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?

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

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.

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