Question

Use the following data. A. Mass of crucible: 12.214 g B. Mass of crucible and hydrate: 13.250 g C. Mass of crucible and anhydrous salt: 12.885 g Note: We are using CuSO$_4$ instead of MgSO$_4$. Calculate the molar mass of CuSO$_4$ and write its value here: 159.61 g/mol. Mass of anhydrous salt: $12.214g + x = 12.885g = 0.671$ Moles of anhydrous salt: $4.20 \times 10^{-3}$ mol Mass of water lost: $1.036 - 0.671 = 0.365$ Molar mass of water: 18.02 g/mol Moles of water: 0.02026 mol Divide the moles of water by the moles of anhydrous salt to find n, the moles of water per mole anhydrous salt. n = 4.82 The empirical formula for our hydrate is CuSO$_4$ \cdot n H$_2$O, where n is the number you just found. Record the empirical formula for the copper(II) sulfate hydrate below. Formula of hydrate:

          Use the following data.
A. Mass of crucible: 12.214 g
B. Mass of crucible and hydrate: 13.250 g
C. Mass of crucible and anhydrous salt: 12.885 g
Note: We are using CuSO$_4$ instead of MgSO$_4$.
Calculate the molar mass of CuSO$_4$ and write its value here: 159.61 g/mol.
Mass of anhydrous salt: $12.214g + x = 12.885g = 0.671$
Moles of anhydrous salt: $4.20 \times 10^{-3}$ mol
Mass of water lost: $1.036 - 0.671 = 0.365$
Molar mass of water: 18.02 g/mol
Moles of water: 0.02026 mol
Divide the moles of water by the moles of anhydrous salt to find n, the moles of water per mole anhydrous salt.
n = 4.82
The empirical formula for our hydrate is CuSO$_4$ \cdot n H$_2$O, where n is the number you just found.
Record the empirical formula for the copper(II) sulfate hydrate below.
Formula of hydrate:

Use the following data.
A. Mass of crucible: 12.214 g
B. Mass of crucible and hydrate: 13.250 g
C. Mass of crucible and anhydrous salt: 12.885 g
Note: We are using CuSO4 instead of MgSO4.
Calculate the molar mass of CuSO4 and write its value here: 159.61 g/mol.
Mass of anhydrous salt: 12.214g + x = 12.885g = 0.671
Moles of anhydrous salt: 4.20 × 10^-3 mol
Mass of water lost: 1.036 - 0.671 = 0.365
Molar mass of water: 18.02 g/mol
Moles of water: 0.02026 mol
Divide the moles of water by the moles of anhydrous salt to find n, the moles of water per mole anhydrous salt.
n = 4.82
The empirical formula for our hydrate is CuSO4 ·n H2O, where n is the number you just found.
Record the empirical formula for the copper(II) sulfate hydrate below.
Formula of hydrate:

Added by Michael J.

Question

Please give Ace some feedback