The reaction, in this case, would look something like this:
Now, since the initial concentration of the acid is given, we'll draw an ICE table:
[ClCH2COOH] | [ClCH2COO-] | [H3O+] | |
Initial Concentration | 2.25 M | 0 | 0 |
Change in Concentration | -x | +x | +x |
Equilibrium Concentration | (2.25 - x) M | x M | x M |
Now, we have to ascertain the value of Ka from the given value of pKa
Now, from the reaction, we can write the following relation:
From this we will get the following quadratic equation:
Solving this quadratic equation would give us the value of x, which is as follows:
So, the equilibrium concentrations of all the species are as follows:
[H3O+] = 0.0544 M
[ClCH2COO-] = 0.0544 M
[ClCH2COOH] = 2.25 - 0.0544 = 2.20 M
Now, we'll ascertain the pH of the solution:
Be sure to answer all parts. Chloroacetic acid, CICH,COOH, has a pK, of 2.87. What are...
2 attempts left Check my work Be sure to answer all parts. Chloroacetic acid, CICH,COOH, has a pK, of 2.87. What are H30*], pH, CICH,COO), and CICH,COOH) in 2.90 M CICH,COOH? [H3O+]= M aces [CICH,000 ] - [CICH,COOH) = pH =
Chloroacetic acid (CICH2COOH) has a pka = 2.87 What is the value of the equilibrium constant for this reaction: CICH,COOH(aq) + H2O(l) = CICHC00 (aq) + H3O+ (aq)? O A More information is needed to answer O B 6.43x10-5 o C 7.41x10-12 O D [math]1.35 x 10^{-3[/math] Unanswered Submit
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Be sure to answer all parts. In a 0.25 M solution, a weak acid is 3.6% dissociated. (a) Calculate the [H30+ ], pH, [OH ], and pOH of the solution. [H30+]= M [OH]= X 10 pH = pOH = (b) Calculate Kg of the acid. KA=
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Be sure to answer all parts. A 0.035 M solution of a weak acid (HA) has a pH of 4.39. What is the Ka of the acid?
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