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.

2h2o2--> 2h2o + o2

this reaction is of the spontaneous decomposition of hydrogen peroxide down into water and oxygen.

add 2 molecules of hydrogen peroxide and 2 molecules of water. since oxygen is naturally diatomic, the total number of atoms of each element is now the same on both sides of the equation so it is balanced.

this may not be entirely correct but let me know.