To make some solution 500mL H2SO4 0.3 M. How many grams of H2SO4 are used?
find the RMM OF H2SO4 =2+32+(16*4) =98
there fore 1mole =98gm what for 0.3M
0.3*98/1=29.4gms
weigh 29.4 gms
I disagree with the answer by wilred ngure"skyicon". That calculation gives grams H2SO4 for 1 L of soln. The problem asks for 500 mL.
mols needed = M x L = 0.3 x 0.5 = 0.15
0.15 mols x molar mass of 98 = 14.7 grams.
To calculate the number of grams of H2SO4 needed to make a 500mL solution of 0.3 M concentration, you will need to use the formula:
n = C x V
Where:
n = number of moles of solute (H2SO4)
C = concentration in moles per liter (M)
V = volume of the solution in liters
First, convert the volume from milliliters to liters:
V = 500 mL / 1000 mL/L = 0.5 L
Next, substitute the given values into the formula:
n = 0.3 M x 0.5 L = 0.15 moles
To convert moles to grams, you will need the molar mass of H2SO4. The molar mass of H2SO4 is calculated as follows:
(2 x Atomic mass of H) + Atomic mass of S + (4 x Atomic mass of O) = (2 x 1.008 g/mol) + 32.06 g/mol + (4 x 16.00 g/mol) = 98.09 g/mol
Finally, calculate the mass using the number of moles and the molar mass:
Mass = n x Molar mass = 0.15 moles x 98.09 g/mol = 14.72 grams
Therefore, approximately 14.72 grams of H2SO4 would be needed to make a 500mL solution of 0.3 M concentration.