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## Homework Statement

Hi,

I need to calculate the Ksp of Ag2CrO4 based on experimental data.

During the experiment, 1.25g of pure copper was placed in a 1.00 L solution of silver chromate. When the copper was extracted, only 1.24g remained.

Balanced chemical equation: Cu + Ag2CrO4 --> CuCrO4 + 2Ag

## The Attempt at a Solution

Here's what I did:

mole of copper = 0.01g / 63.546

= 1.57 * 10^-4

Since volume is 1.00 L, the number of moles is equal to the concentration.

There are 2 moles of Ag and 1 mole of CrO4 for every mole of copper, so:

Ksp = (1.57 * 10^-4) (3.15 * 10^-4) (3.15 * 10^-4)

= 1.56 * 10^-11

But this doesn't seem correct because the actual value is 1.1 * 10^-12.

This would give me a percentage error of over 1000%...

Any help would be much appreciated.