Acid-base Titration
Acid-base Titration - Related Videos
02:23
Acid-Base Titration Curves
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2020
A titration curve is a plot of some solution property versus the amount of added titrant. For acid-base titrations, solution pH is a useful property to monitor because it varies predictably with the solution composition and, therefore, may be used to monitor the titration’s progress and detect its endpoint. Acid-base titration can be performed with a strong acid and a strong base, a strong acid and a weak base, or a strong base and a weak acid. For a titration carried out for 25.00 mL of 0.100...
03:55
Titration Calculations: Weak Acid - Strong Base
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2020
Calculating pH for Titration Solutions: Weak Acid/Strong Base For the titration of 25.00 mL of 0.100 M CH3CO2H with 0.100 M NaOH, the reaction can be represented as: The pH of the titration solution after the addition of the different volumes of NaOH titrant can be calculated as follows: (a) The initial pH is computed for the acetic acid solution in the usual ICE approach: (b) The acid and titrant are both monoprotic and the sample and titrant solutions are equally concentrated; thus, this...
02:28
Titration Calculations: Strong Acid - Strong Base
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2020
Calculating pH for Titration Solutions: Strong Acid/Strong Base A titration is carried out for 25.00 mL of 0.100 M HCl (strong acid) with 0.100 M of a strong base NaOH. The pH at different volumes of added base solution can be calculated as follows: (a) Titrant volume = 0 mL. The solution pH is due to the acid ionization of HCl. Because this is a strong acid, the ionization is complete and the hydronium ion molarity is 0.100 M. The pH of the solution is then: (b) Titrant volume = 12.50 mL.
02:08
Titration of a Polyprotic Acid
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2020
A polyprotic acid contains more than one ionizable hydrogen and undergoes a stepwise ionization process. If the acid dissociation constants of the ionizable protons differ sufficiently from each other, then the titration curve for such polyprotic acid generates a distinct equivalence point for each of its ionizable hydrogens. Therefore, titration of a diprotic acid results in the formation of two equivalence points, whereas the titration of a triprotic acid results in the formation of three...
01:29
Conductometric Titrations: Strong Acid-Base and Weak Acid-Base Titrations
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2026
In acid-base titrations, conductance measurements are utilized to detect the endpoint. This method is grounded on the fact that electrical conductance relies on the number and mobility of ions. For instance, consider titrating strong acid HCl with a strong NaOH base. Initially, the HCl in the conductivity vessel conducts electricity due to the presence of hydrogen ions and chloride ions. As NaOH is gradually added from the burette, the fast-moving hydrogen ions are replaced by slower-moving...
FAQs
The equivalence point is the stoichiometric target, whereas the endpoint is the experimental signal used to locate it. At equivalence, acid and base have reacted in the proportions specified by the balanced equation. The endpoint appears when an indicator changes color or a pH electrode records a sharp pH variation, so accuracy depends on how closely that signal represents equivalence.
Stoichiometry connects the measured amount of standard solution with the unknown concentration. The balanced chemical equation establishes how many reacting species neutralize one another, allowing the added volume and known concentration to be interpreted quantitatively. This relationship converts an observed titration result into a concentration value rather than merely showing that neutralization occurred.
An indicator and a pH electrode detect the endpoint in different ways. The indicator provides a visible color change, while the electrode provides an instrumental record of pH and can reveal a sharp variation during addition. Selecting between them depends on whether visual observation or direct pH monitoring better identifies the experimental transition.
Gradual addition allows changes in acid-base behavior to be followed as the reaction proceeds. Near the stoichiometric point, a sharp pH variation can signal that the system is approaching the endpoint. Adding the standard solution incrementally supports controlled observation and reduces the chance of passing the informative transition without detecting it.
A typical workflow begins with a solution whose concentration is to be determined and a standard acid or base of known concentration. The standard solution is added gradually while an indicator or pH electrode monitors the reaction. The endpoint signal is then related to the balanced equation to determine the unknown concentration.
Chemists apply acid-base titration wherever concentration measurements are required, including reaction analysis, quality control, and laboratory investigations of acid-base behavior. Its value extends beyond a single measurement: the endpoint supplies an experimentally observable marker, while stoichiometric interpretation connects that marker with the composition of the solution being studied.