Determine the number of grams of water which are required to dissolve a mixture of 25 g of KNO3 and 2.0 g of CuSo4 * 5H20 AT 100 Degrees celscius?

Is that the solubility at 100 C? I assume it is. Then KNO3 will require

100g H2O x (25/245) = about 10 g H2O (but you need to do it more accurately).
CuSO4.5H2O will require
100 g x (2/180) = about 1 gram H2O.
Generally, one does not add the masses of the water. Generally, the more soluble salt (in this case KNO3) will take about 10 g H2O to dissolve it AND the solution will have enough room to dissolve the smaller amount of CuSO4.5H2O also.

We need the solubility numbers for KNO3 and CuSO4.5H2O. YOu must have them in a table, either in your text, notes, or in the problem. (Note the correct spelling of celsius.)

So, the soulubility for Kno3 IS 245 of 100 grams in water. The solubility for CuSo4 is 180 grams over 100 grams of water. How would you solve that?

To determine the number of grams of water required to dissolve the mixture of KNO3 and CuSO4 * 5H2O at 100 degrees Celsius, we need to calculate the total mass of the mixture that would dissolve in water.

1. Start by finding the molar masses of KNO3 and CuSO4 * 5H2O:
- Molar mass of KNO3 (potassium nitrate) = molar mass of K (potassium) + molar mass of N (nitrogen) + 3 * molar mass of O (oxygen)
- Molar mass of K = 39.10 g/mol
- Molar mass of N = 14.01 g/mol
- Molar mass of O = 16.00 g/mol
Thus, molar mass of KNO3 = 39.10 + 14.01 + 3 * 16.00 = 101.10 g/mol.

- Molar mass of CuSO4 * 5H2O (copper(II) sulfate pentahydrate) = molar mass of Cu (copper) + molar mass of S (sulfur) + 4 * molar mass of O (oxygen) + 5 * (molar mass of H (hydrogen) + molar mass of O)
- Molar mass of Cu = 63.55 g/mol
- Molar mass of S = 32.07 g/mol
- Molar mass of O = 16.00 g/mol
- Molar mass of H = 1.01 g/mol
Thus, molar mass of CuSO4 * 5H2O = 63.55 + 32.07 + 4 * 16.00 + 5 * (1.01 + 16.00) = 249.69 g/mol.

2. Calculate the number of moles for each substance in the mixture:
- Moles of KNO3 = mass of KNO3 / molar mass of KNO3
- Moles of CuSO4 * 5H2O = mass of CuSO4 * 5H2O / molar mass of CuSO4 * 5H2O

Given:
- Mass of KNO3 = 25 g
- Mass of CuSO4 * 5H2O = 2.0 g

Moles of KNO3 = 25 g / 101.10 g/mol
Moles of CuSO4 * 5H2O = 2.0 g / 249.69 g/mol

3. Determine the substance that limits the amount of water required for dissolution:
- Compare the moles of KNO3 and CuSO4 * 5H2O. The substance with fewer moles is the limiting substance.

4. Calculate the number of moles of water required to dissolve the limiting substance:
- In this case, we assume that both KNO3 and CuSO4 * 5H2O dissolve completely in water without any excess. This means that the molar ratio of water to the limiting substance is determined by the chemical formula.
- Since there are no water molecules in the formula of KNO3, we only consider the formula of CuSO4 * 5H2O to determine the number of moles of water.
- CuSO4 * 5H2O contains 5 moles of water per 1 mole of CuSO4 * 5H2O.

Moles of water = Moles of CuSO4 * 5H2O * 5

5. Calculate the mass of water required:
- Mass of water = Moles of water * molar mass of water

Molar mass of water = 2 * (1.01 g/mol) + 16.00 g/mol = 18.02 g/mol

Mass of water = Moles of water * molar mass of water

After following these steps, you should be able to determine the number of grams of water required to dissolve the given mixture at 100 degrees Celsius.