A chemistry graduate student is given 450. mL of a 1.20M ammonia (NH,) solution. Ammonia is a weak base with K, = 1.8 x 10. What mass of NH¸Br should the student dissolve in the NH, solution to turn it into a buffer with pH =9.56? You may assume that the volume of the solution doesn't change when the NH, Br is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.

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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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O ACIDS AND BASES
Calculating the composition of a buffer of a given pH
4/5
A chemistry graduate student is given 450. mL of a 1.20M ammonia (NH,) solution. Ammonia is a weak base with K, = 1.8 × 10 . What mass of NH,Br
should the student dissolve in the NH, solution to turn it into a buffer with pH =9.56?
You may assume that the volume of the solution doesn't change when the NH,Br is dissolved in it. Be sure your answer has a unit symbol, and round it to 2
significant digits.
Transcribed Image Text:O ACIDS AND BASES Calculating the composition of a buffer of a given pH 4/5 A chemistry graduate student is given 450. mL of a 1.20M ammonia (NH,) solution. Ammonia is a weak base with K, = 1.8 × 10 . What mass of NH,Br should the student dissolve in the NH, solution to turn it into a buffer with pH =9.56? You may assume that the volume of the solution doesn't change when the NH,Br is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.
O KINETICS AND EQUILIBRIUM
Calculating equilibrium composition from an equilibrium constant
OOD 3/5
Suppose a 500. mL flask is filled with 1.5 mol of O, and 0.60 mol of NO. The following reaction becomes possible:
N,(2) -0,(2) – 2NO(2)
The equilibrium constant K for this reaction is 5.01 at the temperature of the flask.
Calculate the equilibrium molarity of O,. Round your answer to two decimal places.
M
Transcribed Image Text:O KINETICS AND EQUILIBRIUM Calculating equilibrium composition from an equilibrium constant OOD 3/5 Suppose a 500. mL flask is filled with 1.5 mol of O, and 0.60 mol of NO. The following reaction becomes possible: N,(2) -0,(2) – 2NO(2) The equilibrium constant K for this reaction is 5.01 at the temperature of the flask. Calculate the equilibrium molarity of O,. Round your answer to two decimal places. M
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