How much sodium bicarbonate is required to neutralise 1.5 litres of acetic acid
Your School SUBJECT is SCIENCE.
How strong is the acetic acid?
Well, assume worst-case I guess with glacial. What's that, molarity about 17.4?
About 5 pounds of bicarb will do it (2193 grams) then, right?
To determine the amount of sodium bicarbonate required to neutralize acetic acid, we need to first identify the balanced chemical equation, which represents the reaction between acetic acid (CH3COOH) and sodium bicarbonate (NaHCO3).
The balanced chemical equation for the reaction is as follows:
CH3COOH + NaHCO3 -> CH3COONa + H2O + CO2
From the equation, we can see that 1 mole of CH3COOH reacts with 1 mole of NaHCO3 to produce 1 mole of CO2, 1 mole of CH3COONa, and 1 mole of H2O.
Now, we need to convert the given volume of acetic acid (1.5 liters) into moles. To do this, we need to know the concentration of acetic acid.
Let's assume the concentration of acetic acid is given as 2 M (molar). This means there are 2 moles of acetic acid in 1 liter of solution.
Therefore, the number of moles of acetic acid in 1.5 liters can be calculated as follows:
moles of acetic acid = volume (liters) * concentration (M)
moles of acetic acid = 1.5 liters * 2 M
moles of acetic acid = 3 moles
From the balanced equation, we know that 1 mole of acetic acid reacts with 1 mole of sodium bicarbonate. Therefore, the number of moles of sodium bicarbonate required to neutralize 3 moles of acetic acid is also 3 moles.
To convert moles of sodium bicarbonate into grams, we need to know the molar mass of NaHCO3, which is:
Na - 22.99 g/mol
H - 1.01 g/mol
C - 12.01 g/mol
O - 16.00 g/mol
Molar mass of NaHCO3 = (22.99 + 1.01 + 12.01 + (3 * 16.00)) g/mol
Molar mass of NaHCO3 = 84.01 g/mol
Therefore, the mass of sodium bicarbonate required can be calculated as follows:
mass of sodium bicarbonate = moles of NaHCO3 * molar mass of NaHCO3
mass of sodium bicarbonate = 3 moles * 84.01 g/mol
mass of sodium bicarbonate = 252.03 grams
Hence, approximately 252.03 grams of sodium bicarbonate is required to neutralize 1.5 liters of acetic acid with a concentration of 2 M.