Question

Classify the following as acid-Base reactions or oxidation-reduction reactions:

Answer 1

Explanation:

(a) $Na_2S+HCl\rightarrow H_2S+2NaCl$

This is acid base reaction because there is no change of oxidation state on either side of the reaction.

(b) $2Na+2HCl\rightarrow H_2+2NaCl$

This is a oxidation reduction reaction because sodium in elemental state ( 0 oxidation state) oxidizes to Na⁺ in NaCl. Also H⁺ in HCl reduces to H° in H₂.

(c) $Mg+Cl_2\rightarrow MgCl_2$

This is a oxidation reduction reaction because magnesium in elemental state ( 0 oxidation state) oxidizes to Mg²⁺ in MgCl₂. Also Cl° in Cl₂ reduces to Cl⁻ in  MgCl₂.

(d) $MgO+2HCl\rightarrow H_2O+MgCl_2$

This is acid base reaction because there is no change of oxidation state on either side of the reaction.

(e) $K_3P+2O_2\rightarrow K_3PO_4$

This is a oxidation reduction reaction because phosphorous in P³⁻ in K₃P oxidizes to P⁵⁺ in K₃PO₄ and oxygen reduces.

(f) $3KOH+H_3PO_4\rightarrow K_3PO_4 + 3H_2O$

This is acid base reaction because there is no change of oxidation state on either side of the reaction.