Data starts here. Solution 1: 3 mL of CuSO4 and 1 mL H2O Solution 2: 2 mL of CuS

Question

Data starts here.

Solution 1: 3 mL of CuSO4 and 1 mL H2O

Solution 2: 2 mL of CuSO4 and 3 mL H2O

Solution 3: 2 mL of CuSO4 and 8 mL H2O

Solution 1: 2 mL of CuSO4 and 13 mL H2O

Absorbance (635 nm) for solution 1: 0.194

Absorbance (635 nm) for solution 2: 0.104

Absorbance (635 nm) for solution 3: 0.050

Absorbance (635 nm) for solution 4: 0.025

Absorbance from fitrate a (done in lab): .086

Absorbance from fitrate a (done in lab): .017

Absorbance from fitrate a (done in lab): .009

Absorbance from fitrate a (done in lab): .040

[Cu2+] in solution 1: 0.15 M

[Cu2+] in solution 2: 0.08 M

[Cu2+] in solution 3: 0.04 M

[Cu2+] in solution 4: 0.03 M

CuC4H4O6 (s) <--> Cu2+ (aq) + C4H4O62- (aq)

A = m * [Cu2+] + (y-intercept) and

A = 1.33 * [Cu2+] - 00.51

[Cu2+] in filtrate a: 0.065

[Cu2+] in filtrate b: 0.013

[Cu2+] in filtrate c: 0.0068

[Cu2+] in filtrate d: 0.030

Data ends here.

Question #1a

Calculate Ksp in filtrate a:

Calculate Ksp in filtrate b:

Question #1b

Calculate molar solubility in filtrate a:

Calculate molar solubility in filtrate b:

Calculate molar solubility in filtrate c:

Calculate molar solubility in filtrate d:

Explanation / Answer

That answer is wrong.

moles does not equal concentration/volume.

the number of moles is equal to concentration(mol/L) X volume (L); L cancel out leaving you with the number of moles.

concentration is equal to the number of moles per liter. therefore that c=n*v is wrong also

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