What is the approximate concentration of free Cu* ion at equilibriumwhen 1.20x10-² mol copper(I) nitrate is added to 1.00 L of solutionthat is 1.270 M in CN. For [Cu(CN)₂]¯, Kƒ = 1.0×10²4.[Cut] =M The solubility of AgBr in water is 5.74x10-7 M, but increases in the presence of thiosulfate ion. Calculate thesolubility of AgBr when the solid is added to a solution that is 0.535 M in thiosulfate ion. For AgBr, Ksp3.30x10-13 and for Ag (S₂03)2³-, Kf = 2.00×10¹³.Solubility=M=

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What is the approximate concentration of free Cu* ion at equilibrium when 1.20×10-² mol copper(I) nitrate is added to 1.00 L of solution that is 1.270 M in CN™. For [Cu(CN)₂]¯, Kf = 1.0×10²4. [Cut] = = M

What is the approximate concentration of free Cu* ion at equilibrium when 1.20×10-² mol copper(I) nitrate is added to 1.00 L of solution that is 1.270 M in CN™. For [Cu(CN)₂]¯, Kf = 1.0×10²4. [Cut] = = M

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Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

What is the approximate concentration of free Cu* ion at equilibrium
when 1.20x10-² mol copper(I) nitrate is added to 1.00 L of solution
that is 1.270 M in CN. For [Cu(CN)₂]¯, Kƒ = 1.0×10²4.
[Cut] =
M

The solubility of AgBr in water is 5.74x10-7 M, but increases in the presence of thiosulfate ion. Calculate the
solubility of AgBr when the solid is added to a solution that is 0.535 M in thiosulfate ion. For AgBr, Ksp
3.30x10-13 and for Ag (S₂03)2³-, Kf = 2.00×10¹³.
Solubility
=
M
=

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