Sulfuric acid (H2SO4) is a very strong diprotic
acid. If 0.065 moles of sulfuric acid is mixed
with water to make 456 mililiter of solution,
what is the molarity of H+?
Answer in units of M.
If only one H^+ is involved, you will have 0.065 moles/0.456L = ??M
I don't know if you are to calculate the second H^+ or not? I suspect so since the question asks for M.
The second ionization is not a strong acid; the Ka (k2) is 1.2 x 10^-2 in my text but you should look it up in your text and use that number.
The ionization is
HSO4^- ==> H^+ + SO4^-2
k2 = 1.2 x 10^-2 = (H^+)(SO4^-2)/(HSO4^-).
Then you make an ICE chart, substitute and solve.
If you call this second H^+ x, the SO4^-2 will be x and HSO4^- will be 0.1425-x. Then into k2 you substitute
0.1425+x for H^+, x for SO4^- and 0.1425-x for HSO4^-.
I went through it and got close to 0.01 for x but you need to confirm that. The total H^+ then would be 0.1425 + 0.01 and to two s.f. I would round to 0.15 M. Check my thinking. Check my work carefully.
To find the molarity of H+ in the given solution of sulfuric acid, we need to determine the concentration of H+ ions in moles per liter of solution.
Sulfuric acid (H2SO4) is a diprotic acid, meaning it can donate two protons (H+ ions) per molecule. Each mole of sulfuric acid yields 2 moles of H+ ions.
Given that we have 0.065 moles of sulfuric acid, this will produce 0.065 x 2 = 0.13 moles of H+ ions.
The solution is prepared by diluting the 0.065 moles in 456 milliliters (mL) of solution, which is equal to 0.456 liters (L). Therefore, the molarity of H+ ions can be calculated using the formula:
Molarity (M) = moles of solute / volume of solution in liters
Molarity of H+ = 0.13 moles / 0.456 L = 0.2851 M
So, the molarity of H+ ions in the solution is 0.2851 M.