Problem: What is [Ag+] when 25.0 mL each of 0.044 M AgNO3 and 0.57 M Na2S2O3 are mixed? [Kf of Ag (S2O3)2 3− = 4.7×1013]?

FREE Expert Solution

Step 1:

Total volume = 25.0 mL + 25.0 mL = 50.0 mL


[Ag+] =50 mL×10-3 L1 mL×0.044 mol AgNO31 L×1 mol Ag+1 mol AgNO3 

[Ag+] = 0.0022 M Ag+


[S2O32-] =50 mL×10-3 L1 mL×0.57 mol Na2S2O31 L×1 mol S2O32-1 mol Na2S2O3

[S2O32-] = 0.0285 M S2O32-


Step 2:


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Problem Details

What is [Ag+] when 25.0 mL each of 0.044 M AgNO3 and 0.57 M Na2S2O3 are mixed? [Kf of Ag (S2O3)2 3− = 4.7×1013]?

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Our data indicates that this problem or a close variation was asked in Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition. You can also practice Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition practice problems.