Calculating Change in [Cl-] in 2AgNO3(aq) + CuCL2(aq) Reaction

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SUMMARY

The reaction between 2AgNO3(aq) and CuCl2(aq) produces 2AgCl(s) and Cu(NO3)2(aq). The concentration of AgNO3 at t = 30s is 0.42 mol/L, decreasing to 0.28 mol/L at t = 60s. This indicates a change in the concentration of Cl^- ions, which can be calculated based on the stoichiometry of the reaction. The decrease in AgNO3 directly correlates to the formation of AgCl, thus affecting the Cl^- concentration.

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Homework Statement



2AgNO3(aq) + CuCL2(aq) --> 2AgCl(s) + Cu(NO3)2(aq)

The concentration of Ag(NO3)2(aq) at t = 30s is .42 mol/L. At t = 60.0 its concentration is .28 mol/L. What is the change in [CL^-] during this time?

Homework Equations


The Attempt at a Solution



Not really sure even how to begin.
 
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Complex_ said:
t = 30s is .42 mol/L.
Complex_ said:
t = 60.0 its concentration is .28 mol/L.
What could change the concentration of silver nitrate?
Complex_ said:
What is the change in [CL^-]
Got any ideas?
Complex_ said:
2AgNO3(aq) + CuCL2(aq) --> 2AgCl(s) + Cu(NO3)2(aq)
This help?
 

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