If given the information below, how do you calculate the #K_c# for the reaction #2HF(aq) + C_2O_4^(2-)(aq) rightleftharpoons 2F^(-)(aq) + H_2C_2O_4(aq)#?
Here's what I got.
You know that
Before moving on, take the time to write the expressions of the two equilibrium constants given to you.
You will have
Now, notice that your target equilibrium
has the oxalate anion on the products' side, so star by reversing the second equilibrium
The new equilibrium constant for this reaction is
As you can see, you can write this as
This will get you
The new equilibrium constant for this reaction will be
You can rewrite this as
which means that you will have
You can now add the two equilibrium reactions to get the target equilibrium
This simplifies to
The equilibrium constant for this equilibrium will be
The answer is rounded to two sig figs.
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[ K_c = \frac{{[\text{{F}}^-]^2 \cdot [\text{{H}}_2\text{{C}}_2\text{{O}}_4]}}{{[\text{{HF}}]^2 \cdot [\text{{C}}_2\text{{O}}_4^{2-}]}} ]
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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
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- According to Le Chatelier's Principle: What happens when you add DIFFERENT species to the equilibrium?
- How many mols of #"CO"_2# were added at constant temperature and volume to a #"1-L"# container containing #"0.400 mols"# of #"CO"_2# and of #"H"_2#, and #"0.200 mols"# of #"CO"# and of #"H"_2"O"(g)# (#K_c = 4#) to cause #"CO"_2# to drop to #"0.300 mols"#?
- What is common ion effect ? Give 3 examples of salt that xan affect the ionization of HNO2 solution?

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