Ka, Kb, and Kc
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Re: Ka, Kb, and Kc
Ka is used for acids. Kb is used for bases. And Kc is more general and used when calculating molar concentration as opposed to partial pressure, Kp, for a given reaction. For Ka, Kb, Kc and Kp, you would do [products]/[reactants]. For Ka you would do {H3O+][A-]/[HA] where A is the acid and H is the hydrogen atom attached to it. For Kb you would do [OH-][HB+]/[B]. Nonetheless, all of these follow the same general formula of [products]/[reactants], which is more general and how you would define Kc and Kp.
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Re: Ka, Kb, and Kc
Ka is used for acids. Kb is used for bases. And Kc is more general and used when calculating molar concentration as opposed to partial pressure, Kp, for a given reaction. For Ka, Kb, Kc and Kp, you would do [products]/[reactants]. For Ka you would do {H3O+][A-]/[HA] where A is the acid and H is the hydrogen atom attached to it. For Kb you would do [OH-][HB+]/[B]. Nonetheless, all of these follow the same general formula of [products]/[reactants], which is more general and how you would define Kc and Kp.
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Re: Ka, Kb, and Kc
KA specifically refers to the equilibrium constant for the dissociation of an acid, while KB specifically refers to the equilibrium constant for the dissociation of a base. KC has a broader definition and refers to any equilibrium constant that is calculated with molar concentrations of reactants and products.
Hopefully this helps and please correct me if there are any mistakes.
Hopefully this helps and please correct me if there are any mistakes.
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Re: Ka, Kb, and Kc
Ka is used when dealing with a chemical reaction that includes an acid and Kb is used when there is a chemical reaction that includes a base. Kc is the equilibrium constant of concentrations.
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Re: Ka, Kb, and Kc
Ka is the acidity equilibrium constant; the counterpart is Kb, which is the basicity equilibrium constant. Kc is the equilibrium constant described by molar concentration. Ka and Kb both belong to a kind of Kc.
Re: Ka, Kb, and Kc
In general, they are all equilibrium constants but a specifies it is for an acid, b specifies it is for a base, and c is more of a general K value just dealing with concentrations in general.
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Re: Ka, Kb, and Kc
You use Ka when dealing with acids, Kb when dealing with bases, and Kc when dealing with concentrations in general.
Re: Ka, Kb, and Kc
ka,kb, and kc are equilibrium constants.
More specifically, ka is for acids, kb is for bases, and kc is for concentrations.
More specifically, ka is for acids, kb is for bases, and kc is for concentrations.
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Re: Ka, Kb, and Kc
All of these terms are to describe equilibrium constants in a reaction. Ka is used for acids, Kb for bases, and Kc is a bit more general and just used for the concentration in general.
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Re: Ka, Kb, and Kc
Ka is used for acids, and similarly Kb is used for bases. These are specific to calculations when finding the pH of a solution or something related. Kc is more general as it represents the equilibrium constant for a reaction based on concentrations of molecules.
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Re: Ka, Kb, and Kc
They are all equilibrium constants,
ka is for acids, kb is for bases, and kc is for concentrations
ka is for acids, kb is for bases, and kc is for concentrations
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Re: Ka, Kb, and Kc
They all refer to equilibrium constants. Ka is for acids. Kb is for bases. Kc is a general term for concentration that could be used with acid or base concentration.
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