Calculate [H2S], [H3O+], [HS-], [S2-] for 0.10M H2S.
Ka1= 1.1 x 10-7
Ka2= 1.0 x 10-14
Major Species? Dominant Equilibrium?
Calculate [H2S], [H3O+], [HS-], [S2-] for 0.10M H2S. Ka1= 1.1 x 10-7 Ka2= 1.0 x 10-14...
Calculate the pH of a 0.982 M solution of hydrogen sulfide (H2S) Where: H2S (aq) -> H+ (aq) + HS- (aq) Ka1 = 1.0 x 10-7 HS- (aq) -> H+ (aq) + S2- (aq) Ka2 = 1.0 x 10-19 Enter your answer with at least 2 sig figs.
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
Calculate the pH and [S2-] in a 0.15 M H2S solution. Assume Ka, 1.0 x 10-7, Ka2 = 1.0 x 10-19. pH s2-1 Need Help? Read It Supporting Materials ■ Supplemental Data Periodic Table Constants & Factors 7. -6.25 points ZumChemP8 7.E.098. Calculate the pH of a 3.4x 10-3 M solution of H2SO4
The ionization constants for the diprotic acid H 2S are 1.0 x 10 -7 and 1.3 x 10 -13. H2S (aq) + H2O (l) <=> HS -(aq) + H3O +(aq) Ka = 1.0 x 10 -7 HS -(aq) + H2O (l) <=> S-2 (aq) + H3O +(aq) Ka = 1.3 x 10 -13 What is the equilibrium concentration of HS - in a 0.300 M solution of H2S?
Calculate the pH and the equilibrium concentration of S2- in a 7.90×10-2 M hydrosulfuric acid solution, H2S (aq). For H2S, Ka1 = 1.0×10-7 and Ka2 = 1.0×10-19
For a 1.0 M solution of H2S at equilibrium, which of the following statements are correct? Ka: H2S = 9.1 x 10-8 HS- = 1.0 x 10-13 1. [H3O+] = [H2S] 2. [OH-] = 1.0 x 10-7 M 3. [HS-] = 9.1 x 10-8 M 4. [S2-] = 1.0 x 10-13 M
The ionization constants for the diprotic acid H 2S are 1.0 x 10 -7 and 1.3 x 10 -13. H2S (aq) + H2O (l) <=> HS -(aq) + H3O +(aq) Ka = 1.0 x 10 -7 HS -(aq) + H2O (l) <=> S-2 (aq) + H3O +(aq) Ka = 1.3 x 10 -13 What is the equilibrium concentration of HS - in a 0.300 M solution of H2S?
1) Given the two reactions: a) H2S<--> HS- + H+, K1=9.13 x 10-8 b) HS-<--> S2- + H+, K2=1.20 x 10-19 what is the equilibrium constant Kfinal for thefollowing reaction? S2- + 2H+<--> H2S 2) Given the two reactions: a)PbCl2 <--> Pb2+ + 2Cl-,K1= 1.80 x 10-10 b) AgCl<--> Ag+ + Cl-, K2= 1.23 x10-4 what is the equilibrium constant Kfinal for thefollowing reaction? PbCl2 + 2Ag+<--> 2AgCl + Pb2+
Calculate the concentrations of all species present in 0.14 M H2SO3. (Ka1=1.5×10−2, Ka2=6.3×10−8). Calculate the concentration of H2SO3, HSO3- , H3O+, SO32- in solution.
Q. The pH of a solution of 1.1M H2A (Ka1 = 1.0 x 10^-6 an Ka2 = 1.0 x 10^-10) is: a. 10.00 b. 5.96 c. 11.02 d. 2.98 e. None of these