Question

Peroxodisulfate on hydrolysis yields:
A. water
B. dihydrogen
C. hydrogen peroxide
D. deuterium

Answer 1

Hint: We need to know that the chemical formula of peroxydisulfate ion is ${S_2}{O_8}^{2 - }$ which an oxyanion is. Peroxodisulfate can also refer to as the persulfate ion or peroxodisulfate anions. We can also refer this term as peroxymonosulfate ion i.e. $S{O_5}^{2 - }$ .

Complete answer:
We know that the salts of peroxydisulfate are mainly used to initiate the polymerization of various alkenes which include styrene, acrylonitrile, and fluoroalkenes. When polymerization reaction is initiated by the homolysis of the peroxydisulfate then the reaction is:
${[{O_3}SO - OS{O_3}]^{2 - }} \rightleftharpoons 2{[S{O_4}]^ - }$
Approximately 500,000 tons of salts containing this anion are produced annually. Important salts include sodium persulfate $(N{a_2}{S_2}{O_8})$ , potassium persulfate $({K_2}{S_2}{O_8})$, and ammonium persulfate $({(N{H_4})_2}{S_2}{O_8})$.These salts are colorless, water-soluble solids that are strong oxidants.
On hydrolysis, Peroxodisulfate yields hydrogen peroxide (option C).
$H{O_3}SO - OS{O_3}H(aq) + 2{H_2}O(l)\xrightarrow{{hydrolysis}}2HS{O_4}^ - (aq) + 2{H^ + }(aq) + {H_2}S{O_2}(aq)$
Moreover, we also know that sodium peroxydisulfate can be used for water and wastewater treatment, soil and groundwater remediation, and etching of copper on circuit boards. Also, it can be used to produce hair lighteners and bleaches, medical drugs, cellophane, rubber, soaps, detergents, adhesive papers, dyes for textiles, and in photography.
In addition to the major commercial applications, peroxydisulfate participates in reactions of interest in the laboratory:
-Elbs persulfate oxidation
-Oxidation of $A{g^ + }toA{g^{2 + }}$
And hence option C is correct.

Note:
We also need to note that we can prepare hydrogen peroxide from sodium peroxide. When Sodium peroxide is gradually added to an ice-cold solution of 20% ${H_2}S{O_4}$ it yields hydrogen peroxide.
$N{a_2}{O_2} + {H_2}S{O_4} \to N{a_2}S{O_4} + {H_2}{O_2}$
After that we can also prepare Barium peroxide:
(a) By the action of dilute sulfuric acid:
$Ba{O_2}.8{H_2}O(s) + {H_2}S{O_4}(aq) \to BaS{O_4}(s) + {H_2}{O_2}(aq) + 8{H_2}O(l)$
(b) By the action of carbon dioxide:
$Ba{O_2} + {H_2}O + C{O_2} \to BaC{O_3} + {H_2}{O_2}$
(c) By the action of phosphoric acid:
$3Ba{O_2} + 2{H_3}P{O_4} \to B{a_3}{(P{O_4})_2} + 3{H_2}{O_2}$ .