What mass of calcium carbonate (CaCO3) is required to neutralize 20 ML of sulphuric acid (H2SO4) of concentration 490 g/L?
BALANCE the equation
CaCO3 + H2SO4>>>CaSO4 + H2O + CO2
so for every mole of sulfuric acid you need one mole of calcium carbonate.
Moles Sulfuric acid= 20/1000*490/molmassH2SO4
=20/1000*490/98=.1 moles check that.
mass of CaCO3: .1moles*molmass=.1*100=10grams.
check my math
Why did the calcium carbonate go to therapy?
Because it had acid-neutralization issues! 😄
To calculate the mass of calcium carbonate required to neutralize the sulfuric acid, we need to consider the stoichiometry of the reaction. The balanced chemical equation for the reaction is:
CaCO3 + H2SO4 -> CaSO4 + H2O + CO2
From the equation, we can see that the molar ratio between calcium carbonate (CaCO3) and sulfuric acid (H2SO4) is 1:1. This means that 1 mole of calcium carbonate reacts with 1 mole of sulfuric acid.
First, we need to find the number of moles of sulfuric acid present in the given volume (20 mL) of the solution. We can use the concentration (490 g/L) to calculate this:
Number of moles of H2SO4 = Concentration x Volume
Number of moles of H2SO4 = (490 g/L) x (20 mL) / 1000 mL/L = 9.8 g
Since the molar ratio is 1:1, the number of moles of calcium carbonate required to neutralize the sulfuric acid is also 9.8 g.
Hence, the mass of calcium carbonate required to neutralize 20 mL of sulfuric acid of concentration 490 g/L is 9.8 grams.
To determine the mass of calcium carbonate required to neutralize the sulfuric acid, we need to use stoichiometry and the balanced equation for the reaction.
The balanced equation for the reaction between calcium carbonate (CaCO3) and sulfuric acid (H2SO4) is:
CaCO3 + H2SO4 -> CaSO4 + H2O + CO2
From the balanced equation, we can see that 1 mole of calcium carbonate reacts with 1 mole of sulfuric acid.
1 mole of sulfuric acid (H2SO4) has a molar mass of 98 g/mol.
To determine the number of moles of sulfuric acid in 20 mL of a 490 g/L solution, we need to convert mL to L.
20 mL = 20 / 1000 = 0.02 L
The number of moles of sulfuric acid can be calculated using the molarity formula:
moles = concentration (g/L) x volume (L) / molar mass (g/mol)
moles = 490 g/L x 0.02 L / 98 g/mol
moles = 0.1 mol
Since 1 mole of calcium carbonate reacts with 1 mole of sulfuric acid, we need 0.1 moles of calcium carbonate.
The molar mass of calcium carbonate (CaCO3) is 100 g/mol.
Mass = moles x molar mass
Mass = 0.1 mol x 100 g/mol
Mass = 10 g
Therefore, 10 grams of calcium carbonate (CaCO3) is required to neutralize 20 mL of sulfuric acid (H2SO4) with a concentration of 490 g/L.
To determine the mass of calcium carbonate required to neutralize the given volume of sulfuric acid, we need to follow these steps:
Step 1: Calculate the number of moles of sulfuric acid.
To do this, we need to convert the given volume of sulfuric acid to liters, using the conversion factor 1 mL = 0.001 L.
20 mL * 0.001 L/mL = 0.02 L
Next, we can calculate the number of moles using the formula:
Number of moles = concentration (in g/L) * volume (in L) / molar mass (in g/mol)
Molar mass of H2SO4 = (1 * 2) + (32.06) + (4 * 16.00) = 98.09 g/mol
Number of moles of H2SO4 = 490 g/L * 0.02 L / 98.09 g/mol
Step 2: Calculate the stoichiometric ratio.
The balanced chemical equation for the neutralization of sulfuric acid and calcium carbonate is:
H2SO4 + CaCO3 → CaSO4 + CO2 + H2O
From the equation, we can see that one mole of sulfuric acid reacts with one mole of calcium carbonate.
So the stoichiometric ratio is 1:1.
Step 3: Calculate the mass of calcium carbonate.
Since the stoichiometric ratio is 1:1, the number of moles of calcium carbonate required will be the same as the number of moles of sulfuric acid:
Number of moles of CaCO3 = Number of moles of H2SO4
Finally, we can calculate the mass using the formula:
Mass (g) = Number of moles * molar mass
Molar mass of CaCO3 = (1 * 40.08) + (1 * 12.01) + (3 * 16.00) = 100.09 g/mol
Mass of CaCO3 = Number of moles of CaCO3 * molar mass of CaCO3
By plugging in the values, we can find the mass of calcium carbonate required.