To solve stoichiometry problems, you must always calculate numbers of moles. Rec

Question

To solve stoichiometry problems, you must always calculate numbers of moles. Recall that molarity, M, is equal to the concentration in moles per liter: M = mol/L. When solutions of silver nitrate and potassium chloride are mixed, silver chloride precipitates out of solution according to the equation. What mass of silver chloride can be produced from 1.72 L of a 0.285 M solution of silver nitrate? Express your answer with the appropriate units. Mass AGCL = The reaction described in Part A required 3.62 L of potassium chloride. What is the concentration of this potassium chloride solution? Express your answer with the appropriate units.

Explanation / Answer

Part A

AGNO3(aq)+ KCl (aq)------> AGCl (s)+ KNO3(aq)

if 1.72 L of 0.285M solution of AgNO3 solution is used, the mass of AgCl produced will be:

number of moles of AgNO3 used= 0.285 x 1.72=0.4902 moles

from the equation, 1 mole of AgNO3 yields one mole of AgCl

hence number of moles of AgCl produced=0.4902 moles

mass= moles x molar mass

=0.4902 x 143.32

mass of AgCl=70.255 grams

part B

if KCl used=3.62 litres

from the balanced equation, 1 mole of AgNO3 requires one mole of KCl. hence number of moles of KCl required=0.4902 moles

this is the number of moles of KCl contained in 3.62 litres

concentration=moles/volume

=0.4902/3.62

concentration of KCl=0.1354 M KCl

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