Ammonium Hydroxide Concentration
Ammonium Hydroxide Concentration - Related Videos
09:50
Electrochemically and Bioelectrochemically Induced Ammonium Recovery
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Cited by 31 •
2015
We demonstrate the extraction of ammonium from an ammonium-rich stream using an electrochemical and a bioelectrochemical system. The reactor setup, operation and data analysis are discussed.
14:48
Acid and Base Concentrations - Student Protocol
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2020
Source: Smaa Koraym at Johns Hopkins University, MD, USA Preparation of ~0.1 M NaOHExpand In the first part of the lab, you will use a 50% w/w solution of NaOH to prepare 500 mL of ~0.1 M. The 50% w/w NaOH is indicative of its weight ratio. For example, if the instructor prepared 150 mL of the 50% w/w NaOH solution, then 150 g of NaOH was dissolved in 150 g of water, and the total weight of the solution is 300 g. To begin, put on the appropriate personal protective equipment,...
06:35
Acid and Base Concentrations - Concepts
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2020
Acids and Bases An Arrhenius acid produces hydrogen ions when it is dissolved in water: HA + H2O → H+(aq) + A-(aq) Here, HA is the non-dissociated acid, H+ is the hydrogen cation, and A- is the solvated anion — called the conjugate base. An Arrhenius base produces hydroxide ions when dissolved in water: BOH + H2O → B+(aq) + OH-(aq) Here, BOH is the non-dissociated base, OH- is the hydroxide ion, and B+ is the solvated cation — called the conjugate acid. A conjugate base is formed when an acid...
05:17
Acid and Base Concentrations - Instructor Prep
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2020
Source: Smaa Koraym at Johns Hopkins University, MD, USA Preparation of ReagentsExpand Here, we show the laboratory preparation for 10 students working in pairs, with some excess. Please adjust quantities as needed. Prepare 25 mL of 50% w/w NaOH solution. Weigh 25 g of NaOH pellets and add them to a 125-mL Erlenmeyer flask. Measure 25 mL of deionized water and add it to the flask. Add a magnetic stir bar and mix the solution on a stir plate until the solution appears...
01:25
Isolation of Ammonium-Oxidizing Iron Reducers from a Wetland Soil–Derived Enrichment Culture
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2025
Begin with a wetland soil-derived enrichment culture containing bacterial communities.The culture exhibits Feammox activity, ammonium oxidation coupled to ferric iron reduction, indicating the enrichment of a bacterium capable of this metabolic process.Serially dilute the culture using media.Streak the diluted samples onto test agar plates supplemented with ferric iron and ammonium.Use control plates that lack either ferric iron or ammonium, or contain ferric iron with organic carbon instead of...
FAQs
Changing the concentration alters the balance in the reversible reaction between ammonia, water, ammonium, and hydroxide ions. This changes the extent of ionization rather than converting all dissolved ammonia into ions. As a result, solutions with different concentrations can show different chemical behavior, including differences in pH and alkalinity.
The equilibrium produces hydroxide ions, which give the solution its basic character. A change in concentration changes the amount of ammonia available for this reversible ionization and therefore affects hydroxide formation. Monitoring concentration is consequently important when a procedure requires a controlled pH, a predictable alkaline environment, or reproducible acid–base behavior.
These expressions represent concentration in different reporting formats. Molarity describes the amount in relation to solution volume, mass percent expresses the amount as a percentage by mass, and normality reports concentration in terms relevant to reactive capacity. Selecting one format matters because preparation, labeling, and calculations must use compatible concentration information.
Begin with a solution whose concentration is known, determine the dilution needed for the target concentration, and combine the measured solution with an appropriate amount of water. The resulting preparation should be mixed and labeled with its concentration. Accurate dilution is essential because concentration controls the solution’s subsequent chemical behavior.
Controlled concentration supports several laboratory uses, including acid–base titrations, buffer preparation, qualitative analysis, and precipitation reactions. In each case, the concentration helps establish the intended basic conditions and improves consistency between samples. It also allows observations or reaction outcomes to be interpreted in relation to a known chemical environment.
Concentrated solutions require careful handling because they release irritating ammonia vapors and are strongly basic. Preparation should therefore include accurate dilution, clear labeling, and attention to the solution’s concentration before use. These practices help maintain the intended composition while reducing risks associated with exposure and unintended contact during chemical work.