Suppose a student mixes 5.00 mL of 2.00 x 10 M Fe(NO,), with 4.00 mL of 2.00 x 10- M KSCN and 1.00 ml of water The student then determines the [FENCS] at equilibrium to be 9.25 x 10 M. Find the equilibrium constant for the following reaction. Show all your calcula- tions for each step. Fe + SCN -FENCS Step 1. Calculate the initial number of moles of Fe" and SCN (use Equation 12). moles of Fe* 100105 moles of SCN 80410-6 S00ML o DosooL 2.00101M SCN 400ML . 000400 L 2 00 104u mol Fest •2.0010M D0osooL 1.0e10-5 mel mot sCN 0u D00400L 2.001O 8.0210.6mol

Suppose a student mixes 5.00 mL of 2.00 x 10 M Fe(NO,), with 4.00 mL of 2.00 x 10- M KSCN and 1.00 ml of water The student then determines the [FENCS] at equilibrium to be 9.25 x 10 M. Find the equilibrium constant for the following reaction. Show all your calcula- tions for each step. Fe + SCN -FENCS Step 1. Calculate the initial number of moles of Fe" and SCN (use Equation 12). moles of Fe* 100105 moles of SCN 80410-6 S00ML o DosooL 2.00101M SCN 400ML . 000400 L 2 00 104u mol Fest •2.0010M D0osooL 1.0e10-5 mel mot sCN 0u D00400L 2.001O 8.0210.6mol

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

At 22 °C, an excess amount of a generic metal hydroxide, M(OH),, is mixed with pure water. The resulting equilibrium solution has a pH of 10.18. What is the Kp of the salt at 22 °C? -12 1.4 x10 Ksp = Incorrect
Hi! All necessary information for the below question. Even if you can't finish the problem, please solve as much as you can. I'll be happy if you can at least set the question up well. Thanks!
What concentration of SO? is in equilibrium with Ag, SO, (s) and 1.00 × 10-3 M Ag+? The Ksp of Ag,SO, can be found in this table. [so; ] = M
An equilibrium reaction between chromate ions, CrO4 2- (yellow), and H+ ions is established to produce dichromate, Cr₂072- (orange). Note the colours. A student adds NaOH to a test tube containing an orange mixture of the above reagents. What is observed? 01. The solution turns from orange to yellow O 2.A precipitate forms 3. The solution tuimns from orange to colourless O4. The solution remains orange
Will a precipitate form when 20.0 mL of 1.8 x 10-3 M Pb(NO3)2 is added to 30.0 mL of 5.0 x 10-4 M Na2SO4? The Ksp of PbSO4 is 6.3x10-7. A) No because the ion product, Q<Ksp B) No because the Ksp equals the ion product C) No because the ion product, Q>Ksp D) Yes because the ion product, Q>Ksp E) Yes because the ion product, Q<Ksp
Determine the equilibrium concentration of chloride ions when solid AgCl is dissolved in 0.10 M NH3. Ksp for AgCl is 1.8 × 10-10 and the Kf for Ag(NH3)2+ is 1.7 × 107. 1.3 x 10-5 M O 5.0 × 10-8 M 5.5 x 10-2 M 5.5 x 10-3 M
Ksp = 1.50×10–14
When 12.0 mL of a 6.60×10-4 M sodium phosphate solution is combined with 15.0 mL of a 5.56×10-4 M aluminum iodide solution does a precipitate form? (yes or no) For these conditions the Reaction Quotient, Q, is equal to
Two students conducted an experiment, where they mixed 6 ml of 0.002M Fe(NO with 3 ml of 0.050 M HNO, A1 ml of 0.002 M NasCN was then added. Assuming that the equilibrium of FeSCN" concentrate is 7.96x 10 M. Determine Keg for the formation of FeSCN O 741 10-4 O 169 10-3 O 3.32 102 O 5.90 10 2 O 117 105
Using the appropriate Ksp values, find the concentration of K+ ions in the solution at equilibrium after 550 mL of 0.40 M aqueous Cu(NO3)2 solution has been mixed with 500 mL of 0.30 M aqueous KOH solution. (Enter in M.) (Ksp for Cu(OH)2 is 2.6x10-19). (Determine which reactions are taking place, and what will be precipitating from the Ksp values. Find the equilibrium concentrations of each species present. Remember, some ions are spectator ions)
3. Calculate the molar concentration of Co+ at equilibrium when 0.12 moles Co3+ is mixed with 0.98 moles NHs in 100 mL total volume of solution. Kf Co(NH3)6+ = 1.0 x 105 * Co3* + 6NH3 2 Co(NH3)63* 3.9 x 10-3 M 3.9 x 10 M O 3.0 x 10-11 M O 4.6 x 10-M
Will a precipitate form when 40.00 mL of 0.0122 M calcium nitrate solution is mixed with 60.00 mL of 0.00386 M potassium sulfate solution? (Ksp for calcium sulfate = 4.9 x 10-5)