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26 December, 02:02

How many grams of precipitate can be formed in the reaction between 6.00 mL of 0.10 M silver nitrate and 5.00 mL of 0.15 M potassium chloride? Hint: Start with a balanced chemical equation. Do not enter units with your answer.

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  1. 26 December, 02:20
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    0.09 g of precipitate can be formed.

    Explanation:

    The chemical equation can be written as follows:

    AgNO₃ + KCl → AgCl (↓) + NO₃⁻ + K⁺

    From the equation, we know that 1 mol AgNO₃ reacts with 1 mol KCl to produce 1 mol AgCl.

    The problem gives us data to calculate the initial number of moles of silver nitrate and potassium chloride:

    n° of moles of silver nitrate = concentration * volume

    n° of moles of silver nitrate = 0.10 mol/l * 0.006 l = 6 x 10⁻⁴ mol AgNO₃

    n° of moles of KCl = 0.15 mol/l * 0.005 l = 7.5 x 10⁻⁴ mol KCl

    Since 1 mol AgNO₃ reacts with 1 mol KCl, 6 x 10⁻⁴ mol AgNO₃ will react with 6 x 10⁻⁴ mol KCl and produce 6 x 10⁻⁴ mol AgCl.

    1.5 x 10⁻⁴ mol KCl is in excess.

    The molar mass of AgCl is 143.32 g/mol, then, 6 x 10⁻⁴ mol AgCl will have a mass of (6 x 10⁻⁴ mol AgCl * 143.32 g / 1 mol) 0.09 g.
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