What is the Molarity of a solution formed by mixing 10.0g H2SO4 with enough water to make 100.0mL of solution?

Not well understood

To determine the molarity of a solution, you need to know the amount of solute (in moles) and the volume of the solution (in liters). Let's break down the steps:

1. Convert the given mass of H2SO4 (10.0g) into moles.
H2SO4 is an acid with a molar mass of approximately 98.09 g/mol.
Moles = mass / molar mass
Moles = 10.0g / 98.09 g/mol

2. Calculate the volume of the solution in liters.
The given volume is 100.0 mL, but molarity is typically expressed in liters.
Volume = 100.0 mL / 1000 (to convert mL to L)

3. Calculate the molarity (M) using the formula:
Molarity (M) = Moles / Volume

Now, let's perform the calculations:

1. Moles of H2SO4 = 10.0g / 98.09 g/mol
Moles of H2SO4 = 0.102 moles

2. Volume of the solution = 100.0 mL / 1000 L/mL
Volume of the solution = 0.100 L

3. Molarity (M) = 0.102 moles / 0.100 L
Molarity (M) = 1.02 M

Therefore, the molarity of the solution formed by mixing 10.0g of H2SO4 with enough water to make 100.0mL of solution is 1.02 M.

mols H2SO4 = grams/molar mass

Then M = mols H2SO4/L solution.
Note: 100 mL = 0.100 L.

What mass of water is required to dissolve 175 g of potassium nitrate to produce a 2.25 m solution?