Asolution was prepared by dissolving 1210 mg
ofk3fe(cn)6 (329.2 g/mol) in sufficient
waterto give 775 ml. calculate:
a) the molar analytical concentration
ofk3fe(cn)6.
b) the molar concentration of k+.
c) the molar concentration
offe(cn)63-.
d) the weight/volume percentage
ofk3fe(cn)6.
e) the number of millimoles of k+ in 50.0 ml of
thissolution
f) ppm fe(cn)63-.
g) pk for the solution
h) pfe(cn)6 for the solution.

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

What happened to the amount of carbon dioxide in the atmosphere from 2010–2017?

The volume of a single vanadium atom is 9.29×10-24 cm3. what is the volume of a vanadium atom in microliters?