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I want to make sodium acetate from sodium bicarbonate and vinegar. I'm a bit stumped at calculating amounts of each reagent. I'm starting with 8% acetic acid vinegar. I was going to add, to 1 L of the 8% acid (80 mL acetic acid), 80 grams of bicarb soda. I came to this as the 80 mL acetic acid has a mass of ~83 grams, and I'm guessing I should use an excess of acetic acid. Is this right?

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  • $\begingroup$ You should use excess of acid, but excess in terms of the number of moles. Reactions occur not by weight, but by moles. Weight of compound = number of moles x molar mass $\endgroup$
    – TRC
    Aug 13 '21 at 15:47
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The density of acetic acid is 1.053 g/ml, so you'll have 80 x 1.053g = 84.24g of acetic acid in 1L. The molecular weight of acetic acid is 60.052 so you have 80 x 1.053/60 = 1.404 moles. Multiply this by the molecular weight of sodium bicarbonate which is 84.007 to get the weight of sodium bicarbonate required for equivalence = 117.946g.

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