When nitric acid is added to water the following reaction occurs.

${\mathrm{HNO}}_3+ {\mathrm{H}}_2\mathrm{O} \to {{\mathrm{NO}}_3}^{-} +{\mathrm{H}}_3{\mathrm{O}}^{+}$

Give the name and the formula of the particle transferred from nitric acid to water.

This question is about the following oxides. Aluminium oxide $\left({\mathrm{Al}}_2{\mathrm{O}}_3\right)$, Calcium oxide $\left(\mathrm{CaO}\right)$, Carbon dioxide$\left({\mathrm{CO}}_2\right)$, Carbon monoxide $\left(\mathrm{CO}\right)$, `Magnesium oxide $\left(\mathrm{MgO}\right)$, Sulphur dioxide $\left({\mathrm{SO}}_2\right)$

(i) Which will react with hydrochloric acid but not with aqueous sodium hydroxide?

Which will react with aqueous sodium hydroxide but not with hydrochloric acid? 

gt;This question is about the following oxides. Aluminium oxide $\left({\mathrm{Al}}_2{\mathrm{O}}_3\right)$, Calcium oxide $\left(\mathrm{CaO}\right)$, Carbon dioxide$\left({\mathrm{CO}}_2\right)$, Carbon monoxide $\left(\mathrm{CO}\right)$, `Magnesium oxide $\left(\mathrm{MgO}\right)$, Sulphur dioxide $\left({\mathrm{SO}}_2\right)$

(iii) Which will react both with hydrochloric acid and aqueous sodium hydroxide?

>This question is about the following oxides. Aluminium oxide $\left({\mathrm{Al}}_2{\mathrm{O}}_3\right)$, Calcium oxide $\left(\mathrm{CaO}\right)$, Carbon dioxide$\left({\mathrm{CO}}_2\right)$, Carbon monoxide $\left(\mathrm{CO}\right)$, `Magnesium oxide $\left(\mathrm{MgO}\right)$, Sulphur dioxide $\left({\mathrm{SO}}_2\right)$

(iv) Which will react neither with hydrochloric acid nor with aqueous sodium hydroxide?

Use the above data to show that the following reaction is exothermic.

$\mathrm{H}-\mathrm{H} + \mathrm{F}-\mathrm{F} \to 2\mathrm{H}-\mathrm{F}$

Hydrogen reacts with the halogens to form hydrogen halides. They react with water to form acidic solutions. 

$$\begin{gathered} \mathrm{HCl} + {\mathrm{H}}_2\mathrm{O} \leftrightarrow {\mathrm{H}}_3{\mathrm{O}}^{+} + {\mathrm{Cl}}^{-} \\ \mathrm{HF} + {\mathrm{H}}_2\mathrm{O} \leftrightarrow {\mathrm{H}}_3{\mathrm{O}}^{+} + {\mathrm{F}}^{-} \end{gathered}$$

Explain why water behaves as a base in both of these reactions.

Hydrogen reacts with the halogens to form hydrogen halides. They react with water to form acidic solutions. 

$$\begin{gathered} \mathrm{HCl} + {\mathrm{H}}_2\mathrm{O} \leftrightarrow {\mathrm{H}}_3{\mathrm{O}}^{+} + {\mathrm{Cl}}^{-} \\ \mathrm{HF} + {\mathrm{H}}_2\mathrm{O} \leftrightarrow {\mathrm{H}}_3{\mathrm{O}}^{+} + {\mathrm{F}}^{-} \end{gathered}$$

At equilibrium, only $1\%$ of the hydrogen chloride exists as molecules, the rest has formed ions. In the other equilibrium, $97\%$ of the hydrogen fluoride exists as molecules, only $3\%$ has formed ions. What does this tell you about the strength of each acid?

Hydrogen reacts with the halogens to form hydrogen halides. They react with water to form acidic solutions. 

$$\begin{gathered} \mathrm{HCl} + {\mathrm{H}}_2\mathrm{O} \leftrightarrow {\mathrm{H}}_3{\mathrm{O}}^{+} + {\mathrm{Cl}}^{-} \\ \mathrm{HF} + {\mathrm{H}}_2\mathrm{O} \leftrightarrow {\mathrm{H}}_3{\mathrm{O}}^{+} + {\mathrm{F}}^{-} \end{gathered}$$

How would the pH of these two solutions differ?