The approximate concentration of hcl,in the stomach is 0.17.Calculate the mass of the following antacids required to neutralise
A bicarbonate of soda NaHCO3
Aluminum hydroxide Al(OH)3
To calculate the mass of antacids required to neutralize a given concentration of HCl, you'll need to use the concept of stoichiometry and balanced chemical equations.
Step 1: Write the balanced chemical equation for the neutralization reaction between HCl and the respective antacid.
The balanced chemical equation for the neutralization of HCl with sodium bicarbonate (NaHCO3) is:
2NaHCO3 + 2HCl → 2CO2 + 2H2O + 2NaCl
The balanced chemical equation for the neutralization of HCl with aluminum hydroxide (Al(OH)3) is:
Al(OH)3 + 3HCl → AlCl3 + 3H2O
Step 2: Determine the molar ratio between HCl and the antacid.
For sodium bicarbonate (NaHCO3):
From the balanced equation, 2 moles of NaHCO3 neutralize 2 moles of HCl. Therefore, the molar ratio between NaHCO3 and HCl is 1:1.
For aluminum hydroxide (Al(OH)3):
From the balanced equation, 1 mole of Al(OH)3 neutralizes 3 moles of HCl. Therefore, the molar ratio between Al(OH)3 and HCl is 1:3.
Step 3: Convert the given concentration of HCl to moles.
Given:
Concentration of HCl = 0.17 M (moles per liter)
To convert the concentration to moles, we need to multiply by the volume. However, since the volume is not given, we'll assume it to be 1 liter for simplicity.
Moles of HCl = Concentration × Volume
Moles of HCl = 0.17 M × 1 L
Moles of HCl = 0.17 moles
Step 4: Calculate the mass of the antacid required using the molar ratio.
For sodium bicarbonate (NaHCO3):
Since the molar ratio between NaHCO3 and HCl is 1:1, the mass of NaHCO3 required would be equal to the moles of HCl we calculated in Step 3.
Mass of NaHCO3 = Moles of HCl × molar mass of NaHCO3
For aluminum hydroxide (Al(OH)3):
Since the molar ratio between Al(OH)3 and HCl is 1:3, we need to consider the molar mass of Al(OH)3 and convert the moles of HCl used earlier to moles of Al(OH)3.
Mass of Al(OH)3 = (Moles of HCl × (1 mole of Al(OH)3 / 3 moles of HCl)) × molar mass of Al(OH)3
Step 5: Calculate the final mass of the antacids.
Use the molar mass values:
NaHCO3: 84.01 g/mol
Al(OH)3: 78.00 g/mol
Plug in the previously calculated values to find the mass required for each antacid.
Note: Since we initially assumed the volume as 1 liter, the masses calculated here represent the amount required to neutralize 0.17 moles of HCl in 1 liter of solution. If the actual volume is different, you would need to adjust the amount of antacid accordingly.
I hope this explanation helps you calculate the mass of antacids required to neutralize HCl!