Asked by Mark
HCOOH(aq) <-----> H^+ (aq)+ HCOO^-(aq)
The equilibrium constant (Ka) for Reaction 3 at 25 °C is 1.80 × 10−4 mol dm−3. Calculate the equilibrium concentration of hydrogen ions if the concentration of formic acid at equilibrium is 0.00500 mol dm−3
The equilibrium constant (Ka) for Reaction 3 at 25 °C is 1.80 × 10−4 mol dm−3. Calculate the equilibrium concentration of hydrogen ions if the concentration of formic acid at equilibrium is 0.00500 mol dm−3
Answers
Answered by
DrBob222
I don't know what reaction 3 is.
........HCOOH ==> H^+ + HCOO^-
I.......0.005.....0.......0
C.......-x........x.......x
E......0.005-x....x.......x
Substitute the E line into the Ka expression and solve for x = H^+.
........HCOOH ==> H^+ + HCOO^-
I.......0.005.....0.......0
C.......-x........x.......x
E......0.005-x....x.......x
Substitute the E line into the Ka expression and solve for x = H^+.
Answered by
Mark
Sorry I should have left that out, it's just the formula
HCOOH(aq) <-----> H^+ (aq)+ HCOO^-(aq)
HCOOH(aq) <-----> H^+ (aq)+ HCOO^-(aq)
Answered by
DrBob222
The solution I posted stands.
Answered by
Mark
OK thanks....
In the question, and in the example in the textbook there was no example of using an ICE table. Tables make assigning values so much easier
In the question, and in the example in the textbook there was no example of using an ICE table. Tables make assigning values so much easier
Answered by
DrBob222
ICE tables are the baling wire of chemistry.
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