Answer:
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.
