How would the titration curve of hydrochloric acid solution differ if barium hydroxide was used to titrate instead of sodium hydroxide?
How would the titration curve of hydrochloric acid solution with sodium hydroxide differ from the titration curve of acetic acid solution with sodium hydroxide?
No diagrams can be drawn on this forum. Can you rephrase your question. Alternately, I can look for some curves on the net but I doubt I can find one that exactly fits your needs.
So 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)
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?
To understand how the titration curve of hydrochloric acid solution would differ if barium hydroxide (Ba(OH)2) was used instead of sodium hydroxide (NaOH), and how it would differ from the titration curve of acetic acid (CH3COOH) solution with sodium hydroxide, we need to consider the chemical reactions that occur during titration.
1. Titration curve with barium hydroxide instead of sodium hydroxide:
In the case of hydrochloric acid (HCl) solution being titrated with barium hydroxide, the chemical reaction is represented as:
2HCl + Ba(OH)2 -> 2H2O + BaCl2
The reaction between hydrochloric acid and barium hydroxide forms water and barium chloride as products. The titration curve for this reaction would show a similar pattern as the titration curve with sodium hydroxide, with a steep rise in pH initially when the base (barium hydroxide) is added to the acid (hydrochloric acid). However, the equivalence point, where the acid and base react in stoichiometric proportions, may occur at a different pH value due to differences in the strength and concentration of the analyte and titrant.
2. Titration curve with hydrochloric acid solution and sodium hydroxide vs. acetic acid solution and sodium hydroxide:
The main difference between the titration curve of hydrochloric acid solution with sodium hydroxide and acetic acid solution with sodium hydroxide lies in the nature of the acid:
- Hydrochloric acid (HCl) is a strong acid that dissociates completely in water to form H+ ions. It reacts rapidly and completely with sodium hydroxide, resulting in a rapid and sharp pH change around the equivalence point, which is at pH 7 (neutral).
- Acetic acid (CH3COOH), on the other hand, is a weak acid that only partially dissociates in water to form H+ ions. The reaction between acetic acid and sodium hydroxide is represented as:
CH3COOH + NaOH -> CH3COONa + H2O
The reaction between acetic acid and sodium hydroxide forms sodium acetate and water as products. Since acetic acid is a weak acid, the titration curve will show a gradual increase in pH rather than a sudden change. The equivalence point would occur at a higher pH value, slightly above pH 7, indicating a weakly basic solution due to the presence of the acetate ion.
In summary, the titration curve of hydrochloric acid solution with barium hydroxide would show a similar pattern to that of sodium hydroxide but with a different equivalence point pH value. The titration curve of hydrochloric acid solution with sodium hydroxide would exhibit a sharp pH change at the equivalence point. The titration curve of acetic acid solution with sodium hydroxide would show a gradual pH increase and the equivalence point would occur at a slightly higher pH value.