$27 \mathrm{g}$ of aluminium burns in chlorine to form $133.5 \mathrm{g}$ of aluminium chloride. $\left[{\mathrm{A}}_{\mathrm{r}}: \mathrm{Al}=27, \mathrm{Cl}=35.5\right]$

How many moles of aluminium atoms are present in $27 \mathrm{g}$ of aluminium?

Find the simplest formula of aluminium chloride.

$1 {\mathrm{dm}}^3$ of an aqueous solution is made using $13.35 \mathrm{g}$ of aluminium chloride. What is its concentration in moles per ${\mathrm{dm}}^3$?

You have to prepare some $2 \mathrm{M}$ solutions, with $10 \mathrm{g}$ of solute. What volume of solution will you prepare, for the following solute? $\left[{\mathrm{A}}_{\mathrm{r}}: \mathrm{H}=1, \mathrm{Li}=7, \mathrm{N}=14, \mathrm{O}=16, \mathrm{Mg}=24, \mathrm{S}=32\right]$

• Lithium sulfate $\left({\mathrm{Li}}_2{\mathrm{SO}}_4\right)$

You have to prepare some $2 \mathrm{M}$ solutions, with $10 \mathrm{g}$ of solute. What volume of solution will you prepare, for the following solute? $\left[{\mathrm{A}}_{\mathrm{r}}: \mathrm{H}=1, \mathrm{Li}=7, \mathrm{N}=14, \mathrm{O}=16, \mathrm{Mg}=24, \mathrm{S}=32\right]$

• Magnesium sulfate $\left({\mathrm{MgSO}}_4\right)$

You have to prepare some $2 \mathrm{M}$ solutions, with $10 \mathrm{g}$ of solute. What volume of solution will you prepare, for the following solute? $\left[{\mathrm{A}}_{\mathrm{r}}: \mathrm{H}=1, \mathrm{Li}=7, \mathrm{N}=14, \mathrm{O}=16, \mathrm{Mg}=24, \mathrm{S}=32\right]$

• Ammonium nitrate $\left({\mathrm{NH}}_4{\mathrm{NO}}_3\right)$