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Require to prepare 100.0mL of a pH=4.00 buffer solution using 0.100 M benzoic acid pKa=4.20 and 0.120 M sodium benzoate.
Explain how much of each solution must be mixed to prepare this buffer?
Calculate the final temperature of a mixture of 150.0 g of ice initially at -13.5 degrees celsius and 345.0 g of water initially at 86.5 degrees celsius.
An aqueous solution of sodium chloride in an electrolytic cell is subjected to a current of 2.50 amps for 15.0 minutes. How many mL of chlorine gas are collected at 25.0oC if the pressure if 750.0 torr
consider the composition of dry air in 0 humidity is just about 21 o2 78 n2 and 1 argon by moles. compute the density
which of the following atoms with the specified electronic configuration would have the lowest first ionization energy? (a) (He)2s^2 2p^3 (b) (ne) 3s^2 3p^4 (c) [Xe]6s^1 (d) [Xe]6s^2 4f^14 5d^10 6p^1
The osmotic pressure of this solution was 0.00178 atm at 25 C. Calculate the molar mass of hemoglobin, which is a molecular compound and a nonelectrolyte
Rhodium has a density of 12.41 g/cm3 and crystallizes in a face-centered cubic lattice. Calculate the radius of a rhodium atom?
A 800 mL sample of a saturated aqueous solution of calcium oxalate, CaC2O4, at 95 degrees C is cooled to 13 degrees C. How many milligrams if calcium oxalate will precipitate?
at a fixed temperature equal moles of n2 g and f2 g are mixed in a constant pressure container the volume of the
A sample of nitrogen gas in a 4.6-L container at a temperature of 26°C exerts a pressure of 3.9 atm. Calculate the number of moles of gas in the sample.
Construct a Born Haber cycle for the formation of the hypothetical compound NaCl2, where the sodium ion has a 2+ charge. A. How large would the lattice energy need to be for the formation of NaCL2 to be exothermic
How does the addition of aqueous NH3 to a solution separate and identify Cu2 and Bi3 ions? Why wouldn't the additon of a strong base, such as KOH, work just as well as the addition of aqueous NH3?
100 mL of 0.150 M acid H2A are mixed with 100 mL of 0.1600 M NaOH. Calculate the [H+] of the resulting solution at equilibrium. Ka1 = 1.0 x 10^-5 Ka2 = 1.0 x 10^-7
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