An antacid tablet containing calcium carbonate as an active ingredient required 9.19 mL of 0.0956 M H2SO4 for complete neutralization. The mass of the tablet was 0.193 g. What percent of calcium carbonate was in the tablet? Thanks!
To find the percentage of calcium carbonate in the tablet, we need to determine the number of moles of H2SO4 that reacted with the calcium carbonate.
1. Determine the number of moles of H2SO4:
- Volume of H2SO4 used: 9.19 mL = 9.19 x 10^(-3) L
- Concentration of H2SO4: 0.0956 M
- Number of moles of H2SO4 = Concentration x Volume
= 0.0956 mol/L x 9.19 x 10^(-3) L
= 8.78 x 10^(-4) mol
2. Determine the number of moles of CaCO3:
- The balanced equation for the reaction between H2SO4 and CaCO3 is:
H2SO4 + CaCO3 → CaSO4 + H2O + CO2
- From the balanced equation, we can see that 1 mole of H2SO4 reacts with 1 mole of CaCO3.
- Therefore, the number of moles of CaCO3 is also 8.78 x 10^(-4) mol.
3. Calculate the molar mass of CaCO3:
- The molar mass of CaCO3 is the sum of the atomic masses of calcium (Ca), carbon (C), and three oxygen (O) atoms.
- Mass of Ca: 1 atom x 40.08 g/mol = 40.08 g/mol
- Mass of C: 1 atom x 12.01 g/mol = 12.01 g/mol
- Mass of O: 3 atoms x 16.00 g/mol = 48.00 g/mol
- Molar mass of CaCO3 = 40.08 g/mol + 12.01 g/mol + 48.00 g/mol = 100.09 g/mol
4. Calculate the mass of CaCO3 in the tablet:
- Mass of H2SO4 = 8.78 x 10^(-4) mol x 98.09 g/mol (molar mass of H2SO4)
- = 8.63 x 10^(-2) g
- Mass of CaCO3 = Mass of tablet - Mass of H2SO4
- = 0.193 g - 8.63 x 10^(-2) g
- = 0.106 g
5. Calculate the percentage of calcium carbonate:
- Percentage of CaCO3 = (Mass of CaCO3 / Mass of tablet) x 100%
- = (0.106 g / 0.193 g) x 100%
- ≈ 55.02%
Therefore, the tablet contains approximately 55.02% of calcium carbonate.
To find the percentage of calcium carbonate in the tablet, we need to calculate the amount of calcium carbonate used in the neutralization reaction.
First, let's find the number of moles of H2SO4 used. We can do this using the equation:
moles of H2SO4 = Molarity of H2SO4 × Volume of H2SO4
In this case, the molarity of H2SO4 is 0.0956 M, and the volume used is 9.19 mL (which can be converted to liters by dividing by 1000):
moles of H2SO4 = 0.0956 M × (9.19 mL / 1000 mL/L)
Now, we can calculate the number of moles of calcium carbonate used in the reaction. According to the balanced chemical equation between calcium carbonate (CaCO3) and sulfuric acid (H2SO4), the molar ratio is 1:1. This means that for every mole of H2SO4, there is one mole of CaCO3.
moles of CaCO3 = moles of H2SO4
Next, we can calculate the mass of calcium carbonate used. The molar mass of CaCO3 can be calculated by adding up the atomic masses of calcium (Ca), carbon (C), and three oxygen (O) atoms.
molar mass of CaCO3 = (1 × atomic mass of Ca) + (1 × atomic mass of C) + (3 × atomic mass of O)
Now, we can calculate the mass of calcium carbonate:
mass of CaCO3 = moles of CaCO3 × molar mass of CaCO3
Finally, we can calculate the percentage of calcium carbonate in the tablet by dividing the mass of calcium carbonate by the mass of the tablet and multiplying by 100:
percentage of CaCO3 = (mass of CaCO3 / mass of tablet) × 100
Plugging in the given values, we can now calculate the percentage of calcium carbonate in the tablet.
9.19mL of .0956M H2SO4 contains
.00919*.0956 = .0008786 moles H2SO4
CaCO3 + H2SO4 = CaSO4 + H2CO3
since each mole of H2SO4 racats with one mole CaCO3, there were .0008786 moles CaCO3 in the tablet.
Since each mole CaCO3 has mass 100g, the pill was .08786/.193 = .455 = 45.5% CaCO3