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Related Concept Videos

Weak Acid Solutions04:02

Weak Acid Solutions

42.4K
Few compounds act as strong acids. A far greater number of compounds behave as weak acids and only partially react with water, leaving a large majority of dissolved molecules in their original form and generating a relatively small amount of hydronium ions. Weak acids are commonly encountered in nature, being the substances partly responsible for the tangy taste of citrus fruits, the stinging sensation of insect bites, and the unpleasant smells associated with body odor. A familiar example of a...
42.4K
Titration Calculations: Weak Acid - Strong Base03:55

Titration Calculations: Weak Acid - Strong Base

49.1K
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:
49.1K
Titration of a Weak Acid with a Weak Base01:08

Titration of a Weak Acid with a Weak Base

4.9K
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...
4.9K
Titration of a Weak Acid with a Strong Base01:30

Titration of a Weak Acid with a Strong Base

4.4K
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...
4.4K
Titration of a Weak Base with a Strong Acid01:20

Titration of a Weak Base with a Strong Acid

8.7K
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...
8.7K
Weak Base Solutions03:21

Weak Base Solutions

24.9K
Some compounds produce hydroxide ions when dissolved by chemically reacting with water molecules. In all cases, these compounds react only partially and so are classified as weak bases. These types of compounds are also abundant in nature and important commodities in various technologies. For example, global production of the weak base ammonia is typically well over 100 metric tons annually, being widely used as an agricultural fertilizer, a raw material for chemical synthesis of other...
24.9K

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Related Experiment Video

Updated: Jan 23, 2026

Fabrication Procedures and Birefringence Measurements for Designing Magnetically Responsive Lanthanide Ion Chelating Phospholipid Assemblies
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Fabrication Procedures and Birefringence Measurements for Designing Magnetically Responsive Lanthanide Ion Chelating Phospholipid Assemblies

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Process for lanthanides-Y leaching from phosphogypsum fertilizers using weak acids.

M S Gasser1, Z H Ismail1, E M Abu Elgoud1

  • 1Hot Laboratories Center, Atomic Energy Authority, Post Code 13759, Egypt.

Journal of Hazardous Materials
|June 22, 2019
PubMed
Summary

This study shows citric acid effectively leaches lanthanides and yttrium (Ln-Y) from phosphogypsum fertilizer (PGF). Optimized three-cycle leaching achieved 83.4% Ln-Y recovery, with high selectivity for certain rare earth elements.

Keywords:
Lanthanides-YLeachingPhosphogypsum fertilizerWeak acids

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Area of Science:

  • Environmental Chemistry
  • Inorganic Chemistry
  • Materials Science

Background:

  • Phosphogypsum (PG) is a major industrial byproduct containing valuable lanthanides and yttrium (Ln-Y).
  • Modified PG is utilized as phosphogypsum fertilizer (PGF), retaining significant Ln-Y content.
  • Efficient recovery of Ln-Y from PGF is crucial for resource utilization and environmental management.

Purpose of the Study:

  • To investigate the leaching efficiency of Ln-Y from PGF using various weak organic acids.
  • To optimize citric acid leaching parameters for maximum Ln-Y recovery.
  • To develop a multi-cycle leaching process for enhanced Ln-Y extraction.

Main Methods:

  • Leaching experiments were conducted using boric, malic, and citric acids at varying concentrations and retention times.
  • Optimized citric acid leaching involved adjusting acid concentration, liquid-to-solid ratio (L/S), retention time (Rt), and temperature.
  • A three-cycle leaching flow sheet was designed and evaluated for overall Ln-Y recovery.

Main Results:

  • Citric acid demonstrated superior leaching efficiency for Ln-Y compared to boric and malic acids.
  • Optimized conditions (1.0 mol/L citric acid, L/S=5.0, Rt=15 min, 358 K) in one cycle recovered 53.3% of total Ln-Y.
  • A three-cycle process achieved a maximum leaching efficiency of 83.4% for total Ln-Y.
  • Citric acid exhibited selective leaching, with high recovery for Er, Ce, and La, and lower recovery for Pr and Y.

Conclusions:

  • Citric acid is a highly effective lixiviant for recovering lanthanides and yttrium from phosphogypsum fertilizer.
  • A multi-cycle leaching strategy significantly enhances the overall recovery of valuable Ln-Y elements.
  • The developed process offers a promising route for the valorization of phosphogypsum waste, recovering critical rare earth elements.