# Calculating Ksp of Ag2CrO4 from Experimental Data

• Seinfeld4
In summary, the question asked for the calculation of Ksp for Ag2CrO4 based on experimental data. The experiment involved placing 1.25g of pure copper in a 1.00 L solution of silver chromate and extracting the copper, leaving 1.24g remaining. The balanced chemical equation for the reaction is Cu + Ag2CrO4 --> CuCrO4 + 2Ag. The calculated Ksp using the given data was 1.56 * 10^-11, which had a percentage error of over 1000% compared to the actual value of 1.1 * 10^-12. The approach used was to calculate the number of moles of copper, which is equal to
Seinfeld4

## 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.

Your approach looks correct and the answer seems to be consistent with the data given.

I don't like this question. I wonder how they extracted the copper. Solid left after reaction completed should weigh more, not less.

Ok, I thought I was doing it properly. I'm not sure why they made a question that produced a % error greater than 1000. Anyways, thanks Borek!

I'm currently working on this same question, lol, can you tell me if the answer to this question was marked correctly? I got the same answers with the same approach.. I know this thread is a year old ._.

I would first check the accuracy of the experimental data and the assumptions made in the calculation. It is important to ensure that the mass of pure copper used and the mass remaining after the reaction were measured accurately. Additionally, the assumption that all of the copper reacted with the silver chromate may not be completely accurate, as there could be other factors at play such as impurities or side reactions.

Assuming the experimental data is accurate, I would suggest rechecking the stoichiometry of the balanced equation. It appears that the number of moles of Ag and CrO4 used in the calculation may be incorrect. It may be helpful to double check the coefficients in the equation and make sure they are correctly accounted for in the calculation.

If the stoichiometry and experimental data are accurate, the discrepancy between the calculated and actual value could be due to experimental error or limitations of the assumptions made in the calculation. I would suggest repeating the experiment and/or using alternative methods to confirm the accuracy of the results. Additionally, it may be helpful to compare the calculated value to other published values for Ksp of Ag2CrO4 to determine the level of agreement.

In summary, as a scientist, I would recommend thoroughly checking the accuracy of the experimental data and assumptions before drawing any conclusions about the calculated Ksp value.

## 1. How do you calculate the Ksp of Ag2CrO4?

To calculate the Ksp of Ag2CrO4, you will need to use the solubility product constant equation, which is Ksp = [Ag+]^2[CrO4^-]. This equation can be derived from the balanced chemical equation for the dissolution of Ag2CrO4. You will also need to know the molar solubility of Ag2CrO4, which can be determined experimentally.

## 2. What experimental data is needed to calculate the Ksp of Ag2CrO4?

To calculate the Ksp of Ag2CrO4, you will need to know the molar solubility of Ag2CrO4 and the concentrations of Ag+ and CrO4^- ions in the solution. These concentrations can be determined using various methods such as titrations, spectrophotometry, or ion-selective electrodes.

## 3. How does temperature affect the Ksp of Ag2CrO4?

The solubility product constant, Ksp, is temperature-dependent. As the temperature increases, the Ksp of Ag2CrO4 will also increase. This is because an increase in temperature usually leads to an increase in the solubility of solids, resulting in higher concentrations of ions in solution.

## 4. What factors can affect the accuracy of the calculated Ksp of Ag2CrO4?

Several factors can affect the accuracy of the calculated Ksp of Ag2CrO4, such as experimental error, incomplete dissolution of the solid, and the presence of other ions or compounds in the solution that can interfere with the equilibrium. It is essential to carefully control and monitor these factors to obtain an accurate Ksp value.

## 5. How can the calculated Ksp of Ag2CrO4 be used in real-life applications?

The Ksp value of Ag2CrO4 can be used to predict the solubility of the compound in different solutions and conditions. This information is essential in various fields, such as environmental science, pharmaceuticals, and materials science. It can also be used to determine the purity of the compound and to troubleshoot issues in industrial processes involving Ag2CrO4.

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