0.030 moles of a weak acid, HA, was dissolved in 2.0 L of water to form a solution. At equilibrium, the concentration of HA was found to be 0.013 M. Determine the value of Ka for the weak acid.
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.030 moles of a weak acid, HA, was dissolved in 2.0L of water to form a solution. At equilibrium the concentration of HA was found to be .013 M. Determine the value of Ka for the weak acid.
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0.030 moles of a weak acid, HA, was dissolved in 2.0 L of water to form a
solution. At equilibrium, the concentration of HA was found to be 0.013 M.
Determine the value of Ka for the weak acid.
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2
Based on your ICE table and definition of Ka, set up the expression for Ka and then
evaluate it. Do not combine or simplify terms.
Ka
%3D
%3D
5 RESET
[0]
[2.0]
[0.030]
[0.013]
[0.060]
[0.015]
[0.017]
[0.002]
[0.011]
[x]
[2x]
[0.030 + x]
[0.030 - x]
[0.015 + x]
[0.015 - x]
3 x 10-4
3 x 103
0.2](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fda9c8b35-666b-48ab-a806-a1fce889b83d%2F9d792e6e-b386-4841-b767-1fb8fa0df180%2Fl9swg5p.png&w=3840&q=75)
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