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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. 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

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. 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

Principles of Modern Chemistry
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter16: Solubility And Precipitation Equilibria
Section: Chapter Questions
Problem 37P
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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 help 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. 

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!
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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