Question

Use the solubility rules to determine if:

A. NaCl will react with MgBr
B. KOH will react with Naci
C. Mgs will react with NaOH.

Answer 1

A reaction is said to occur if there is a formation of an insoluble solid or a precipitate(s) or a liquid (l) or a gas(g).

If both the reactants and products are in aqueous state, No reaction takes place.

`$2 \mathrm{NaCl}(a q)+M g B r_(2)(a q)>M g C l_(2)(a q)+2 \mathrm{NaBr}(a q)(\mathrm{NO} \text { REACTION })$`

All chlorides and Bromides are soluble except that of Ag, Hg and Pb.

Hence, No reaction takes place since all the reactants and products are in aqueous states.

`${KOH}(a q)+{NaCl}(a q)>K C l(a q)+{NaOH}(a q)(\mathrm{NO} \text { REACTION })$`

Salts of Group IA are soluble. Hence No reaction takes place

`$M g S(a q)+2 {NaOH}(a q)>M g(O H)_(2)(s)+N a_(2) S(a q)$`

(REACTION TAKES PLACE)

All hydroxides are insoluble except that of Group IA, ammonium ion and Group IIA down from Calcium.

Hence Reaction takes place with the formation of
`Mg(OH)_2` precipitate