Question

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

(a)Na2S + HCl -> H2S + 2NaCl
(b)2Na + 2HCl -> H2 + 2NaCl
(c)Mg + Cl2 = MgCl2
(d)MgO + 2HCl = H2O + MgCl2
(e)K3P+2O2 -> K3PO4
(f)3KOH +H3PO4 -> K3PO4 + 3H2O

Answer 1

Step-by-step 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.