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1) Would you use UV spectrophotometry to screen for either or both of methamphetamine and diazepam compounds?
2) How can the relative scarcity of drugs that fluorescence be an advantage in some instances and a disadvantage in others?
What is the concentration of the compound in a solution whose absorbance at 219 nm is A = 0.080 with a sample pathlength of 1.00 cm
Why is it necessary to use relatively exotic reagents to form precipitates with the Lithium group ions
Derive an expression for the force constant of an oscillator that can be modelled by a Morse potential using equation 12.37 which states
An aqueous CaCl2 solution has a vapor pressure of 83.7mmHg at 50 C . The vapor pressure of pure water at this temperature is 92.6mmHg.
Hydrogen gas can be produced in the labratory through the reaction of magnesium metal with hydrolic acid: Mg (s) + 2HCl (aq) ---> MgCl2 (aq) +H2 (g). What is the volume, in liters, of H2 gas produced at 26C and 770mmHg from the reaction of 13.0g o..
Suppose that a 25-mL sample of a solution is to be tested for I- ion by addition of 1 drop (0.20 mL) of 0.27 M Pb(NO3)2. What is the minimum number of grams of I- that must be present
90.0 of is initially at room temperature (22.0). A chilled steel rod at 2.0 is placed in the water. If the final temperature of the system is 21.5.
what mass of limestone is required to remove all the sulfur dioxide formed by the combustion of 9.2 X 10^4 kg of coal that is 0.33 mass % sulfur?
Use standard heats of formation and absolute entropies to calculate the equilibrium pressure (atm) PCO2 at 340 K.
The first ionization energy of Na is 495.9 kJ/mol. What is the longest wavelength of light that could remove an electron from a Na atom
Consider the titration of a 23.0 mL sample of 0.110M HC2H3O2 with 0.130M NaOH. Determine the pH at 6.00 mL of added base.
calculate the total heat in j needed to convert 30.00 g of ice at -3.25 c to liquid water at 0.250 c m.p. at 1 atm 0.0
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