Silver ion is being considered as a reagent for separating I from SCN¯ in a solution that is 0.060 M in KI and 0.070 M in NaSCN. Given that the Ksps are 8.3 x 10-17 for AgI and 1.1 x 10-12 for AgSCN, answer the following. a) What Ag* concentration is needed to reduce the I- concentration to 6.0 x 10-6 M (i.e., remove 99.99% from solution)? b) What is the Ag* concentration when AgSCN begins to precipitate? c) What is the ratio of [SCN¯] to [I] when the AgSCN begins to precipitate? d) Can Ag* effectively be used to separate I and SCN- from solution? (Yes or no?) Explain your choice.

Silver ion is being considered as a reagent for separating I from SCN¯ in a solution that is 0.060 M in KI and 0.070 M in NaSCN. Given that the Ksps are 8.3 x 10-17 for AgI and 1.1 x 10-12 for AgSCN, answer the following. a) What Ag* concentration is needed to reduce the I- concentration to 6.0 x 10-6 M (i.e., remove 99.99% from solution)? b) What is the Ag* concentration when AgSCN begins to precipitate? c) What is the ratio of [SCN¯] to [I] when the AgSCN begins to precipitate? d) Can Ag* effectively be used to separate I and SCN- from solution? (Yes or no?) Explain your choice.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Calculate the following points on the titration curve for the reaction of 20.00 mL of 0.1075 M Pb4+ with 0.1250 M Cu+. The analytical reaction is Pb4+ + 2Cu+ ⇋ Pb2+ + 2Cu2+ and Pb4+ + 2e− ⇋ Pb2+ E° = 1.690 V Cu2+ + e− ⇋ Cu+ E° = 0.161 V After the addition of 17.20 mL of 0.1250 M Cu+. After the addition of 34.40 mL of 0.1250 M Cu+. What is the equilibrium constant for the reaction between Pb4+ and Cu+?
Solve question 10
At 25oC the Ksp for PbCl2 is 1.6 × 10–5. Calculate Q for the following: 125.0 mL of 0.0100 M Pb(NO3)2 is mixed with 75.0 mL of 0.0200 M NaCl at 25oC
What concentration of OH- ions is required to begin the precipitation of Cr(OH)3 from a solution containing 0.250 M Cr3+ ions? Ksp for Cr(OH)3 = 6.7 x 10-31.
P Please don't provide the handwriting solution
NaCl is added slowly to a solution that is 0.010 M each in Cu+1, Ag+1, and Au+1. Given: the Ksps: CuCl = 1.9x10-7, AgCl = 1.8x10-10, AuCl = 2.0x10-13 Which compound will precipitate first?
What [I-1] is needed to start the precipitation of AgI from a saturated solution of AgCl? Ksp = 2.9 ✕ 10-16 for AgI and Ksp = 1.2 ✕ 10-10 for AgCl. (in M)
The following concentrations are found in mixtures of ions in equilibrium with slightly soluble solids. From the concentrations given, calculate Ksp for each of the slightly soluble solids indicated: a. AgBr:[Ag*] = 5.7 × 10-7 M, [Br]= 5.7 × 10-7M b. CaCO3: [Ca²+] = 5.3 × 10-³M, [CO3²¯] = 9.0 × 10-7M c. PbF₂: [Pb²+] = 2.1 × 10-³ M, [F] = 4.2 × 10-³ M
The solubility of lead (II) iodide is found to be .00130 M What is the Ksp for PbI2?
Calculate the equilibrium concentration of Zn²+ in a solution initially with 0.150 M Zn²+ and 2.50 M CN™. The Ksp for ZnCl₂ is 3.0 x 10-16
The formation constant K; for the complex ion Zn(OH),² is 2.8 x 1015. What is the concentration of zinc ion, Zn?+, in a solution that is initially 0.35 M in Zn(OH),2 ? 2- [Zn²+] =[ M
stion 5 Calculate the molar solubility of silver carbonate, Ag2CO3, in a solution containing 0.030 M sodium carbonate, Na2C03. Ksp of Ag2CO3 = 8.1 * 10-12 О 25× 10-3 м 8.2 * 10-6 M 9,7 * 10-9 M 84 * 10-10 M 1.5 * 10-8 M