Sulfuric acid (H2SO4) is a very strong diprotic
acid. If 0.062 moles of sulfuric acid is mixed
with water to make 200 mililiter of solution,
what is the molarity of H+?
Answer in units of M
To find the molarity of H+ (hydrogen ions), we need to calculate the amount of H+ ions present in the solution.
Sulfuric acid is a diprotic acid, meaning it can donate two hydrogen ions (H+) per molecule. Since each mole of sulfuric acid produces two moles of H+ ions, we can convert the given amount of sulfuric acid to moles of H+ ions.
Given:
- Moles of sulfuric acid (H2SO4) = 0.062 moles
- Volume of solution = 200 milliliters = 0.2 liters (since 1 liter = 1000 milliliters)
To calculate the moles of H+ ions:
Moles of H+ ions = 2 * moles of sulfuric acid
Moles of H+ ions = 2 * 0.062 moles = 0.124 moles
Now, we can calculate the molarity (M) of H+ ions:
Molarity = Moles / Volume
Molarity of H+ ions = 0.124 moles / 0.2 L = 0.62 M
Therefore, the molarity of H+ ions in the solution is 0.62 M (moles per liter).
M H2SO4 = mols/L = 0.062 mols/0.200L = ?M H2SO4.
M H^+ is 2x that.