the different Ks
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the different Ks
I am confused about the different Ks: Ka, Kb, Kw, Kc, and Kp. What exactly are the differences between them?
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Re: the different Ks
Ka, Kb, Kw, Kc, and Kp
Ka: This is when you find the K value for a reaction with a compound that is acting as an acid.
Kb: This is when you find the K value for a reaction with a : compound that is acting as a base.
Kw: This is a constant!! At 25 degrees Celscius, it is 10ˆ-14 but it changes as temperature changes. This is the K value for water autoprotolysis.
Kc: Use this when you find the K value for a reaction (not including an acid or a base) and the units you're using is molarity
Kp: Use this when you find the K value for a reaction (not including an acid or a base) consisting of just gases and you have their partial pressures.
Note: you calculate all of these the same way. The notation is just different.
Ka: This is when you find the K value for a reaction with a compound that is acting as an acid.
Kb: This is when you find the K value for a reaction with a : compound that is acting as a base.
Kw: This is a constant!! At 25 degrees Celscius, it is 10ˆ-14 but it changes as temperature changes. This is the K value for water autoprotolysis.
Kc: Use this when you find the K value for a reaction (not including an acid or a base) and the units you're using is molarity
Kp: Use this when you find the K value for a reaction (not including an acid or a base) consisting of just gases and you have their partial pressures.
Note: you calculate all of these the same way. The notation is just different.
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Re: the different Ks
Hi!
K represents the equilibrium constant of a given reaction. There are different types of Ks because they are used for different reactions involving different substances.
Ka: equilibrium constant for reactions involving acids.
Kb: equilibrium constant for reactions involving bases.
Kw: equilibrium constant for water.
Kc: equilibrium constant for any reaction where reactants and products are at equilibrium (using concentration: mols/L)
Kp: equilibrium constant for reactions involving gases where reactants and products are at equilibrium (using partial pressure)
I hope this summary helped!!
K represents the equilibrium constant of a given reaction. There are different types of Ks because they are used for different reactions involving different substances.
Ka: equilibrium constant for reactions involving acids.
Kb: equilibrium constant for reactions involving bases.
Kw: equilibrium constant for water.
Kc: equilibrium constant for any reaction where reactants and products are at equilibrium (using concentration: mols/L)
Kp: equilibrium constant for reactions involving gases where reactants and products are at equilibrium (using partial pressure)
I hope this summary helped!!
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Re: the different Ks
Adding on to that
Kw can be used to calculate Ka and Kb when given two using the equation Kw=Ka*Kb
Kw can be used to calculate Ka and Kb when given two using the equation Kw=Ka*Kb
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