If you are aiming for a specific pH they require less of a base.
If you need to simply full titrate it, it depends on how much of the acid you have, not how strong it is.
The pH at the endpoint of a titration depends on the nature of the acids and bases involved. Usually, for a strong acid-strong base titration, the pH at the endpoint is around 7 due to the neutralization of the acid and base. For weak acid-strong base titrations, the pH may be greater than 7, while for weak base-strong acid titrations, the pH may be less than 7.
The stoichiometric point for a weak acid-strong base titration is generally greater than pH 7 because the titration involves adding a strong base (like NaOH) to a weak acid solution. At the stoichiometric point, all of the weak acid has been neutralized by the strong base, resulting in the formation of the conjugate base and water, which makes the solution slightly basic.
In an acid-base titration, the substance being titrated is typically less abundant or more prone to contamination than the titrant. By placing the acid in the burette and titrating it with a base, the volume of base required to reach the equivalence point can be precisely measured and controlled. This setup allows for accurate determination of the concentration of the acid being titrated.
Because it only partly ionises because it has less H+ ions so the reaction is not as fast, therefore the titration is easier to do becasue you have more time to see when it has reached neutral etc Edit: This answer is entirely incorrect. NEVER use a weak acid or a weak base as the titrant. Doing so will result in the formation of a buffer during the titration, and no useful information can be gained.
pH plays a crucial role in titration as it helps determine the endpoint of the reaction. The pH at the equivalence point depends on the acid-base reaction being titrated. For strong acid-strong base titrations, the pH at the equivalence point is 7; for weak acid-strong base titrations, the pH is greater than 7; and for weak base-strong acid titrations, the pH is less than 7. pH indicators can also be used to visually show the endpoint of the titration based on color change.
The pH at the endpoint of a titration depends on the nature of the acids and bases involved. Usually, for a strong acid-strong base titration, the pH at the endpoint is around 7 due to the neutralization of the acid and base. For weak acid-strong base titrations, the pH may be greater than 7, while for weak base-strong acid titrations, the pH may be less than 7.
Bases tend to recieve an H+ ion in a titration, and acids tend to give an H+ ion in a titration. Bases have a pH greater than 7 and acids have a pH less than 7.
The stoichiometric point for a weak acid-strong base titration is generally greater than pH 7 because the titration involves adding a strong base (like NaOH) to a weak acid solution. At the stoichiometric point, all of the weak acid has been neutralized by the strong base, resulting in the formation of the conjugate base and water, which makes the solution slightly basic.
In an acid-base titration, the substance being titrated is typically less abundant or more prone to contamination than the titrant. By placing the acid in the burette and titrating it with a base, the volume of base required to reach the equivalence point can be precisely measured and controlled. This setup allows for accurate determination of the concentration of the acid being titrated.
Because it only partly ionises because it has less H+ ions so the reaction is not as fast, therefore the titration is easier to do becasue you have more time to see when it has reached neutral etc Edit: This answer is entirely incorrect. NEVER use a weak acid or a weak base as the titrant. Doing so will result in the formation of a buffer during the titration, and no useful information can be gained.
they are more because they are
pH plays a crucial role in titration as it helps determine the endpoint of the reaction. The pH at the equivalence point depends on the acid-base reaction being titrated. For strong acid-strong base titrations, the pH at the equivalence point is 7; for weak acid-strong base titrations, the pH is greater than 7; and for weak base-strong acid titrations, the pH is less than 7. pH indicators can also be used to visually show the endpoint of the titration based on color change.
If I remember correctly, bases have low pH and acids have high pH; therefore, a base would definitely be less than 7.
1. If acids other than the acetic acid were present in the vinegar, it would be difficult to determine the percent of just the acetic acid, since it would be mixed with another acid.
Carboxylic acids are stronger acids due to the more stable conjugate base formed after donation of a proton. The presence of the highly electronegative carbonyl group helps stabilize the negative charge on the conjugate base. In contrast, 2-naphthol is less acidic as the conjugate base formed lacks this stabilizing effect.
no acids are higher than seven and bases are lower than seven
There are three major differences between strong acid/strong base and weak acid/strong base titrations. For weak acid/strong base titrations: 1. The weak-acid solution has a higher initial pH. 2. The pH rises more rapidly at the start, but less rapidly near the equivalence point. 3. The pH at the equivalence point does not equal 7.00. (should be >7) In an acid-base titration, there is a 1:1 acid:base stoichiometry, so the equivalence point is the point where the moles of titrant added equals the moles of substance initially in the solution being titrated. Therefor the strength of the acid or base should not have an affect on the quantity of base required, only on the pH of the equivalence point. The number of moles of titrant and solution will have an effect on the quantity of base required.