Sulfuric acid (H2SO4) is a very strong diprotic
acid. If 0.036 moles of sulfuric acid is mixed
with water to make 576 mililiter of solution,
what is the molarity of H+?
Molarity=(moles/Litersvolume)* 2
To find the molarity of H+ in the sulfuric acid solution, you need to first calculate the total number of moles of H+ ions present in the solution. Since sulfuric acid is a diprotic acid, it can donate two protons (H+ ions) per molecule.
Given:
Number of moles of sulfuric acid (H2SO4) = 0.036 moles
In one molecule of sulfuric acid (H2SO4), there are two H+ ions. Therefore, the number of moles of H+ ions in the solution is equal to twice the number of moles of sulfuric acid.
Number of moles of H+ ions = 2 * Number of moles of H2SO4
Number of moles of H+ ions = 2 * 0.036 moles
Next, you need to calculate the volume of the solution in liters. The given volume is in milliliters, so you need to convert it to liters by dividing it by 1000:
Volume of solution = 576 milliliters = 576/1000 = 0.576 liters
Finally, you can calculate the molarity (M) of H+ ions using the formula:
Molarity (M) = Number of moles of H+ ions / Volume of solution in liters
Molarity of H+ ions = (2 * 0.036 moles) / 0.576 liters
Now, you can calculate the molarity of H+ ions in the sulfuric acid solution.