 is neutral, and pH values above 7 indicate alkalinity or basicity.
The ion product of water, also known as the autoprotolysis constant or self-ionization constant, can be represented as follows:
H2O ⇌ H+ + OH-
In pure water at 25 degrees Celsius, the concentration of both H+ and OH- ions is the same, giving an equal value for their concentration, typically represented by [H+] and [OH-].
The ion product of water (Kw) is the product of these concentrations:
Kw = [H+][OH-]
Given that the ion product of D2O (heavy water, where the hydrogen is replaced with deuterium) is 1.35x10^-15, we can assume the value of [H+] and [OH-] is the same in this case and can be represented as x:
Kw = x^2
Given Kw = 1.35x10^-15, we can solve for x by taking the square root of Kw:
√(1.35x10^-15) ≈ 1.16x10^-8
So, the concentration of both [H+] and [OH-] in the solution would be approximately 1.16x10^-8 M.
To determine if a solution is acidic, neutral, or basic, we compare the concentration of H+ ions to OH- ions. In an acidic solution, [H+] > [OH-], in a basic solution, [OH-] > [H+], and in a neutral solution, [H+] = [OH-].
In this case, given that both [H+] and [OH-] are approximately 1.16x10^-8 M, the solution is neutral since the concentrations of H+ and OH- ions are equal.
Therefore, to answer your question, for a solution to be acidic, the concentration of H+ ions ([H+]) must be higher than the concentration of OH- ions ([OH-]).