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Titration of a Weak Base with a Strong Acid01:20

Titration of a Weak Base with a Strong Acid

4.7K
The titration curve of a weak base like ammonia with a strong acid like hydrochloric acid is the mirror image of the titration curve of a weak acid with a strong base.
Using the ICE table and substituting the Kb value, we calculate the initial pH of 50 mL of 0.1 M ammonia to be 11.11. Addition of 25 mL of 0.1 M hydrochloric acid to this solution of ammonia results in a buffer with an equal concentration of ammonia and ammonium ions. The pH of this buffer can be calculated by substituting these...
4.7K
Titration of a Weak Acid with a Strong Base01:30

Titration of a Weak Acid with a Strong Base

2.2K
In titrating a weak acid with a strong base, different calculation methods are applied at various stages. Initially, the pH of a weak acid like acetic acid is calculated using its dissociation constant (Ka) and an ICE table. Upon addition of a strong base such as sodium hydroxide, a buffer forms, and its pH is determined using the Henderson-Hasselbalch equation. As more base is added and the titration reaches the halfway point, the pH becomes equal to the pKa of the acid, indicating equal...
2.2K
Titration Calculations: Weak Acid - Strong Base03:55

Titration Calculations: Weak Acid - Strong Base

44.2K
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:
44.2K
Instrument Calibration01:12

Instrument Calibration

170
Instrument calibration is essential for ensuring that instruments produce accurate and consistent results. It is vital in manufacturing, healthcare, testing laboratories, and scientific research. Calibration processes are specific to each instrument and help enhance data accuracy. Each instrument has a unique calibration process tailored to its design and function to improve data accuracy.
Analytical Balance Calibration
An analytical balance measures mass and requires regular calibration to...
170
Titration of a Weak Acid with a Weak Base01:08

Titration of a Weak Acid with a Weak Base

2.8K
Weak acids and bases do not undergo dissociation completely, and titrations between these two are rarely studied. When such studies are performed, say, for the titration of a weak acid with a weak base, the titration curve plots the change in pH as a function of the volume of base added. Take the titration of acetic acid with ammonia, for instance. During the titration, these two species form ammonium acetate and water, but the pH change is slow and gradual.
As a result, there is no simple...
2.8K
Titration Calculations: Strong Acid - Strong Base02:28

Titration Calculations: Strong Acid - Strong Base

29.5K
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:
29.5K

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Measuring Enzymatic Stability by Isothermal Titration Calorimetry
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Calibrating ITC instruments: Problems with weak base neutralization.

Žiga Medoš1, Marija Bešter-Rogač1, Epameinondas Leontidis2

  • 1Faculty of Chemistry and Chemical Technology, University of Ljubljana, Večna pot 113, 1000, Ljubljana, Slovenia.

Analytical Biochemistry
|July 8, 2024
PubMed
Summary
This summary is machine-generated.

Accurate isothermal titration calorimetry (ITC) calibration requires accounting for titrant volume loss, especially in precise measurements. A variable-volume protocol helps correct for diffusive HCl loss from the syringe tip, improving heat factor accuracy.

Keywords:
Acid-base reactionCalibrationCalorimetryDiffusionIsothermal titration calorimetry

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Area of Science:

  • Analytical Chemistry
  • Biophysical Chemistry

Background:

  • Isothermal titration calorimetry (ITC) instruments offer high precision but require chemical calibration for accuracy.
  • The reaction of hydrochloric acid (HCl) into the weak base TRIS is a standard method for determining the heat factor.

Purpose of the Study:

  • To investigate calibration issues with modern ITC instruments, specifically focusing on the HCl/TRIS reaction.
  • To identify and quantify sources of error affecting accuracy in ITC measurements.

Main Methods:

  • Utilized VP-ITC and two Nano-ITCs for calibration experiments.
  • Employed a variable-titrant-volume protocol to detect and correct for titrant loss.
  • Performed mathematical modeling to analyze diffusive loss of HCl from the syringe tip.
  • Estimated data variance functions from replicate data for improved least-squares fitting.

Main Results:

  • Observed a significant titrant volume shortfall (Δv ≈ 0.3 μL) attributed to HCl diffusion from the syringe tip.
  • Demonstrated the effectiveness of the variable-volume protocol in accounting for this shortfall.
  • Found that carbonate contamination and weak base hydrolysis can introduce substantial errors.
  • Quantified low-signal precision (σ ≈ 1 μJ) and titrant volume uncertainty across different instruments.

Conclusions:

  • The diffusive loss of titrant is a critical factor impacting ITC accuracy and necessitates a variable-volume protocol for precise calibration.
  • Standard calibration protocols may be insufficient due to unaddressed sources of error like diffusion, contamination, and hydrolysis.
  • Accurate determination of heat factors requires careful consideration of these systematic errors and instrument-specific uncertainties.