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a. What combination of a molecular base (that is a neutral compound, not an ion!) and a salt of the conjugate acid of that molecular base should you select to prepare a buffer solution that would maintain a pH of 9.00? For full credit, explain your choice (in a simple, straightforward manner, keep your answer under 40 words and don%u2019t forget to specify a common spectator ion as the counter-ion in the salt).
b. What ratio of concentrations of the molecular base you chose in part a and its conjugate acid would be necessary to achieve a pH of exactly 9.00?
c. Describe, using one well-written sentence, a simple and practical way to make 1.00L of this buffer solution, assuming a 1.0 M solution of the molecular base is available and that the chloride salt of the conjugate acid is available as a solid. (Note: Laboratory balances are calibrated in grams and pipettes in mL, neither are calibrated in moles - hint)
Nitrogen reacts with a metal to form a compound in which there are three atoms of the metal for each atom of nitrogen. If 1.486 g of the metal reacts with 1.000 g of nitrogen
Determine number of moles of oxygen molecules are in the cylinder and compute the mass of solid C 2 H 3 NaO 2 required mixing with 60.0mL of .125M C 2 H 4 O 2 to form a ph 4.20 buffer?
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The osmotic pressure,pie , of a solution of glucose is 83.1atm . Find the molarity of the solution at 298k .
A compound is constituted by mass of 22.6% phosphorus, the rest being chlorine. Given that a volume of 307 mL of the gas has a mass of 1.55 g at 25 °C and 90 kPa, find the molecular formula for this compound
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2 NaClO3-> 2 NaCl + 3 O2 Determine the number of moles of O2 produced by the decomposition of 213 g of NaClO3.
the total pressure in the container is 3.70 atm . Calculate the partial pressure of each gas in the container
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The dipole moment and the normal boiling point of acetaldehyde (CH3CHO) are 2.7 D and 293 K, respectively. The dipole moment and the normal boiling point of n-octane (C8H18) are 0 D and 298 K.
For the following molecules and ions, draw a Lewis structure, calculate formal charges for each atom, and determine the oxidation number for each atom.
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