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1) What is the advantage of measuring the absorbance of a solution at lambda max wavelength?
2) Under what conditions would it be wise to measure the absorbance of a compound at a wavelength other than lambda max wavelength?
State net ionic equations for the reactions if any that take place when the aqueous solutions listed below are mixed.
Explain the dissolution of the sulfides of copper, bismuth and cadmium in nitric acid. Include ionic equations. If a yellow precipitate is obtained upon addition of hydrogen sulfide to an unknown solution of Group II cations, which ions are probably..
Calculate the molarity of a solution made by dissolving 0.850 grams of Na2SO4 in enough water to form exactly 930 mL of solution.
Balance the subsequent equations. Utilize the lowest possible whole number coefficients. Comprise states-of-matter under the given conditions
how does the first ionizaiton energy of the alkali metal in a given period compare with the first ionization energy of the halogen in the same period. what is the result in terms of how these elements tend to react with each other
Compute percent of purity of alum, presence of aluminum, potassium & sulphate in the sample. The mass of aluminum & potassium in the sample analyzed.
The molecular mass of propanoic acid is 75.1 amu. Calculate the molecular mass of methyl ethanoate, an isomer of propanoic acid. Express your answer with appropriate units.
Consider the reaction COg) + NH3=HCONH2, Kc=0.800. If a reaction vessel initially contains only CO and NH3 at concentrations of 1.00 M &2.00M, respectively, what will the concentration of HCONH2 be at equilibrium
Q 3: The salt NaBrO(3) oxides Sn^2+ to SnCl(6)^2- in the presence of hydrochloric acid according to the equation
Why is the iodine added. What is the role of the magnesium in this reaction. Why is the 3-phenylpropyl-bromide mixed with anhyrous diethyl ether. What does the dry ice do. What does the HCl do
what is the dose in rads to the animal in the first 4.0 hours following the ingestion of the radioactive material?
Problem- A 53.7 g ice cube at -19 C is dropped into an insulated cup containing 125.0 ml of hot water at 78 C. The specific heat of ice is 2.12 J/g deg. assuming no heat is able to pass through the insulated cup
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