Hydrated Salts question

Firstly, could you confirm that I've done this correctly:

A hydrated salt has the formula XNO3.3H20
State the negative ion in the salt: NO3-
State the positive ion in the salt: X+

If the hydrated salt has a molecule mass of 123.0g mol-1,

a) Calculate the molar mass of the an hydrous salt: 123 - (3*18) = 69g.

b) Calculate the molar mass of the metal X and use the periodic table to identify it: 69-14-(1683)=7g; making the salt Lithium.

Secondly, I'm stuck on this question:

A hydrated salt has the formula XCl2.6H20
Negative ion: Cl2-
Positive ion: X2+

Mass of hydrated salt: 5.51g
Mass of anhydrous salt: 3.01g

a) Calculate the amount, in moiled of H20 removed when sample of hydrated salt was heated: 5.51 - 3.01 = 2.5g removed; 2.5/18 = 0.138 moles

b) Construct an equation: XCL2.6H20(aq) ---heated---> 6H20(l) + XCl2(aq)

c) Deduce amount in moles of the anhydrous salt formed when the hydrated salt was heated.

d) Calculate the molar has of the anhydrous salt, and hence calcite the molar mass of X:

e) Decuce the identity of X in the formula of the hydrated salt, XCl2.6H20


The normal, black font is the question;
The bold is what I put, and what I'm unsure of - can you check it please;
The red is the questions that I'm stuck on;
The green is what I could do, but because of the other questions I cannot, due to lack of info.

Thanks.

Chloride ion is Cl^-, not Cl^2-, thus X is ²⁺

c) For every 6 moles of H₂O produced, 1 mole of anhydrous salt is produced. If 0.138 moles of H₂O is produced, how many moles of anhydrous salt is produced?

d) Mass of a. salt is 3.01 g, so use M_r = $\frac{mass}{moles}$ to work out the relative formula mass.

e) You know the mass of 1 chlorine atom, 35.5. Now use that to work out the relative mass of X.