Kf for the complex ion Ag(NH3)2+ is 1.7 × 107. Ksp for AgCl is 1.6 × 10-10. Calculate the molar solubility of AgCl in 1.0 M NH3.
Answer to relevant Questionsa. Using the Ksp for Cu(OH)2 (1.6 × 10-19) and the overall formation constant for Cu(NH3)42+ (1.0 × 1013), calculate a value for the equilibrium constant for the reaction Cu(OH)2(s) + 4NH3(aq) ⇌ Cu(NH3) 42+(aq) + ...The salts in Table 8.5, with the possible exception of the hydroxide salts, have one of the following mathematical relationships between the Ksp value and the molar solubility s. i. Ksp = s2 ii. Ksp = 4s3 iii. Ksp = 27s4 iv. ...The copper(I) ion forms a complex ion with CN- according to the following equation: Cu+(aq) + 3CN-(aq) ⇌ Cu(CN)32-(aq) Kf = 1.0 × 1011 a. Calculate the solubility of CuBr(s) (Ksp = 1.0 × 10-5) in 1.0 L of 1.0 M NaCN. b. ...The following are representations of acid– base reactions: a. Label each of the species in both equations as an acid or a base and explain. b. For those species that are acids, which labels apply: Arrhenius acid and/ or ...Use Table to order the following from the strongest to the weakest base. ClO2-, H2O, NH3, ClO4- Table
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