When sodium reacts with titanium chloride $\left({\mathrm{TiCl}}_4\right)$, sodium chloride $\left(\mathrm{NaCl}\right)$ and titanium $\left(\mathrm{Ti}\right)$ are produced. Construct the balanced symbol equation for the reaction.

When sodium reacts with titanium chloride $\left({\mathrm{TiCl}}_4\right)$, sodium chloride $\left(\mathrm{NaCl}\right)$ and titanium $\left(\mathrm{Ti}\right)$ are produced. Calculate the mass of titanium produced from $380 \mathrm{g}$ of titanium chloride. Give your answer to $3$ significant figures. (${\mathrm{A}}_{\mathrm{r}}$ values: $\mathrm{Ti}=47.9, \mathrm{Cl}=35.5$).

When sodium reacts with titanium chloride $\left({\mathrm{TiCl}}_4\right)$, sodium chloride $\left(\mathrm{NaCl}\right)$ and titanium $\left(\mathrm{Ti}\right)$ are produced. Calculate the mass of titanium produced using $46.0 \mathrm{g}$ of sodium. Give your answer to $3$ significant figures. (${\mathrm{A}}_{\mathrm{r}}$ value: $\mathrm{Na}=23.0$).

In this question give all answers to $3$ significant figures. The reaction between $\mathrm{NaOH}$ and $\mathrm{HCl}$ can be written as:

$\mathrm{HCl}+\mathrm{NaOH}\to \mathrm{NaCl}+{\mathrm{H}}_2\mathrm{O}$

In this reaction, $15.0 {\mathrm{cm}}^3$ of hydrochloric acid was neutralised by $20.0 {\mathrm{cm}}^3$ of $0.0500 \mathrm{mol} {\mathrm{dm}}^{-3}$ sodium hydroxide. Calculate the volume in ${\mathrm{dm}}^3$ of the acid. 

In this question give all answers to $3$ significant figures. The reaction between $\mathrm{NaOH}$ and $\mathrm{HCl}$ can be written as:

$\mathrm{HCl}+\mathrm{NaOH}\to \mathrm{NaCl}+{\mathrm{H}}_2\mathrm{O}$

In this reaction, $15.0 {\mathrm{cm}}^3$ of hydrochloric acid was neutralised by $20.0 {\mathrm{cm}}^3$ of $0.0500 \mathrm{mol} {\mathrm{dm}}^{-3}$ sodium hydroxide. Calculate the volume in ${\mathrm{dm}}^3$ of the alkali.

In this question give all answers to $3$ significant figures. The reaction between $\mathrm{NaOH}$ and $\mathrm{HCl}$ can be written as:

$\mathrm{HCl}+\mathrm{NaOH}\to \mathrm{NaCl}+{\mathrm{H}}_2\mathrm{O}$

In this reaction, $15.0 {\mathrm{cm}}^3$ of hydrochloric acid was neutralised by $20.0 {\mathrm{cm}}^3$ of $0.0500 \mathrm{mol} {\mathrm{dm}}^{-3}$ sodium hydroxide. Calculate the number of moles of alkali.

In this question give all answers to $3$ significant figures. The reaction between $\mathrm{NaOH}$ and $\mathrm{HCl}$ can be written as:

$\mathrm{HCl}+\mathrm{NaOH}\to \mathrm{NaCl}+{\mathrm{H}}_2\mathrm{O}$

In this reaction, $15.0 {\mathrm{cm}}^3$ of hydrochloric acid was neutralised by $20.0 {\mathrm{cm}}^3$ of $0.0500 \mathrm{mol} {\mathrm{dm}}^{-3}$ sodium hydroxide. Calculate the number of moles of acid then its concentration.

Give all answers to $3$ significant figures. Ammonium nitrate decomposes on heating to give nitrogen(II) oxide and water as follows:

${\mathrm{NH}}_4{\mathrm{NO}}_3\left(\mathrm{s}\right)\to {\mathrm{N}}_2\mathrm{O}\left(\mathrm{g}\right)+2{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)$

(${\mathrm{A}}_{\mathrm{r}}$ values: $\mathrm{N}=14.0, \mathrm{H}=1.0, \mathrm{O}=16.0$).

Deduce the formula mass of ammonium nitrate.

Give all answers to $3$ significant figures. Ammonium nitrate decomposes on heating to give nitrogen(II) oxide and water as follows:

${\mathrm{NH}}_4{\mathrm{NO}}_3\left(\mathrm{s}\right)\to {\mathrm{N}}_2\mathrm{O}\left(\mathrm{g}\right)+2{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)$

(${\mathrm{A}}_{\mathrm{r}}$ values: $\mathrm{N}=14.0, \mathrm{H}=1.0, \mathrm{O}=16.0$).

How many moles of ammonium nitrate are present in $0.800 \mathrm{g}$ of the solid?