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A person takes 6.1 g of an anta-acid tab...

A person takes `6.1 g` of an anta-acid tablet comprising bicarbonate ion at 20.8%. The volume of `CO_(2)` evolved at (1 atm and `25^(@)C`) in the stomach (on neutralisation) multipled by a factor of '10' will be `x L`. Calculate the approximate (integer) value of `x`.

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To solve the problem step by step, we need to calculate the volume of CO₂ evolved from the antacid tablet and then multiply that volume by a factor of 10 to find the value of \( x \). ### Step 1: Calculate the mass of bicarbonate ion in the antacid tablet Given that the antacid tablet weighs \( 6.1 \, \text{g} \) and contains \( 20.8\% \) bicarbonate ion (HCO₃⁻), we can calculate the mass of bicarbonate ion. \[ \text{Mass of HCO}_3^- = \frac{20.8}{100} \times 6.1 \, \text{g} = 1.2688 \, \text{g} \] ...
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