I am confused on these specific parts of the problem: 1b(ii), 1e(i), and 1e(ii)
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Everything else makes sense, but I do not know how I would be able to determine the formula for the hydrate, along with the percent by mass (in this scenario).

Thank you!
Ansam

For 1 C
Subtract the mass of hydrated salt(MgCl₂.nH₂O) from the anhydrous salt (MgCl₂) which is obtained after strong heating as water vaporizes as gas.
Use that mass as mass of water and convert it to moles of water.
For 1 e part
First write the balanced equation
2AgNO₃ (aq) + MgCl₂ (aq)---> Mg(NO₃ )₂ (aq)+ 2AgCl (s)

Now start with mass of AgCl formed as precipitate convert it to moles of AgCl and convert it to moles of MgCl₂


For 1e(ii) convert moles of MgCl₂ to grams of MgCl₂ and to calculate percent by mass of MgCl₂
(Mass of MgCl2 obtained in above calculation / mass of sample in the starting of the experiment) x100 %


To determine the moles of water  in 1 mole of MgCl2 you need to do some mathematics on the data you collected here
Like you have moles of water from 1b(i) and moles of MgCl2 form 1e(i)
Moles of water /moles of MgCl₂ will give you moles of water per mole of MgCl₂ .