Sulfuric acid (H2SO4) is a very diprotic acid. If 0.046 moles of sulfuric acid is mixed with water to make 638 mililiter of solution,what is the molarity of H+? Answer in units of M.

M = mols/L of solution.

22M

656.8 To find the molarity of H+ in the sulfuric acid solution, we need to determine the number of moles of H+ ions present in the solution. Since sulfuric acid (H2SO4) is a diprotic acid, it can donate two protons (H+) per molecule.

Given:
Number of moles of sulfuric acid (H2SO4) = 0.046 moles
Total volume of solution = 638 mL

To find the molarity (M), we'll use the formula:

Molarity (M) = moles of solute / volume of solution in liters

First, we need to calculate the volume of the solution in liters:

Volume of solution (L) = 638 mL × (1 L / 1000 mL) = 0.638 L

Now, let's calculate the moles of H+ ions present in 0.046 moles of sulfuric acid. Since each molecule of sulfuric acid donates 2 H+ ions, we'll multiply the number of moles of sulfuric acid by 2:

Moles of H+ ions = 0.046 moles × 2 = 0.092 moles

Finally, we can calculate the molarity of H+ ions:

Molarity (H+) = 0.092 moles / 0.638 L = 0.144 M

Therefore, the molarity of H+ ions in the sulfuric acid solution is 0.144 M.