What concentration of sulfuric acid will make a solution of pH=3.4
From your earlier question about H2SO4, let's take the simple route.
pH = -log(H^+) so for pH of 3.4 then (H^+) = 3.98E-4
H2SO4 ==> 2H^+ + SO4^2-
So half that is what you want.
Oh, sulfuric acid, the not-so-refreshing choice of beverage! Well, if you're aiming for a pH of 3.4, you'll need to dilute your sulfuric acid solution to a concentration of approximately... drumroll, please... 0.000546 M! Just be careful not to mistake it for your morning orange juice, unless you're a fan of a good chemical reaction in your tummy!
To determine the concentration of sulfuric acid required to make a solution with a pH of 3.4, we can use the formula for calculating pH:
pH = -log[H+]
Here, [H+] represents the concentration of hydrogen ions in the solution. However, sulfuric acid dissociates into two hydrogen ions per molecule, so the concentration of [H+] will be twice the concentration of sulfuric acid.
Given that pH = 3.4, we can rearrange the formula to calculate [H+]:
10^(-pH) = [H+]
Substituting the pH value:
10^(-3.4) = [H+]
[H+] = 0.0000398107 M
Since the concentration of [H+] equals twice the concentration of sulfuric acid, we need to divide it by 2:
Sulfuric acid concentration = [H+] / 2
Sulfuric acid concentration = 0.0000398107 M / 2
Sulfuric acid concentration = 0.00001990535 M
Therefore, a sulfuric acid concentration of approximately 0.0000199 M will result in a solution with a pH of 3.4.
To determine the concentration of sulfuric acid needed to make a solution with a pH of 3.4, we can use the equation for the pH of a strong acid solution:
pH = -log[H+]
In this equation, [H+] is the concentration of hydrogen ions in moles per liter. Since sulfuric acid is a strong acid, it completely dissociates in water, meaning that the concentration of hydrogen ions is equal to the concentration of sulfuric acid.
Take the antilog of both sides of the equation:
10^(-pH) = [H+]
Substitute the given pH value into the equation:
[H+] = 10^(-3.4)
[H+] = 0.00039810717 moles per liter
Since sulfuric acid (H2SO4) dissociates to produce 2 moles of hydrogen ions for every mole of sulfuric acid, you need half the concentration of sulfuric acid to achieve the desired hydrogen ion concentration:
[H2SO4] = [H+] / 2
[H2SO4] = 0.00039810717 moles per liter / 2
[H2SO4] = 0.000199053585 moles per liter
Therefore, a sulfuric acid concentration of approximately 0.000199 M (moles per liter) will make a solution with a pH of 3.4.