I just need help with the [SBO+ ], I can'tfigure out what I did wrong. Please helpA buffered solution of 0.0340 M SbO* and 0.0180 M Cď²+ was prepared with a pH of 2.15 at 25 °C.Eso. = 0.208 VEe. = -0.402 VSbo* + 2H* + 3e"= Sb(s) + H,OCd2+ + 2e- = Cd(s)Which ion is more easily reduced?Sbo*O Ca²+What is the concentration of SbO* at the potential when Cd2+ will begin to be deposited?[SbO*] = 0.396IncorrectDetermine the potential at the cathode when the SbO* concentration is 0.0015 M?Ecathode =0.0674V

Since only second part is asked, thus solution of second part is being provided. Calculation of…

I just need help with the [SBO+ ], I can't figure out what I did wrong. Please help A buffered solution of 0.0340 M SbO* and 0.0180 M Cď²+ was prepared with a pH of 2.15 at 25 °C. Eso: = 0.208 V E. = -0.402 V Sbo* + 2H* +3e= Sb(s) + H,O Ca2+ + 2e = Cd(s) Which ion is more easily reduced? Sbo* What is the concentration of SbO* at the potential when Cd²+ will begin to be deposited? [SbO*] = 0.396 Incorrect Determine the potential at the cathode when the SbO* concentration is 0.0015 M? Ecahode = 0.0674

I just need help with the [SBO+ ], I can't figure out what I did wrong. Please help A buffered solution of 0.0340 M SbO* and 0.0180 M Cď²+ was prepared with a pH of 2.15 at 25 °C. Eso: = 0.208 V E. = -0.402 V Sbo* + 2H* +3e= Sb(s) + H,O Ca2+ + 2e = Cd(s) Which ion is more easily reduced? Sbo* What is the concentration of SbO* at the potential when Cd²+ will begin to be deposited? [SbO] = 0.396 Incorrect Determine the potential at the cathode when the SbO concentration is 0.0015 M? Ecahode = 0.0674

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

7. Find the pH of a mixture of 0.100 M HClO₂ (aq) (Ka = 1.1 x 10-2) solution and 0.150 M HClO (aq) (Ka = 2.9 x 10-8). Find the percent dissociation for HClO2.
Calculate the pH for each of the cases in the titration of 25.0 mL of 0.130 M pyridine, C,H,N(aq) with 0.130 M HBr(aq). The K₁ of pyridine is 1.7 × 10-9. before addition of any HBr pH = after addition of 12.5 mL of HBr pH = after addition of 15.0 mL of HBr pH = after addition of 25.0 mL of HBr pH =
Determine the resulting pH when 0.003 mol of solid NaOH is added to a 100.0 mL buffer containing 0.13 M HClO and 0.37 M NaClO. The value of Ka for HClO is 2.9 × 10⁻⁸ Please solve for the pH
7.5mL of 333mM Tris was added to 192.5ml of water. The resulting solution was added to 240mL of water and the pH was adjusted to 8.0 using 10mL of HCl. A further 33.3mL of water was added. What is the concentration of the final solution (in millimolar)? The MW of Tris is 121.14
Help needed
Consider the below reaction, where you have 20.0ml of .18M C5H5N, which has a kB of 1.42x10^-9 C5H5N(aq) + HCl(aq) -> C5H5NH+(aq) + Cl-(aq) A. What is the pH at equivalence point using .069M HCl solution? What is the pH instead If you add 37 mL of .069M HCl solution?
50.00 mL of 0.100 M CH;COOH is being titrated with 0.100 M of NaOH. What is the pH at the equivalence point? K, of CH3COOH is 1.8 x 105. Upload your work in order to receive credit.
In the titration of 25.0 mL of 0.1 M F− (where the solution was made using NaF(aq)) with 0.1 M HCl, how is the pH calculated after 12.5 mL of titrant is added? Group of answer choices The pH is based on the concentration of protons present in the solution, which is equal to the original concentration of the acid. The pH is equal to the pKa of the conjugate acid. The pH is 7. The pH is calculated by determining the concentration of weak base present in the solution, using an ICE table to calculate the hydroxide ion concentration present after hydrolysis, subtracting pOH from 14, and taking the negative log of the result. The pH is calculated by determining the concentration of excess hydroxide ions in the solution, subtracting pOH from 14, and taking the negative log of the result. The pH is 1. The pH is 14. The pH is calculated by determining the concentration of protons left in the solution after neutralization, and taking the negative log of the result.
The pK, values for the dibasic base B are pKi = 2.10 and pk2 = 7.49. %3! Calculate the pH at each of the points in the titration of 50.0 ml. of a 0.55 M B(aq) solution with 0.55 M HCI(aq). What is the pH before addition of any HCI? pH What is the pH after addition of 25.0 ml. HCI? pH = What is the pH after addition of 50.0 mL HC? pH What is the pH after addition of 75.0 mlL HCI? pH = What is the pH after addition of 100.0 ml. HCI? pH =
An aqueous solution has [HC7H5O2] = 0.100 M and [Ca(C7H5O2)2] = 0.200 M. Ka= 6.3 × 10-5for HC7H5O2. Thesolution volume is 5.00 L. What is the pH of the solution after 10.00 mL of 5.00 M NaOH is added?
iew History Bookmarks Profiles Tab Window Help )) * 33% [4 Thu 11:56 AM 三 101 Chem101 -> A app.101edu.co 山 ☆ Tp O Update : Question 6 of 10 Submit al Determine the pH of a buffer formed by dissolving 21.5 g HC,H,O2 and 37.7 g of NaC,H;O2 in 200.0 mL of solution. The value of Ka for HC,H5O2 is 6.3 x 10-5. < PREV 1 3 NEXT Based on your ICE table and definition of Ka, set up the expression for Ka in order to determine the unknown. Do not combine or simplify terms. Ka = 6.3 x 10-5 %3D %3D O RESET [0] [37.7] [0.176] [0.261] [0.880] [1.31] [0.178] [21.5] [2x] [21.5 - x] [37.7 + x] [0.176 - x] [0.261 + x] [0.880 - x] [0.888] [x] [1.31 + x] [0.178 + x] [0.888 + x] lil
A solution witha volume of 1.00 Lis 0.350 M in CH3COOH(aq) and 0.450 M in CH3COONA(aq). What will the pH be after 0.0400 mol of HCl is added to the solution? Ka for CH3COOH(aq) = 1.80 x 10 OA. 4,94 OB. 9.23 C.4.77 D.9.06 E. 4.85