Identify each of the following as an acid or a base; (10.1)

A. $\mathrm{Sr}(\mathrm{OH}{)}_2$$\mathrm{Sr}(\mathrm{OH}{)}_2$

B. ${\mathrm{H}}_2{\mathrm{SO}}_3$

C.${\mathrm{HC}}_2{\mathrm{H}}_3{\mathrm{O}}_2$

D.$\mathrm{CsOH}$

A base, according to the Arrhenius hypothesis, is a chemical that produces a metal ion and hydroxide ions in an aqueous solution$\left({\mathrm{OH}}^{-}\right)$.The following equation represents the combination of $\mathrm{Sr}(\mathrm{OH}{)}_2$with water:

localid="1652608648142" $\mathrm{Sr}\left(\mathrm{OH}{)}_2\right(s\left)\stackrel{{\mathrm{H}}_2\mathrm{O}}{⟶}{\mathrm{Sr}}^{2+}\right(aq)+2{\mathrm{OH}}^{-}(aq)$

$\begin{array}{lcc}\text{Strontium}& \text{Strontium}& \text{Hydroxide}\\ \text{hydroxide}& \text{ion}& \text{ion}\end{array}$

Consequently, $\mathrm{Sr}(\mathrm{OH}{)}_2$is a base

An acid, and according to Arrhenius theory, is indeed a chemical that creates hydrogen ions in either an aqueous solution $\left({\mathrm{H}}^{+}\right)$. The combination between ${\mathrm{H}}_2$and ${\mathrm{SO}}_4$ and water has been represented as follows:

${\mathrm{H}}_2{\mathrm{SO}}_3\left(aq\right)+2{\mathrm{H}}_2\mathrm{O}\left(l\right)\rightleftarrows {\mathrm{SO}}_3^{2-}\left(aq\right)+2{\mathrm{H}}_3{\mathrm{O}}^{+}\left(aq\right)$

localid="1652608666937" $\begin{array}{cccc}\text{Sulfurous}& \text{Water}& \text{Sulfite ion}& \text{Hydronium}\\ \text{acid}& & \text{ion}& \end{array}$

A single proton $\left({\mathrm{H}}^{+}\right)$does not exist in water; however, it quickly reacts with it to generate the hydronium ion $\left({\mathrm{H}}_3{\mathrm{O}}^{+}\right)$.

As a result, ${\mathrm{H}}_2{\mathrm{SO}}_3$is an acid.

An acid, according to the Arrhenius theory, would be a molecule capable releases hydrogen ions in an aqueous solution $\left({\mathrm{H}}^{+}\right)$The reaction among both ${\mathrm{HC}}_2{\mathrm{H}}_3{\mathrm{O}}_2$and oxygen is expressed in the form:

localid="1652608692233" ${\mathrm{HC}}_2{\mathrm{H}}_3{\mathrm{O}}_2\left(aq\right)+{\mathrm{H}}_2\mathrm{O}\left(l\right)\rightleftarrows {\mathrm{C}}_2{\mathrm{H}}_3{\mathrm{O}}_2^{-}\left(aq\right)+{\mathrm{H}}_3{\mathrm{O}}^{+}\left(aq\right)$

localid="1652608697746" $AceticacidWaterAcetateionHydroniumion$

A molecular proton $\left({\mathrm{H}}^{+}\right)$does not exist in water; however, it quickly reacts with it to generate the hydronium ion $\left({\mathrm{H}}_3{\mathrm{O}}^{+}\right)$

As a consequence, ${\mathrm{HC}}_2{\mathrm{H}}_3{\mathrm{O}}_2$is indeed an acidic.

A bases, as per the Arrhenius theory, seems to be a substance that generates a metal ion and hydroxide ions in such an aqueous solution $\left({\mathrm{OH}}^{-}\right)$. This same following equation reflects the interaction of $\mathrm{CsOH}$ using water:

localid="1652608748534" $\mathrm{CsOH}\left(s\right)\stackrel{{\mathrm{H}}_2\mathrm{O}}{⟶}{\mathrm{Cs}}^{+}\left(aq\right)+{\mathrm{OH}}^{-}\left(aq\right)$

$\begin{array}{l}\text{Cesium}\hspace{0.25em}\hspace{0.25em}\hspace{0.25em}\hspace{0.25em}\text{Cesium}\hspace{0.25em}\hspace{0.25em}\hspace{0.25em}\hspace{0.25em}\text{Hydroxide}\\ \text{hydroxide}\hspace{0.25em}\hspace{0.25em}\hspace{0.25em}\hspace{0.25em}\text{ion}\hspace{0.25em}\hspace{0.25em}\hspace{0.25em}\hspace{0.25em}\text{ion}\end{array}$

As a conclusion, CsOH is a base.