How many grams of H2SO4 are in 125 mL of a 3.00 M solution of H2SO4?

To find the number of grams of H2SO4 in a given volume of the solution, you need to use the formula:

Mass (in grams) = Concentration (in M) × Volume (in L) × Molar mass (in g/mol)

1. Convert the volume from milliliters (mL) to liters (L):
Volume = 125 mL ÷ 1000 mL/L = 0.125 L

2. Calculate the mass using the formula mentioned above:
Mass = 3.00 M × 0.125 L × (2 × 1.01 g/mol + 32.07 g/mol + 4 × 16.00 g/mol)

The molar mass of H2SO4 is 98.09 g/mol because it has 2 hydrogen atoms (2 × 1.01), 1 sulfur atom (32.07), and 4 oxygen atoms (4 × 16.00).

Simplifying the expression:
Mass = 3.00 M × 0.125 L × 98.09 g/mol

Solving the equation:
Mass = 3.67625 g

Therefore, there are 3.67625 grams of H2SO4 in 125 mL of a 3.00 M solution of H2SO4.

To calculate the number of grams of H2SO4 in the solution, we can use the equation:

moles = concentration (M) x volume (L)

First, we need to convert the volume from milliliters (mL) to liters (L). There are 1000 mL in 1 L, so:

125 mL ÷ 1000 = 0.125 L

Next, we substitute the given values into the equation:

moles = 3.00 M x 0.125 L

moles = 0.375 moles

To convert moles to grams, we need to know the molar mass of H2SO4. The molar mass of H2SO4 is:

2(1.01 g/mol) + 1(32.07 g/mol) + 4(16.00 g/mol) = 98.09 g/mol

Finally, we can calculate the grams of H2SO4 in the solution:

grams = moles x molar mass

grams = 0.375 moles x 98.09 g/mol

grams ≈ 36.77 grams

Therefore, there are approximately 36.77 grams of H2SO4 in 125 mL of a 3.00 M solution of H2SO4.