How many tums of Tablets each 500mg CaCo3 will it take to neutralize a quart of vinegar 0.83 moles (CH3COOH)
Didn't I just do this? Please don't post duplicates.
To calculate the number of Tums tablets needed to neutralize the given amount of vinegar, we need to understand the chemical reaction between calcium carbonate (CaCO3) and acetic acid (CH3COOH).
The balanced chemical equation for the reaction is as follows:
CaCO3 + 2CH3COOH → Ca(CH3COO)2 + H2O + CO2
From the equation, we see that 1 mole of CaCO3 reacts with 2 moles of CH3COOH to produce 1 mole of product (Ca(CH3COO)2), 1 mole of water (H2O), and 1 mole of carbon dioxide (CO2).
Step 1: Calculate the moles of acetic acid (CH3COOH) in a quart of vinegar.
Given: Moles of CH3COOH = 0.83 moles
Step 2: Determine the stoichiometric ratio between the reactants.
From the balanced equation, we see that 1 mole of CaCO3 reacts with 2 moles of CH3COOH.
Step 3: Calculate the moles of CaCO3 needed to neutralize the given moles of CH3COOH.
Moles of CaCO3 needed = Moles of CH3COOH / Stoichiometric ratio
= 0.83 moles / 2
= 0.415 moles of CaCO3
Step 4: Convert the moles of CaCO3 to milligrams.
Moles to milligrams conversion: 1 mole of CaCO3 = 1000 mg
0.415 moles × 1000 mg/mole = 415 mg of CaCO3
Step 5: Determine the number of Tums tablets required.
Each Tums tablet contains 500 mg of CaCO3.
Number of Tums tablets required = Total mg of CaCO3 / mg per tablet
= 415 mg / 500 mg per tablet
≈ 0.83 Tums tablets
Therefore, it would take approximately 0.83 Tums tablets of 500mg CaCO3 each to neutralize a quart of vinegar containing 0.83 moles of acetic acid (CH3COOH).