You could add solid KCl to the solution to precipitate out AgCl (s). What mass of KCl is needed to precipitate the silver ions from 12.0 mL of 0.160 M AgNO3 solution? Express your answer with the appropriate units.

Question

Eileen Hancock

Chemistry

4 August, 06:59

You could add solid KCl to the solution to precipitate out AgCl (s). What mass of KCl is needed to precipitate the silver ions from 12.0 mL of 0.160 M AgNO3 solution? Express your answer with the appropriate units.

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Answers (1)

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Quinn Vaughan · Answer 1

0.143 g of KCl.

Explanation:

Equation of the reaction:

AgNO3 (aq) + KCl (aq) - -> AgCl (s) + KNO3 (aq)

Molar concentration = mass/volume

= 0.16 * 0.012

= 0.00192 mol AgNO3.

By stoichiometry, 1 mole of AgNO3 reacts with 1 mole of KCl to form a precipitate.

Number of moles of KCl = 0.00192 mol.

Molar mass of KCl = 39 + 35.5

= 74.5 g/mol

Mass = molar mass * number of moles

= 74.5 * 0.00192

= 0.143 g of KCl.