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a) Prepare 3 liters of 0.5 M glutamic acid buffer, with pH 4.1, from solid glutamic acid (pKa=4.2) and 2 M NaOH. How many grams of solid glutamic acid (MW=147 g/mol) would you have to use and how many mls of 2 M NaOH would you need?
b) Prepare 2 liters of 0.5 M "lactate" buffer with a pH of 4.0, using a 2 M solution of lactic acid (pKa=3.86) and a 1M solution of sodium lactate. (Note: a 0.5 M buffer has a total concentration of 0.5M by adding [HA] and [A-])
A two-component mixture is analyzed by gas chromatography with flame ionization detection. compound x has a retention time of tr= 11.53 min with N= 16,520 theoretical plates
How many moles of O2 will be produced if 4.83 moles of CO2 react completely?
Key by key on calculator how would I solve for x in 0.2=(0.5)^(x/14.2)? -Original question that brought me to that point-"The half-reaction of 32P is 14.2 days
A vessel containing 45.0 cm3 of helium gas at 25°C and 106 kPa was inverted and placed in cold ethanol. As the gas contracted, ethanol was forced into the vessel to maintain the same pressure of helium.
How many grams of Ca(OH)2 are needed to neutralize 3.6 moles of HCl in 655 mL of solution? The molar mass of HCl is 36.46 g/mol. The molar mass of Ca(OH)2 is 74.1 g/mol.
If one were to perform carbon dating on living clams instead of getting a zero age ( they are in fact living) one would get an age of approximately 400 years old for these living clams.
An oxide of phosphorus contains 56.4% oxygen and has a molar mass of 284 g/mol. What is the molecular formula for this compound?
At a certain temperature and pressure 4.2 L of N2 reacts with 6.3 L of O2. If all the N2 and O2 are consumed, what volume of N2O3, at the same temperature and pressure, will be produced?
a gas diffuses only .5 times as fast as an oxygen molecule at the same temperature. what is the molecular weight of the gas?
Explain the general idea of the LCAO-MO method.
Balance the following molecular equations for these reactions. Write the ionic equation for the reactions. Write the net ionic equation for the reactions.
A student added 5.85g of KMnO4 to a beaker containing 150ml of 0.200 M KMnO4 solution. Calculate the molar concentration of the final solution. Assume volume remains constant.
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