If two titrations were completed were completed: 1) the titration of HCl with Na(OH) 2)the titration of HCl with Ba(OH)2 (the concentrations of acid and base for both titrations are the same)
How would the titration curves of each solution be different?
I know what the titration curve of the first one looks like, but compared to the second one what would it be? How would the curves look different? Would the initial pH be higher/lower/same? Would the final pH be higher/lower/same?
Starting with HCl and titrating with Ba(OH)2, I don't think the curves would be that different. You are starting with HCl so the initial pH would be the same. Ba(OH)2 is a strong base, too, so the equivalence point will be the same. The pH after the equivalence point should look about the same since it's a strong base in excess. The only thing I can think of that would be a little different is that you are adding more hydroxide ions with each drop of Ba(OH)2 than with NaOH so the line connecting the starting point and the equivalence point would be shorter.
I looked on the web for one but couldn't find one i liked.
To understand how the titration curves of the two solutions would be different, we need to consider the reactions involved in each titration.
1) Titration of HCl with Na(OH):
HCl + NaOH → NaCl + H2O
2) Titration of HCl with Ba(OH)2:
HCl + Ba(OH)2 → BaCl2 + 2H2O
In both cases, the reaction involves a strong acid (HCl) and a strong base (NaOH or Ba(OH)2). This means that the initial pH of both solutions would be very low (acidic) since HCl is a strong acid.
However, there are some key differences between the two titration curves:
1) NaOH is a monoprotic base, which means it donates only one hydroxide ion (OH-) per molecule. As a result, in the titration of HCl with NaOH, the equivalence point is reached when all the HCl has reacted with an equal amount of NaOH on a 1:1 mole ratio. The pH at the equivalence point will be around 7 (neutral) since the solution will contain equal amounts of the strong acid and base.
2) Ba(OH)2 is a diprotic base, which means it donates two hydroxide ions (OH-) per molecule. In the titration of HCl with Ba(OH)2, the pH at the first equivalence point (when 1 mole of HCl has reacted with 1 mole of Ba(OH)2) will be around 9, slightly basic. This is because, at this point, there is still some excess hydroxide ions (OH-) from the Ba(OH)2.
The final pH of each solution depends on the amount of acid and base present. If the titrations were conducted using the same concentrations of acid and base, the final pH should be similar in both cases but may vary slightly due to the difference in the nature of the metal salt formed (NaCl vs. BaCl2). However, if the concentrations of acid and/or base are different for the two titrations, the final pH may differ.
To summarize:
- The initial pH for both solutions would be very low (acidic).
- The titration curve for the HCl and Na(OH) solution would have an equivalence point close to a pH of 7 (neutral).
- The titration curve for the HCl and Ba(OH)2 solution would have an initial pH close to 9 (basic) due to the excess OH- in the diprotic base.
- The final pH would depend on the concentrations of the acid and base used.