How many grams of solute in 3.5ml of 0.4N H2SO4?
mL x N x milliequivalent weight = grams
3.5 mL x 0.40 N x 98/2 = ?
To find the number of grams of solute in a given volume and concentration, we can use the formula:
Grams of solute = Volume (in liters) × Concentration (in moles/liter) × Molar mass (in grams/mole)
First, we need to convert the given volume from milliliters (ml) to liters (L):
3.5 ml = 3.5 ÷ 1000 = 0.0035 L
Next, we need to calculate the molar mass of H2SO4.
H2SO4 has two hydrogen atoms (H) with a molar mass of 1.01 g/mol each, one sulfur atom (S) with a molar mass of 32.07 g/mol, and four oxygen atoms (O) with a molar mass of 16.00 g/mol each.
Molar mass of H2SO4 = (2 × 1.01) + 32.07 + (4 × 16.00) = 98.09 g/mol
Now, we can calculate the grams of solute:
Grams of solute = 0.0035 L × 0.4 mol/L × 98.09 g/mol
Grams of solute = 0.0014 mol × 98.09 g/mol
Grams of solute = 0.137 g
Therefore, there are approximately 0.137 grams of solute in 3.5 ml of 0.4N H2SO4.
To find the number of grams of solute in a given volume and concentration of a solution, you need to use the formula:
grams of solute = volume (in liters) × concentration (in moles per liter) × molar mass (in grams per mole)
First, let's convert the given volume of the solution from milliliters (ml) to liters (L). Since 1 L = 1000 ml, dividing 3.5 ml by 1000 will give us the volume in liters:
3.5 ml ÷ 1000 = 0.0035 L
Next, let's determine the molar mass of H2SO4. It is the sum of the atomic masses of all the elements in the compound, which are:
H: 1.01 g/mol
S: 32.07 g/mol
O: 16.00 g/mol (there are four oxygen atoms in H2SO4)
Molar mass of H2SO4 = (2 × 1.01 g/mol) + 32.07 g/mol + (4 × 16.00 g/mol)
= 98.09 g/mol
Now, we can calculate the number of grams of solute:
grams of solute = 0.0035 L × 0.4 N × 98.09 g/mol
To calculate the grams of solute, simply multiply these three values together. Let's do the calculation:
grams of solute ≈ 0.14 grams
Therefore, there are approximately 0.14 grams of solute in 3.5 ml of 0.4N H2SO4.