For the sparingly soluble salts, an equilibrium is established between the undissolved solid unit and ions of the dissolved salt. For a solution of the salt like A_x B_y. A_x B_y =xA^(y+)+yB^(x-) K_(sp)=[A^(y+)]^x [B^(x-)]^y For precipitationto occur , the ionic product must be greater than K_(sp). What is the minimum concentration of OH^- ions required to precipitate Fe(OH)_3 from a 0.001 M solution of FeCl_3 (K_(sp) of Fe(OH)_3 =1xx10^(-36) )

For the sparingly soluble salts, an equilibrium is established between

1.	For the sparingly soluble salts, an equilibrium is established between the undissolved solid unit and ions of the dissolved salt. For a solution of the salt like A_x B_y. A_x B_y =xA^(y+)+yB^(x-) K_(sp)=[A^(y+)]^x [B^(x-)]^y For precipitationto occur , the ionic product must be greater than K_(sp). What is the minimum concentration of OH^- ions required to precipitate Fe(OH)_3 from a 0.001 M solution of FeCl_3 (K_(sp) of Fe(OH)_3 =1xx10^(-36) )
Answer» `1xx10^(-12)` `1xx10^(-11)` `1xx10^(-18)` `1xx10^(-16)` Solution :`K_(sp)=[Fe^(3+)][OH^-]^3` `[Fe^(3+)]=[FeCl_3]`=0.001 M `[OH^-]^3 =(1xx10^(-36))/0.001 =1xx10^(-33)` `THEREFORE [OH^-]=1xx10^(-11)`