What volume of 0.1M Of sulphuric acid is needed to neutralize 100cm³ of a solution of sodium carbonate of mass concentration 20gram over dm³
Equation is H2SO4 + Na2CO3 ==> Na2SO4 + H2O + CO2
mols Na2CO3 = grams/molar mass = ?
mols H2SO4 needed = mols Na2CO3 since 1 mol H2SO4 = 1 mol Na2CO3.
M H2SO4 = mols H2SO4/dm^3 H2SO4. You know M H2SO4 and mols H2SO4, solve for dm^3 H2SO4.
Post your work if you get stuck.
To determine the volume of 0.1M sulphuric acid needed to neutralize 100cm³ of a solution of sodium carbonate with a mass concentration of 20g/dm³, we need to follow these steps:
Step 1: Calculate the number of moles of sodium carbonate in the 100cm³ solution.
Mass concentration (g/dm³) = mass of solute (g) / volume of solution (dm³)
Number of moles = mass of solute (g) / molar mass of sodium carbonate (g/mol)
The molar mass of sodium carbonate (Na2CO3) is calculated by summing the atomic masses of its components:
Na (Sodium) = 22.99 g/mol
C (Carbon) = 12.01 g/mol
O (Oxygen) = 16.00 g/mol
Total molar mass = (2 * Na) + C + (3 * O)
Step 2: Convert the volume of solution from cm³ to dm³.
100cm³ = 100 / 1000 = 0.1 dm³
Step 3: Calculate the number of moles of sodium carbonate using the given mass concentration and volume of solution.
Number of moles = mass concentration (g/dm³) * volume of solution (dm³)
Step 4: Since the reaction between sodium carbonate and sulphuric acid is 1:1, the number of moles of sulphuric acid needed will be the same as the number of moles of sodium carbonate.
Step 5: Calculate the volume of 0.1M sulphuric acid required.
Volume (dm³) = number of moles * molar concentration (mol/dm³)
As the concentration is given as 0.1M, the volume will be the same as the number of moles.
By following these steps, you can calculate the volume of 0.1M sulphuric acid needed to neutralize 100cm³ of a solution of sodium carbonate with a mass concentration of 20g/dm³.