FeSCN2+ becomes visible when SCN- concentration reaches approximately 10^-6 M. W

Question

FeSCN2+ becomes visible when SCN- concentration reaches approximately 10^-6 M. What is the concentration of Ag+ in solution at the end point, given that the Ksp of AgSCN is around 10^-10?

Ksp=[Ag+][SCN-]

Question is asking: If, Ksp=10^-10 and [SCN-] = 10 ^-6, what is the [Ag+]?

Experimental details (if needed but I don't think you do):

Molarity of KSCN = 0.1024 M

Titration Data and Results of Calculations: (Be sure to use the correct number of sig. figs.) Mixture 3 Mixture 2 Mixture 4 Mixture 1 Volume of 30 mL 4. bl KSCN soln used (mL) [Ag (M) O. 10 6 M LC2H302 (M) sp average Ksp: SLO

Explanation / Answer

Ksp = [Ag+][SCN-]

1 *10^-10 = [Ag+][1*10^-6]

[Ag+] = 1*10^-10/[1*10^-6] = 1*10^-4 mol/L

Related Questions

Navigate

• Browse (All)
• Browse F
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.