1. The Kp of gold (1) chloride is 2.0 x 1013, The Kr of the gold (I)-cyanide complex ion is 2.0 x 10%. A. Write the balanced net ionic equation for the reaction between AuCl and NaCN that produces the gold (1)-cyanide complex ion. B. Determine the value of K for the above chemical reaction. C. Determine the solubility of AuCl in a 0.20 M solution of NaCN.

1. The Kp of gold (1) chloride is 2.0 x 1013, The Kr of the gold (I)-cyanide complex ion is 2.0 x 10%. A. Write the balanced net ionic equation for the reaction between AuCl and NaCN that produces the gold (1)-cyanide complex ion. B. Determine the value of K for the above chemical reaction. C. Determine the solubility of AuCl in a 0.20 M solution of NaCN.

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

The solubility of Ca(OH)2(s) is equal to: A. [Ca2+] B. [OH]/2 C. All of the above D. None of the Above
1. What is the pH of the buffer containing 0.10 M Na2HPO4 and 0.15 M NaH2PO4? (Ka = 6.20 x 10-8) 2. Calculate the pH and pOH of 0.27 N Ca(OH)2.
a. Give the chemical equation for the dissociation of PbCl2. b. What is the molar solubility of PbCl2? c. What are the equilibrium concentration of the ions?
What is the molar solubility of calcium hydroxide Ksp (Ca(OH)2) = 5.02 × 10-6J, when it is added to a solution that contains the following: A.) Pure water B.) 0.027 M NaOH
The pKa of finalic acid is 6.50. a. What is the pH of an equimolar solution of finalic acid and sodium finalate? Assume that both solutions are at 0.1 M. b. Would you expect the buffer capacity to be higher or lower if you decrease the concentration of each constituent to 0.01 M? Why? c. What is the effect of water dissociation on the pH of the solutions? d. Only considering the pH of the solution, would it be safe to drink a 0.1 M solution of finalic acid? How about a 0.01 M solution?
Calculate the concentration of metal ions, M³+, in a solution that initially contains 0.20 M M(NO3)3 and 1.60 M lit cyanide which produces the complex ion [M(CN)6]³, Kf = 2.47 × 10³1
6. A buffer solution contains 0.120 moles of propionic acid, HC3H502, and 0.100 moles of sodium propionate, NaC3H5O2, in 1.00 L of solution. Ka = 1.32 x 10-5 a. What is the pH of this buffer? b. What is the pH of this buffer after the addition of 0.010 mol of NaOH? c. Beginning with the initial buffer from part a, what is the pH of the buffer after the addition of 0.010 mol of HBr?
[References] a. Calculate the pH of a buffer that is 0.4 M in acetic acid (CH3 COOH) and 0.4 M in potassium acetate (CH3 COOK). The pK, for acetic acid is 4.74. pH = b. What is the pH of a buffer that is 3 M in acetic acid and 3 M in potassium acetate? pH = c. What is the difference between the buffers described in parts a and b? The solution in part b has buffer capacity than the solution in part a. Submit Answer Try Another Version 5 item attempts remaining
Could aqueous ammonia be used instead of hot water to separate lead ion from the mixed chloride precipitate? Explain
Calculate the solubility product constants of the following salts. a. CaC₂04 -0.0055 g/L b. BaCrO4 -0.0037 g/L c. CaF2 -0.017 g/L How much NaOH must be added to 1.0 L of 0.010 M H3BO3 to make a buffer solution of pH 10.10?
The Kgp values for both AGOH and Ni(OH)2 are 1.5 x 10-8 and 6.5 x 10-18, respectively. When the pH value of the solution is reduced from 7 to 3, which complex has a higher molar solubility? Assume the solution at each pH is buffered. A. AgOH B. Ni(OH)2 C. They have the same solubility D. None of the above
9. Calculate the pH of the solution that results from each mixture. a. 50.0 mL of 0.15 M HCHO₂ with 75.0 mL of 0.13 M NACHO₂ b. What mass of sodium benzoate should you add to 150.0 mL of a 0.15 M benzoic acid solution to obtain a buffer with a pH of 4.25? (Assume no volume change)