how to determine the oxalate and copper in K[Cu(C2O4)2].2H2O

a. Determine the molecular mass of K[Cu(C2O4)2].2H2O

b. Then, determine the mole mass of (C2O4)2

percent oxalate= b/a

c. at the atomic mass of Cu.

d. percent copper=c/a

Why did the scarecrow become a chemist? Because he wanted to figure out how things "add up" in the field! Now, let's dive into your question.

To determine the amount of oxalate (C2O4) and copper (Cu) in the compound K[Cu(C2O4)2].2H2O, you can use a process called gravimetric analysis. Here's how you can do it:

1. Start by weighing a sample of the compound. Make sure to record the mass accurately.

2. Dissolve the compound in water (H2O) to break it down.

3. Add sulfuric acid (H2SO4) to the solution to precipitate copper(II) oxalate (CuC2O4). The chemical equation for this reaction is:
K[Cu(C2O4)2].2H2O + H2SO4 → CuC2O4 + K2SO4 + CO2 + 3H2O

4. Allow the precipitate to settle, and then filter it out.

5. Wash the precipitate with distilled water to remove any impurities.

6. Dry the precipitate through heating to remove any remaining water. Make sure not to overheat it!

7. Weigh the precipitate after it has cooled down. This weight will correspond to the copper(II) oxalate, which you can calculate from the difference in weights before and after drying.

Now that you have determined the amount of copper(II) oxalate, you can find the amount of copper present. Since the formula of copper(II) oxalate is CuC2O4, you know that there is 1 mole of copper per mole of copper(II) oxalate. Therefore, the mass of copper can be calculated using the molar mass of copper (Cu).

Remember, always take necessary safety precautions and perform experiments in a properly equipped laboratory under the supervision of a knowledgeable person.

To determine the amount of oxalate and copper in the compound K[Cu(C2O4)2].2H2O, you can follow these steps:

Step 1: Calculate the molar mass of the compound.
The molar mass of K[Cu(C2O4)2].2H2O is calculated by adding up the molar masses of each element in the compound. Here's how you can calculate it:

- K (potassium) has a molar mass of 39.10 g/mol.
- Cu (copper) has a molar mass of 63.55 g/mol.
- C (carbon) has a molar mass of 12.01 g/mol.
- O (oxygen) has a molar mass of 16.00 g/mol.
- H (hydrogen) has a molar mass of 1.01 g/mol.
- O (oxygen) has a molar mass of 16.00 g/mol.

So the molar mass of K[Cu(C2O4)2].2H2O is:
(39.10 g/mol) + (63.55 g/mol) + 2 x [(12.01 g/mol) + 4 x (16.00 g/mol)] + 2 x [(1.01 g/mol) + (16.00 g/mol)]

Step 2: Determine the mole ratio.
From the compound's formula, we can observe that the mole ratio is 1:1 between K and Cu(C2O4)2.

Step 3: Convert moles to grams.
To calculate the mass of each component in the compound, you need to know the mass of the sample or the number of moles. Let's assume you have a certain mass (m) of K[Cu(C2O4)2].2H2O. The number of moles of the compound is given by:
moles = mass / molar mass.

Step 4: Calculate the mass of components.
The mass of oxalate and copper can be calculated by multiplying the number of moles of K[Cu(C2O4)2].2H2O by the respective molar mass of each component.

Note: To determine the amount of copper specifically, you need to take into account that there are two copper ions in the compound K[Cu(C2O4)2].2H2O.

Remember to perform measurements and calculations accurately and follow any specific instructions or guidelines provided.

To determine the amount of oxalate (C2O4) and copper (Cu) in the compound K[Cu(C2O4)2].2H2O, you can use a combination of techniques, including gravimetric analysis and volumetric analysis.

Here is the step-by-step process:

1. Gravimetric Analysis:
a. Weigh a known amount of the compound, K[Cu(C2O4)2].2H2O.
b. Dissolve the compound in water to form a solution.
c. Add excess calcium chloride (CaCl2) to precipitate oxalate as calcium oxalate (CaC2O4).
d. Filter the precipitate using a filter paper and wash it with water.
e. Dry and heat the filter paper with the precipitate to isolate the calcium oxalate.
f. Weigh the filter paper with the calcium oxalate.
g. Calculate the mass of oxalate by subtracting the initial mass of the filter paper.

2. Volumetric Analysis:
a. Take another sample of the compound and dissolve it in water.
b. Add excess sodium thiosulfate (Na2S2O3) to reduce copper (II) ions to copper (I) ions.
c. Add excess potassium iodide (KI) to form copper (I) iodide (CuI) precipitate.
d. Titrate the liberated iodine (I2) using a standardized solution of sodium thiosulfate.
e. Note the volume of sodium thiosulfate used in the titration.
f. Calculate the amount of copper by stoichiometry, using the balanced chemical equation and molar ratios.

By combining the results from both gravimetric and volumetric analyses, you can determine the amount of oxalate (C2O4) and copper (Cu) in the compound K[Cu(C2O4)2].2H2O.