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Acid and Base Watch

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    A typical vitamin C tablet (containing pure ascorbic acid, H2C6H6O6) weighs 500 mg. One vitamin C tablet is dissolved in enough water to make 200.0 mL of solution. Calculate the pH of this solution. Ascorbic acid is a diprotic acid.
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    (Original post by Hemashini)
    A typical vitamin C tablet (containing pure ascorbic acid, H2C6H6O6) weighs 500 mg. One vitamin C tablet is dissolved in enough water to make 200.0 mL of solution. Calculate the pH of this solution. Ascorbic acid is a diprotic acid.
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    pH = -log[H+]

    so we need to find the conc of H+ ions in the solution
    moles of acid = mass/ Mr = 0.5g / (176) = 0.00284 moles
    ascorbic acid is diprotic meaning it releases 2 protons
    so moles of H+ = 0.00284*2 = 0.00568

    and then you use the equation
 
 
 
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