Answer the following questions concerning a 5.72 wt% acetic acid (CH3COOH) solution. 4. If the solution has a density of 1.06 g/m L, then what is its concentration in molarity (mol/L)? a. b. The dissociation of acetic acid in water (below) has an equilibrium constant of 1.8 x 105. Use an "ICE" table to calculate [CH3COO] at equilibrium in molarity (mol/L). Hint: start with your answer from part (a). CH3C00 (aq) + H30+ (aq) CH3COOH (aq) + H20 (I)

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Answer the following questions concerning a 5.72 wt% acetic acid (CH3COOH) solution.
4.
If the solution has a density of 1.06 g/m L, then what is its concentration in molarity (mol/L)?
a.
b. The dissociation of acetic acid in water (below) has an equilibrium constant of 1.8 x 105.
Use an "ICE" table to calculate [CH3COO] at equilibrium in molarity (mol/L). Hint: start with
your answer from part (a).
CH3C00 (aq) + H30+ (aq)
CH3COOH (aq) + H20 (I)
Transcribed Image Text:Answer the following questions concerning a 5.72 wt% acetic acid (CH3COOH) solution. 4. If the solution has a density of 1.06 g/m L, then what is its concentration in molarity (mol/L)? a. b. The dissociation of acetic acid in water (below) has an equilibrium constant of 1.8 x 105. Use an "ICE" table to calculate [CH3COO] at equilibrium in molarity (mol/L). Hint: start with your answer from part (a). CH3C00 (aq) + H30+ (aq) CH3COOH (aq) + H20 (I)
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