Calculate the normality and molarity of h2so4 solutions containing 4.9g of h2so4 per liter of solutions?
Molarity = mols/L and mols = g/molar mass so
mols = 4.9/98 = 0.05. You have 0.05 mols/L - 0.05 M.
N = 2 x M = 0.05 x 2 = ?
To calculate the normality and molarity of H2SO4 solutions, we need to know the molar mass of H2SO4. The molar mass of H2SO4 can be calculated by adding the atomic masses of each element.
H2SO4 contains:
- 2 hydrogen atoms with an atomic mass of 1.008 g/mol (2 x 1.008 g/mol)
- 1 sulfur atom with an atomic mass of 32.06 g/mol
- 4 oxygen atoms with an atomic mass of 16.00 g/mol (4 x 16.00 g/mol)
Therefore, the molar mass of H2SO4 is:
2(1.008) + 32.06 + 4(16) = 98.09 g/mol
To calculate the normality, we need to determine the number of equivalents of H2SO4 per liter of solution. H2SO4 is a diprotic acid, which means it can donate two hydrogen ions (H+) per molecule.
The normality (N) can be calculated using the formula:
Normality (N) = (Number of moles of solute) / (Volume of solution in liters) * Number of equivalents
Given that the solution contains 4.9 g of H2SO4 per liter of solution, we can calculate the number of moles of H2SO4 using the molar mass:
Number of moles of H2SO4 = (Mass of H2SO4) / (Molar mass of H2SO4)
= 4.9 g / 98.09 g/mol
= 0.05 mol
Since H2SO4 is a diprotic acid, it donates two moles of H+ ions per mole.
Number of equivalents of H2SO4 = (Number of moles of H2SO4) x 2
= 0.05 mol x 2
= 0.10 equivalents
Now we can calculate the normality:
Normality (N) = (Number of moles of H2SO4) / (Volume of solution in liters) * Number of equivalents
= (0.05 mol) / (1 L) * 0.10 equivalents
= 0.10 N
To calculate the molarity, we divide the number of moles of solute by the volume of solution in liters:
Molarity (M) = (Number of moles of H2SO4) / (Volume of solution in liters)
= 0.05 mol / 1 L
= 0.05 M
Therefore, the normality of the H2SO4 solution is 0.10 N, and the molarity is 0.05 M.
To calculate the normality (N) and molarity (M) of H2SO4 solutions, we need to know the molar mass of H2SO4. The molar mass of H2SO4 can be calculated by adding up the atomic masses of each element in the compound.
H2SO4 contains:
2 hydrogen atoms (H) with an atomic mass of 1.008 g/mol each
1 sulfur atom (S) with an atomic mass of 32.06 g/mol
4 oxygen atoms (O) with an atomic mass of 16.00 g/mol each
Using these values, the molar mass of H2SO4 can be calculated as follows:
Molar Mass = (2 * 1.008 g/mol) + (1 * 32.06 g/mol) + (4 * 16.00 g/mol)
= 2.016 g/mol + 32.06 g/mol + 64.00 g/mol
= 98.076 g/mol
Now, we can calculate the normality of the solution. Normality is defined as the number of equivalents of the solute (in this case, H2SO4) present in one liter of the solution. Since H2SO4 is a diprotic acid, meaning it can donate two protons (H+ ions) per molecule, the number of equivalents of H2SO4 is twice the molarity.
Normality (N) = 2 * Molarity (M)
To find the molarity, we need to convert the mass of H2SO4 given to moles, and then divide it by the volume of the solution.
First, let's convert the mass of H2SO4 into moles:
Mass = 4.9 g
Molar mass = 98.076 g/mol (calculated earlier)
Moles of H2SO4 = Mass / Molar mass
= 4.9 g / 98.076 g/mol
≈ 0.0499 mol
Next, let's calculate the molarity by dividing moles by the volume in liters:
Volume = 1 L
Molarity (M) = Moles / Volume
= 0.0499 mol / 1 L
≈ 0.0499 M
Finally, we can calculate the normality using the formula mentioned earlier:
Normality (N) = 2 * Molarity (M)
= 2 * 0.0499 M
= 0.0998 N
Therefore, the normality of the H2SO4 solution containing 4.9g of H2SO4 per liter is approximately 0.0998 N, and the molarity is approximately 0.0499 M.