Question

A person suffered indigestion after eating a freshly jarred pickle. If the amount of white vinegar consumed in the pickle was 25.0 mL (5% or 0.80 M of aqueous acetic acid), how many tums would they need to consume to neutralize the acid?

Answer 1

To neutralize the acid in the jarred pickle, you would need an antacid such as Tums which contains calcium carbonate. The balanced equation for the neutralization reaction between acetic acid and calcium carbonate is 2CH3COOH + CaCO3 -> Ca(CH3COO)2 + H2O + CO2.

Step-by-step explanation:

Vinegar is a solution of acetic acid in water. To neutralize the acid, you would need an antacid such as Tums which contains calcium carbonate (CaCO3). The balanced equation for the neutralization reaction between acetic acid and calcium carbonate is:

2CH3COOH + CaCO3 → Ca(CH3COO)2 + H2O + CO2

Based on the equation, you can determine the number of moles of acetic acid present in the pickle (given the volume and molarity), and then calculate the number of moles of Tums (calcium carbonate) needed to neutralize that amount of acetic acid.

Answer 2

The number of tums they would need to consume to neutralize the acid = 2 tums

Step-by-step explanation:

The reaction between the acetic acid and the tums are as follows;

CaCO₃ + 2CH₃COOH → Ca(CH₃COO)₂ + H₂O + CO

Therefore, 1 mole of tums reacts with 2 moles of acetic acid

The number moles of acetic acid present is given as follows;

25 mL of 0.80 M acetic acid contains 25/1000 × 0.8 moles or 0.02 moles of acetic acid

Therefore, the number of moles of tums required = 0.02/2 = 0.01 moles

Molar mass of CaCO₃ = 100.0869 g/mol

Mass of 0.01 mole = Molar Mass × Number of moles = 100.0869 × 0.01 = 1.000869 g of tums

Mass of tums required = 1.000869 g≈ 1 gram

Size of tums available = 500 mg = 0.5 g

Therefore, number of tums required = 2 tums

The number of tums they would need to consume to neutralize the acid = 2 tums.