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10 December, 03:47

An Alkaline-Seltzer tablet contains exactly 100 mg of citric acid, H3C6H5O7, plus some sodium bicarbonate. What mass of sodium bicarbonate is required to consume 100. mg of citric acid by the following reaction?. H3C6H5O7 (aq) + 3 NaHCO3 (aq) = 3 H2O (l) + 3 CO2 (g) + Na3C6H5O7 (aq).

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  1. 10 December, 04:36
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    mass of NaHCO₃ = 0.126 g

    Explanation:

    balanced chemical equation

    H₃C₆H₅O₇ (aq) + 3 NaHCO₃ (aq) → 3 H₂O (l) + 3 CO₂ (g) + Na₃C₆H₅O₇ (aq).

    given data

    moles of citric acid = 1 mol

    mas of citric acid = 100 mg

    mas of citric acid = 0.1 g

    moles of sodium bicarbonate = 3 mol

    mass of sodium bicarbonate = ?

    Solution

    1st we will find out the mole ratio of H₃C₆H₅O₇ and NaHCO₃ from balanced chemical equation

    H₃C₆H₅O₇ : NaHCO₃

    1 : 3

    Now we find out number of moles of citric acid

    moles = mass / molar mass

    moles = 0.1 g / 192.124 g/mol

    moles = 0.0005 mol

    now we find out moles (x) of sodium bicarbonate needed for 0.0005 mol of citric acid

    from the balanced chemical equation the mole ratios are:

    1 : 3

    0.0005 mol : x

    Cross multiply these ratios

    3 * 0.0005 = 1x

    0.0015 = 1 x

    x = 0.0015 mol

    Now we will find out the mass of sodium bicarbonate

    mass = moles * molar mass

    mass of NaHCO₃ = 0.0015 mol * 84.007 g/mol

    mass of NaHCO₃ = 0.126 g
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