The formula for epsom salt is MgSO4 . 7H20 If 1.250 g of the compound is dissolved in water, calculate the number of milliliters of .200 M Ba(NO3)2 that would be required to precipitate all of the sulfate ions as barium sulfate.

Do it for 1.000 g of alum, which is AlK(SO4)2 .12H2O.

I already did part one. please help me for part 2

I did that for someone. Let me look and find the post. I'll post it here.

http://www.jiskha.com/display.cgi?id=1286736675

To calculate the number of milliliters of 0.200 M Ba(NO3)2 required to precipitate all sulfate ions from 1.000 g of alum (AlK(SO4)2 . 12H2O), you need to follow a series of steps:

Step 1: Determine the molar mass of alum (AlK(SO4)2 . 12H2O)
The molar mass of AlK(SO4)2 . 12H2O can be calculated by summing the atomic masses of each element present in the compound:
Molar mass = (1 * atomic mass of Al) + (1 * atomic mass of K) + (2 * atomic mass of S) + (8 * atomic mass of O) + (24 * atomic mass of H2O)

Step 2: Convert the mass of alum to moles
Using the molar mass from Step 1, convert the mass of alum (1.000 g) to moles by dividing it by the molar mass.

Step 3: Calculate the number of moles of sulfate ions in alum
Since each mole of alum contains two moles of sulfate ions (SO4), multiply the number of moles of alum from Step 2 by 2 to obtain the number of moles of sulfate ions.

Step 4: Use stoichiometry to determine the amount of Ba(NO3)2 required
Based on the balanced chemical equation for the reaction between sulfate ions and Ba(NO3)2, we know that the stoichiometric ratio is 1:1. This means that one mole of sulfate ions requires one mole of Ba(NO3)2. Therefore, the amount of Ba(NO3)2 required in moles is equal to the number of moles of sulfate ions.

Step 5: Convert moles of Ba(NO3)2 to milliliters using the given concentration
Using the given concentration of 0.200 M in Ba(NO3)2, convert the number of moles from Step 4 to milliliters by dividing it by the molar concentration.

Follow these steps to determine the number of milliliters of 0.200 M Ba(NO3)2 required to precipitate all sulfate ions from 1.000 g of alum.

To calculate the number of milliliters of 0.200 M Ba(NO3)2 required to precipitate all of the sulfate ions in 1.000 g of alum (AlK(SO4)2.12H2O), you'll need to follow these steps:

1. Determine the molar mass of alum:
- Molar mass of AlK(SO4)2 = (1 x molar mass of Al) + (1 x molar mass of K) + (2 x molar mass of S) + (8 x molar mass of O) + (24 x molar mass of H2O)
- To find the molar mass of AlK(SO4)2, you'll need to add up the individual molar masses of each element. You can find the atomic masses on the periodic table.
- Substitute the values and calculate the molar mass.

2. Calculate the number of moles of alum (AlK(SO4)2):
- Number of moles = mass / molar mass
- Substitute the mass of the alum (1.000 g) and its molar mass to calculate the number of moles.

3. Determine the ratio between sulfate ions and barium sulfate:
- In the balanced chemical equation, the ratio between sulfate ions (SO4^2-) and barium sulfate (BaSO4) is 1:1.
- This means that for every mole of alum you have, you need one mole of barium sulfate.

4. Calculate the number of moles of barium sulfate needed:
- Since the ratio of sulfate ions to barium sulfate is 1:1, the number of moles of barium sulfate is equal to the number of moles of alum calculated in step 2.

5. Determine the volume of 0.200 M Ba(NO3)2 solution required:
- The Molarity (M) of a solution is defined as moles of solute per liter of solution.
- Rearrange the equation to calculate the volume:
- Volume (in liters) = moles of solute / Molarity
- Substitute the number of moles of barium sulfate calculated in step 4 and the Molarity of Ba(NO3)2 (0.200 M) to calculate the volume.

6. Convert the volume from liters to milliliters:
- Since the density of water is 1 g/mL, 1 mL is equal to 1 cm³.
- Multiply the volume in liters by 1000 to convert it to milliliters.

Follow these steps to calculate the number of milliliters of 0.200 M Ba(NO3)2 required to precipitate all of the sulfate ions in 1.000 g of alum.