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.