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Doss [256]
3 years ago
10

Enough of a monoprotic acid is dissolved in water to produce a 0.0147 M solution. The pH of the resulting solution is 2.46. Calc

ulate the pKa for the acid.
Chemistry
1 answer:
Lera25 [3.4K]3 years ago
6 0
First, we need to calculate Ka in order to determine the pKa. 

The formula for Ka = x^2/ initial concentration

initial concentration= 0.0147 M

we need to find x, and we can use the pH to find it because x is the [H+] concentration.

[H+]= 10^-pH----> [H+]= 10^-2.46= 0.00347 

Ka= x^2/ initial---------> (0.00347)^2/ 0.0147= 8.18 x 10^-4

now that we have Ka, we can determine pKa using the following formula--> pKa= -log Ka

pKa= -log (8.18 x 10^-4)= 3.087
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A certain volume of a gas had a pressure of 800 torr at a temperature of -40 degrees C. What was the original volume if the volu
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Now put all the given values in the above equation, we get:

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8 0
3 years ago
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rate_{NH_3}=\frac{2d[NH_3]}{dt}

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Explanation:

Hello there!

In this case, according to the law of rate proportions, it is possible to write the the rates of reaction for the formation of NH3 and the disappearance of the N2 and H2, by considering that the coefficient in the reaction for NH3 is +2 and those of N2 and H2, -1 and -3 respectively. Moreover, we set up these equations as derivatives as shown below:

a.

rate_{NH_3}=\frac{2d[NH_3]}{dt}

b.

rate_{N_2}=\frac{-1d[N_2]}{dt} \\\\rate_{H_2}=\frac{-3d[H_2]}{dt}

Best regards!

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