Calculate the molar masses of copper (II) nitrate trihydrate and of the precipitate formed by this reaction.

Are these steps right?

Molar mass of Copper: (Cu 2+) 63.55
Molar mass of Nitrate: (NO3 -) 62.01
Copper(II) Nitrate Formula = Cu(No3)2
Molar Mass of Copper(II) Nitrate =(62.01 x 2 = 124.02) (124.02 + 63.55 = 187.57) 187.57

trihydrate: 3H2O - Molar Mass of H2O: 18.02 x 3 = 54.06

**Total Molar mass of Copper(II) Nitrate trihydrate = 241.63g

**Mass of precipitate (Cu(OH)2): 97.57g

All ok.

Yes, the steps you have followed to calculate the molar masses are correct.

To calculate the molar mass of copper(II) nitrate (Cu(NO3)2), you correctly identified the molar mass of copper (Cu2+) to be 63.55 g/mol and the molar mass of nitrate (NO3-) to be 62.01 g/mol. The formula for copper(II) nitrate is Cu(NO3)2, and you multiplied the molar mass of nitrate by 2 to account for the two nitrate ions in the compound. Then, you added the molar mass of copper to get a total molar mass of 187.57 g/mol.

To calculate the molar mass of the trihydrate form of copper(II) nitrate, you correctly identified that each molecule of water (H2O) has a molar mass of 18.02 g/mol. Since the trihydrate has three water molecules, you multiplied the molar mass of water by 3 to get a total molar mass of 54.06 g/mol for the water component. Then, you added this to the molar mass of copper(II) nitrate to get a total molar mass of 241.63 g/mol for copper(II) nitrate trihydrate.

Regarding the precipitate formed by the reaction, Cu(OH)2, you mentioned a mass of 97.57g. However, based on the information provided, it is not clear how you obtained this value. To determine the molar mass of the precipitate, you would need to know the molar mass of copper (Cu), oxygen (O), and hydrogen (H), and then sum these masses according to the formula for copper(II) hydroxide (Cu(OH)2).