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A solution has a [Ag+(aq)] of 0.01 M. The chloride concentration in solution is 1 x 10-5 M. Based on the following reaction, answer the following questions: AgCl(s) Ag+(aq) + Cl-(aq), Ksp = 1.7 x 10-10 Calculate the value of the current solubility product. Is the K value obtained greater or less than Ksp? Will a precipitate of AgCl form?

Respuesta :

kenmyna
 The value  of current  solubility  product  is calculated as  below

K =  (Ag+)( Cl-)

 Ag+  =  0.01 M
Cl-= 1 x10^-5M

K is therefore = 1 x10^-5 x 0.01 = 1 x10  ^ -7 M

The K obtained is greater  than  Ksp

that is    K>  KSp
 1x10^-7 >  1.7 x10 ^-10


will  precipitation  of AgCl form?

yes  the precipitation  of AgCl  will  be formed   since   K> KSP
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