if you have 55.6 grams of nitrate ions in a compound that consists of nitrate ions and plumbous ions, how many grams of the compound do you have?

how do i do this problem im completely stuck!?

Pb(NO3)2.

mols NO3^- = 55.6/molar mass NO3^- = ??
mols Pb(NO3)2 = mols NO3^- x (1 mol Pb(NO3)2/2 mols NO3^-) = ??

grams Pb(NO3)2 = mols plumbous nitrate X molar mass plumbous nitrate.

Why two postings of the same question?

You have an answer at:
http://www.jiskha.com/display.cgi?id=1228951921

thanks sorry i posted it again when i didn't get an answer for a long time

thanks again

To solve this problem, we need to understand the composition of the compound and use some basic knowledge of stoichiometry. Here's how you can approach it step by step:

1. Identify the components of the compound: In this case, we have nitrate ions (NO3-) and plumbous ions (Pb2+).

2. Determine the formula of the compound: Since plumbous ions have a 2+ charge and nitrate ions have a 1- charge, we need two nitrate ions to balance the charge. The compound's formula will be Pb(NO3)2.

3. Calculate the molar mass of nitrate ions (NO3-): Nitrate ions have a molar mass of 62.01 g/mol (14.01 g/mol for nitrogen + 3(16.00 g/mol) for three oxygen atoms).

4. Use the molar mass to convert grams of nitrate ions to moles: Divide the given weight (55.6 g) by the molar mass (62.01 g/mol):
moles of nitrate ions = 55.6 g / 62.01 g/mol

5. Apply the mole ratio to find the moles of the compound: Since we have two nitrate ions per one compound, the mole ratio is 2:1. Multiply the moles of nitrate ions by this ratio:
moles of compound = 2 * (55.6 g / 62.01 g/mol)

6. Convert moles of the compound to grams: Multiply the moles by the molar mass of the compound (formula weight):
grams of the compound = moles of the compound * molar mass of the compound

7. Calculate the final answer: To get the grams of the compound, substitute the moles of the compound into the equation:
grams of the compound = 2 * (55.6 g / 62.01 g/mol) * molar mass of the compound

By following these steps, you should be able to calculate the grams of the compound.