defend or refute the following statements. some chemist say that the AgCL in (1) dissolves, others...

defend or refute the following statements. some chemist say that the AgCL in (1) dissolves, others say that AgCl is prevented from precipitating further by the presence of S2O3

Solutions

Expert Solution

Note that

Ag+(aq) + 2S2O3- --> [Ag(S2O3)2]3-(aq)

therefore, S2O3 will INCREASE solubility of AgCl, mainly due to the equilibrium shift:

AgCl(s) <--> Ag+(Aq) + Cl-(aq)

since Ag+ is also being used in the complex, so the shift goes from AgCl(s) towards Ag+ and Cl- production, therefore, (1) is TRUE, it is dissolving.

Others say that AgCl is prevented from precipitating if S2O3 is added

This is also true,

Since Ag+ ions are present, those will be used in the complex formation rather than in the precipitateion of AgCl

therefore, this is also true.

The thesis/arguemtn must be defended, since both are true; both regard AgCl(s) and Ag(S2O3)2-3(aq) complex formations

queen_honey_blossom answered 2 years ago

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