Suppose 50.00 mL of 2.0 x 10^-6 M Fe(NO3)3 is added to 50.00 mL of 2.0 x 10^-4 M KIO3.
Which of the following statements is true? For Fe(IO3)3, ksp = 1.0 x 10^-4
a) A precipitate forms because Qc > Ksp
b) A precipitate forms because Qc < Ksp
c) No precipitate forms because Qc < Ksp
d) No precipitate forms because Qc = Ksp
3) No precipitate forms because Qc > Ksp
Can you guys explain your thought process so I can understand the problem?
- harboughLv 44 years ago
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- 8 years ago
1)Write chemical equation
Fe(NO3)3 +KIO3 -->Fe(IO3)3 + KNO3
[IO3] = (50mL)(2.0x10^-4M) / 100mL =1.0x10^-4 M
[Fe^3+]= (50mL)(2.0x10^-6M)/100mL = 1.0 x10^-6 M
Fe(IO3)s <----> Fe^3+(aq) +(IO3)-(aq)
Q=(1.0x10^-4)(1.0x10^-6) = 1.0 x10^-10
Ksp for Fe(IO3)3 is 1.0x10^-4. Notice that Q is smaller than Ksp, so the solution is unsaturated in Fe(IO3)3 and a precipate will not form.
answer is CSource(s): chemistry student