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Question: The solubility of Fe(OH)3 in an aqueous solution was determine to be 4.5*10^-10 mol/L. What is the vaule of the Ksp for Fe(OH)3?
so i got the part of :
Fe(OH)3(s) <---> Fe^3+ (aq) + 3OH^- (aq)
Ksp= [Fe^3+][OH^-]^3
i dont get this part here how they got [OH^-]= 3[Fe^3+] where is this coming from
then it comes out to
Can someone please show me how to work out this calculation without a freaking calculator?
Ksp=[Fe^3+](3[Fe^3+])^3=27[Fe^3+]^4
Ksp= (4.5*10^-10)[3(4.5*10^-10)]^3=27(4.5*10^-10)^4
Ksp= ?
and this problem please the calculations:
Question: What are the concentrations of each of the ions in a saturated solution of PbBr2, given that the Ksp of PbBr2 is 2.1*10^-6? If 5 g of PbBr2 are dissolved in water to make 1L of solution and this is then brought to 25degrees C, would the solution be saturated, unsaturated, or supersaturated?
please work this out for me........
so i got the part of :
Fe(OH)3(s) <---> Fe^3+ (aq) + 3OH^- (aq)
Ksp= [Fe^3+][OH^-]^3
i dont get this part here how they got [OH^-]= 3[Fe^3+] where is this coming from
then it comes out to
Can someone please show me how to work out this calculation without a freaking calculator?
Ksp=[Fe^3+](3[Fe^3+])^3=27[Fe^3+]^4
Ksp= (4.5*10^-10)[3(4.5*10^-10)]^3=27(4.5*10^-10)^4
Ksp= ?
and this problem please the calculations:
Question: What are the concentrations of each of the ions in a saturated solution of PbBr2, given that the Ksp of PbBr2 is 2.1*10^-6? If 5 g of PbBr2 are dissolved in water to make 1L of solution and this is then brought to 25degrees C, would the solution be saturated, unsaturated, or supersaturated?
please work this out for me........