Lactic acid HC3H5O3 has one acidic hydrogen. A 0.10 M solution of lactic acid has the concentration of hydronium ion of 0.00363 M. Calculate Ka for lactic acid?
All you have to do in order to find the value of the acid dissociation constant,
Being a weak acid, lactic acid will not dissociate completely to form lactate,
Use an ICE table to help you find the equilibrium concentration of the lactic acid
#" ""HC"_3"H"_5"O"_text(3(aq]) + "H"_2"O"_text((l]) rightleftharpoons "C"_3"H"_5"O"_text(3(aq])^(-) + "H"_3"O"_text((aq])^(+)#
By definition, the acid dissociation constant will be equal to You know that the equilibrium concentration of hydronium ions is This means that the equilibrium concentration of the lactic acid will be This means that the value of the acid dissociation constant will be Rounded to two sig figs, the number of sig figs you have for the molarity of the lactic acid solution, the answer will be
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Ka for lactic acid: 3.63 x 10^-3.
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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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- A sample of carbon is placed in a rigid 1.50 L flask. Dinitrogen monoxide is added and the flask heated to 800C. When the system reached equilibrium the partial pressure of the carbon dioxide is found to be 0.030 atm and the partial pressure of the dinitrogen monoxide to be 1.48 atm. What is the partial pressure of nitrogen in the mixture.
- How do you determine Ka?

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