Using the value of Ksp for Ag2S (see Appendix D), Ka1 and Ka2 for H2S (see...
Using the value of Ksp for Ag2S (see Appendix D), Ka1 and Ka2 for H2S (see Appendix D), and Kf = 1.1*105 for AgCl2-, calculate the equilibrium constant for the following reaction:
Ag2S (s) + 4Cl- (aq) + 2H+ (aq) ↔ 2AgCl2- (aq) + H2S (aq)
ksp for Ag2S= 6*10^-51
for H2S
ka1=9.5*10^-8 ka2=1*10^-19
Homework Answers
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Using the value of Ksp for Ag2S (see
Appendix D), Ka1 and Ka2 for H2S
(see...
1) A buffer contains 0.15 mol of propionic acid (C2H5COOH) and 0.10 mol of sodium propionate...
1) A buffer contains 0.15 mol of propionic acid (C2H5COOH) and 0.10 mol of sodium propionate (C2H5COONa) in 1.20L. (a) What is the pH of this buffer? (b) What is the pH of the buffer after the addition of 0.01 mol of NaOH? (Ka for C2H5COOH is 1.3*10-5) 2) Using the value of Ksp for Ag2S (see Appendix D), Ka1 and Ka2 for H2S (see Appendix D), and Kf = 1.1*105 for AgCl2-, calculate the equilibrium constant for the following...
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Phosphoric acid has a formula of H3PO4, and has a Ka1 of 7.5×10–3 , Ka2 of...
Phosphoric acid has a formula of H3PO4, and has a Ka1 of 7.5×10–3 , Ka2 of 6.2×10–8 , and Ka3 of 4.2×10–13 at 25 ºC. What is the equilibrium constant for the following reaction at 25°C? HPO42–(aq) + H2O(l) ⇄ H2PO4–(aq) + OH–(aq) A.) 4.2×10–13 B.) 1.3×10–12 C.) 2.4×10–2 D.) 7.5×10–3 E.) 1.6×10–7
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1. Calculate the solubility product constant, Ksp, for strontium fluoride if 1.2×10-3mol of F-ion is present in 2.0 L of a saturated strontium fluoride solution. A.9.0×10-8 B.2.7×10-11 C.6.9×10-9 D.1.1×10-10 E.1.4×10-6 2. Choose the correct equilibrium constant expression (Ksp) for the dissolution of Ag2S . (is the answer D?) A. [ Ag2S ] Ksp = [ Ag+]2 [ S2-] B. Ksp = [ Ag+][ S2-]2 C. [ Ag+] [ S2-] Ka = [ Ag2S ] D. Ksp = [ Ag+]2 [...
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Please answer and show all work. thank you!!!!!! 6. The following equilibrium constants have been determined...
Please answer and show all work. thank you!!!!!!
6. The following equilibrium constants have been determined for hydrosulfuric acid at 25°C: H2S(aq)<> H(aq) + HS (aq) K. = 9.5 x 10-8 HS (aq) → H+ (aq) + S2 (aq) K". = 1.0 x 10-19 Calculate the equilibrium constant for the following reaction at the same temperature: H2S(aq) → H(aq) + S2- (aq)
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Using data found in Appendix E of your textbook calculate the nonstandard emf for each of...
Using data found in Appendix E of your textbook calculate the
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molar and everything else is standard (use 298 K for the
temperature, R = 8.314 J/mol-K, and F = 96,485 C/mol):
Using data found in Appendix E of your textbook calculate the nonstandard emf for each of the following reactions if the concentration of each of the ions...
Please answer and show all work. thank you!!!!!!
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temperature, R = 8.314 J/mol-K, and F = 96,485 C/mol):
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