7.00 mL of 6.00 x 103 M Fe(NO3)3 (6.00 times 10 to the minus 3rd power MFe (NO3)3) is added to 4.00 mL of 8.00 x 10³ M KSCN (8.00 times 10 to the minus 3rd power M KSCN) along with 7.00 mL of water. The concentration of [F e(SCN)2*] was found to be 1.00 x 103 M (1.00 times 10 to the minus 3rd power M) at equilibrium. How many initial moles of SCN° (SCN minus) are present in the solution? Express your answer as a decimal number (no exponents).

7.00 mL of 6.00 x 103 M Fe(NO3)3 (6.00 times 10 to the minus 3rd power MFe (NO3)3) is added to 4.00 mL of 8.00 x 10³ M KSCN (8.00 times 10 to the minus 3rd power M KSCN) along with 7.00 mL of water. The concentration of [F e(SCN)2*] was found to be 1.00 x 103 M (1.00 times 10 to the minus 3rd power M) at equilibrium. How many initial moles of SCN° (SCN minus) are present in the solution? Express your answer as a decimal number (no exponents).

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

Hello, the question is: What is the concentration of Cu2+ (aq) in the solution? The information to the question is posted below. Thank you!
The equilibrium constant for the formation of Cu(CN)42- is 2.0 x 1030. Calculate the value of pCu2+, or -log[Cu2+], if 2.21 g of CuCl2 is dissolved in 1.000 L of a 0.926 M solution by NaCN. The addition of CuCl2 does not affect the volume (the final volume is always 1,000 L).
Write the Equilibrium Expression for the Reaction of the Formation of the Complex IonFe(H2O)63+(aq) + SCN1-(aq) → [Fe(H2O)5NCS]2+(aq) + H2O(l)
Consider the series of equilibrium reactions below. In which way would you expect the reaction to “tend” at high pH? What about low pH? Why? Circle the Fe(III) species that you’d expect to be least soluble. Fe3+ + OH- <---> FeOH2+ + OH- <---> Fe(OH)2+ + OH- <---->Fe(OH)3(ferrihydrite) + OH- <--->Fe(OH)4-
solve the following parts a. Would the addition of K2SO4 to a saturated solution of CaSO4 cause the solubility to increase or decrease? Explain your answer in words not with a calculation. b. Balance the following redox reaction under basic conditions. Cr(OH)3(s) + TiO2(s)→Ti2+(aq) + CrO42-(aq)
Which metal sulfides can be precipitated from a solution that is 0.0020 M in Mn2+, 0.0030 M Zn2+, 0.00200 M Na+ and 0.0200 M Cu2+ and 0.0050 M in O2- ? Metal Sulfide Ksp MnO 4.0×102 ZnO 2.6×10-4 CuO 5.0×10-10 Na2O 1.0×10-9
Jj.49.
How many grams of (CH3)NHCI (FW 95.5) needs to be dissolved in a 0.1 Lof 0.5 M (CH3)N (Kb = 6.3 x 10-5) to achieve a buffered solution with a pH of 9? O 51.4 g O None of these are correct. O 34.7 g O 44.9 g
Calculate the pH of a buffer composed of 25 mM NaH₂PO4 (pKa = 7.21), and 20 mM Na₂HPO4 (pKa = 12.3).
What is the value of the formation constant of the complex ion formed below? Equilibrium concentrations: [M3+] = 0.025 M; [L] = 0.015 M; [ML4] = 3.5 x 10-6 M %3D M3+ (aq) + 4L (aq) ML4 (aq) Select one: A. 2.8 x 103 B. 3.6 x 10-4 C. 6.0 x 102 D. 2.8 x 103