How many tums tablets each 500mg CaCO3 will it take to neutralize quart of Vinegar 0.83 moler (CH3COOH)
assuming a quart is one liter, so you have .83 moles of acid in the vinegar.
CaCO3 + 2CH3COOH>>CO2 + H2O + C4H6O4Ca Calcium Acetate
so it takes one mole of calcium carbonate to neutralize 2 moles of acid.
You have .83 moles acid, so you need 0.415 moles, or .415*100 grams of tablets.
How many tablets? n*0.500 grams=41.5 or n= .... you do it.
To determine the number of Tums tablets needed to neutralize a quart of vinegar, we first need to calculate the amount of vinegar in moles.
Given:
- Vinegar concentration: 0.83 M (mol/L)
- Volume of vinegar: 1 quart (946.3 mL)
Step 1: Convert the volume of vinegar from quarts to liters:
1 quart = 946.3 mL = 0.9463 L
Step 2: Calculate the number of moles of acetic acid (CH3COOH) present in the vinegar using the formula:
moles = concentration (M) x volume (L)
moles of CH3COOH = 0.83 M x 0.9463 L = 0.7853 mol
Step 3: Determine the stoichiometry between calcium carbonate (CaCO3) and acetic acid (CH3COOH).
The balanced chemical equation for the neutralization reaction between CaCO3 and CH3COOH is:
CaCO3 + 2CH3COOH → Ca(CH3COO)2 + H2O + CO2
According to the balanced equation, 1 mole of CaCO3 reacts with 2 moles of CH3COOH.
Step 4: Calculate the number of moles of CaCO3 needed to neutralize the acetic acid:
moles of CaCO3 needed = (0.7853 mol CH3COOH) / 2 = 0.3927 mol
Step 5: Convert the moles of CaCO3 to mass using the molar mass of CaCO3:
Molar mass of CaCO3 = (40.08 g/mol) + (12.01 g/mol) + (3 * 16.00 g/mol) = 100.09 g/mol
mass of CaCO3 needed = (0.3927 mol CaCO3) x (100.09 g/mol) = 39.284 g
Step 6: Determine the number of Tums tablets needed, assuming each tablet contains 500 mg (0.5 g) of CaCO3:
number of Tums tablets needed = (39.284 g) / (0.5 g/tablet) ≈ 78.57
Therefore, it would take approximately 79 Tums tablets (rounded up) to neutralize a quart of 0.83 M vinegar.