When a 2.00 g sample of Al2(SO4)3·xH2O is heated to remove all water, a mass of 1.03 g remains. Determine the value of x.
To determine the value of x, we need to calculate the amount of water lost during heating.
First, we need to find the mass of water in the original sample. We know that the mass of the sample before heating is 2.00 g, and the mass of the remaining sample after heating is 1.03 g.
The mass of water lost can be calculated by subtracting the mass of the remaining sample from the mass of the original sample:
Mass of water lost = Mass of original sample - Mass of remaining sample
Mass of water lost = 2.00 g - 1.03 g
Mass of water lost = 0.97 g
Next, we need to convert the mass of water lost to moles using the molar mass of water. The molar mass of water is approximately 18.015 g/mol.
Number of moles of water lost = Mass of water lost / Molar mass of water
Number of moles of water lost = 0.97 g / 18.015 g/mol
Now, let's determine the molar mass of Al2(SO4)3. The atomic masses of aluminum (Al), sulfur (S), and oxygen (O) are 26.98 g/mol, 32.06 g/mol, and 16.00 g/mol respectively.
Molar mass of Al2(SO4)3 = (2 * atomic mass of Al) + (3 * atomic mass of S) + (12 * atomic mass of O)
Molar mass of Al2(SO4)3 = (2 * 26.98 g/mol) + (3 * 32.06 g/mol) + (12 * 16.00 g/mol)
Finally, we can determine the value of x by equating the number of moles of water lost to the number of moles of water in the chemical formula.
Since there are x moles of water in Al2(SO4)3·xH2O:
Number of moles of water lost = x * Number of moles of water in Al2(SO4)3
0.97 g / 18.015 g/mol = x * (18.015 g/mol / Molar mass of Al2(SO4)3)
Simplifying the equation, we find:
x = (0.97 g / 18.015 g/mol) * (Molar mass of Al2(SO4)3 / 18.015 g/mol)
By substituting the molar mass value of Al2(SO4)3 and performing the calculation, you will be able to determine the value of x.