This is the answer I got for this problem, but It’s saying I have the change in concentration wrong. I don’t understand what the prompt is saying here. I also have Ka = 2x/(0.015-x) = 0.0003 Is that correct? It didn’t fit on the snip I took, sorry. Transcribed Image Text: 0.030 moles of a weak acid, HA, was dissolved in 2.0 L of water
equilibrium, the concentration of HA was found to be 0.013 M. Determine the value of
Ka for the weak acid.
form a solution. At
1
2
NEXT
Based on the given values, fill in the ICE table to determine concentrations of all reactants and
products.
HA(aq)
H:O(1)
H:O*(aq)
A (aq)
+
Initial (M)
0.015
Change (M)
-X
+x
+x
Equilibrium (M)
0.015 – x
+x
+x
Incorrect, 2 attempts remaining
Your Change in concentration for HA is incorrect. In this problem, you should use the
difference Initial and Equilibrium conditions given above to determine the Change in
concentration for each relevant species in the reaction. Remember that the Change in
concentration for each species will be directly proportional to the coefficient from the balanced
chemical reaction!
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