Consider the following elementary reaction: (CH₃)₃CBr (aq) → (CH₃)₃⁺ (aq)+ Br⁻ (aq) Suppose we let k₁ stand for the rate constant of this reaction and k₋₁stand for the rate constant of the reverse reaction. Write an expression that gives the equilibrium concentration of (CH₃)₃C⁺ in terms of k₁, k₋₁, and the equilibrium concentrations of (CH₃)₃CBr and Br⁻.

Determine the number o moles of ions/atoms/particle in the following: 2.50 miles of k2s (let me know how to do)

Salicylic acid is a very important acid. it is used to synthesize the aspirin by treating with acetic anhydride. a 0.2015-g sample of salicylic acid was dissolved in a 100.00-ml volumetric flask, and the solution was diluted to the mark. a 10-ml aliquot of this solution was titrated with standard naoh (0.01130 + 0.2% n) to a phenolphthalein faint pink color end point at 19.81 ml. (a) (calculate the normality of the salicylic acid solution used in the titration. (b) assuming the salicylic acid is pure, what is the equivalent weight of the salicylic acid? practice problems for the final exam (continued) (c) (calculate the inherent error in the determination of the equivalent weight you calculated in part (b). use the following absolute errors in the equipment /glassware when calculating the inherent error. 5.00-ml pipet: + 0.02 ml 100-ml volumetric flask: + 0.08 ml analytical balance: + 0.2 mg 25-ml buret: + 0.03 ml

Upon decomposition, one sample of magnesium fluoride produced 1.65 kg of magnesium and 2.56 kg of fluorine. a second sample produced 1.32 kg of magnesium. part a how much fluorine (in grams) did the second sample produce?