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18 September, 08:27

How many grams of Ag2CO3 are required to reacr with 28.5 mL of 1.00 M NaOH solution?

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  1. 18 September, 08:43
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    The reaction between Ag2CO3 and NaOH is shown by the equation below

    Ag2CO3 + NaOH = Ag2O + Na2CO3 + H2O

    we can determine the number of mole of sodium hydroxide

    by (2.85 ml * 1) : 1000 ml, since according to molarity 1 mole is contained in 100ml.

    we get 0.00285 moles of NaOH

    Using the mole ratio we can get the moles of Ag2CO3

    Mole ratio: Ag2NO3 : NaOH = 1:1

    Therefore, the moles of Ag2CO3 will be 0.00285 moles

    but 1 mole of silver carbonate is equivalent to 275.8 g

    Thus the mass will be calculated by 0.00285 moles * 275.8g = 0.78603g

    Mass of silver carbonate required will be 0.78603g
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