Br- in water - 1000μg/ml ±1% (20℃)

Cat. No.: B299455

GRADE & PURITY 1000μg/ml ±1% (20℃)

Storage

Store at 2-8°C

Shipped In

Wet ice

Specifications

Specifications & Purity

1000μg/ml ±1% (20℃)

Storage

Store at 2-8°C

Shipped In

Wet ice

This product requires cold chain shipping. Ground and other economy services are not available.

Application Protocols

Not applicable to this product. No immunoassay or bioassay application validations (e.g., WB, IHC, IF, FC) are associated with an aqueous bromide solution. For analytical uses such as IC or ISE calibration, follow your laboratory’s validated SOPs and the lot‑specific CoA for concentration and uncertainty.

Biological Roles

General literature context (no clinical claims):

• Bromide is a ubiquitous inorganic anion in extracellular fluids and seawater; transported via anion channels and exchangers that also handle chloride (e.g., CFTR, SLC families).
• Redox biochemistry: In the presence of peroxidases and hydrogen peroxide, Br− can be oxidized to hypobromous acid (HOBr), a reactive halogenating agent that participates in innate chemical defenses and post‑translational modifications in certain organisms (literature).
• Enzymology: Some haloperoxidases and halogenases display substrate preferences among halides; bromide often shows intermediate reactivity between chloride and iodide.
• Structural/biophysical uses: Bromide salts (e.g., KBr, NaBr) are commonly used as heavy‑atom soaks or anomalous scatterers in macromolecular crystallography (SAD/MAD phasing), taking advantage of Br absorption edges (literature). An aqueous bromide solution can facilitate such soaks with controlled ionic strength.
• Cell systems: Elevated halide concentrations can modulate membrane potentials and transporter activity in vitro; design experiments with appropriate osmolarity and counter‑ions to avoid off‑target effects.

Note: The specific suitability of this product for biological applications depends on its (unspecified) concentration, counter‑ion, sterility/endotoxin levels, and impurity profile. For cell‑ or enzyme‑based work, verify bioburden, trace metals, and pH on the CoA or perform in‑house qualification.

Buffer Applications

Bromide ion does not constitute a buffering system (Br− is the conjugate base of a strong acid, HBr) and does not provide meaningful pH control.

Relevant aqueous roles (general/literature):

• Ionic strength adjustment: Useful for tuning ionic strength independently of common buffer anions; can reduce activity‑coefficient effects in kinetic or binding assays. Choose counter‑ions (e.g., Na+, K+, choline+) to match biological systems or avoid interference.
• Hofmeister effects: Halides influence protein stability and solubility in the order I− > Br− > Cl− for chaotropicity; bromide is moderately chaotropic and may affect folding, aggregation, or phase behavior at high concentrations.
• Electrophoresis/capillary methods: As a background electrolyte component or displacement ion in certain separations; ensure detection compatibility.

Practical guidance

• Maintain primary pH control with standard buffers (e.g., phosphate, HEPES, Tris). Add bromide only for its ionic or specific halide effects.
• Verify that bromide does not interfere with assay readouts (e.g., halogen‑sensitive redox indicators, haloperoxidase assays).

Item-specific note: Buffer‑relevant parameters (concentration, pH, counter‑ion, conductivity) are not specified for this item; refer to CoA/Spec Sheet.

Green Alternatives

Greener considerations focus on preparation, transport, and waste minimization rather than substitution of the bromide function itself.

• On‑site preparation

  • Preparing bromide solutions in‑house from solid NaBr or KBr and purified water reduces shipping weight/volume and cold‑chain requirements, lowering scope‑3 emissions. Trade‑off: requires validated balances, Class A glassware, and metrological control to achieve the same concentration accuracy as supplier‑prepared standards.

• Concentrate vs. ready‑to‑use

  • Using higher‑concentration stock solutions and diluting at point of use reduces packaging. Trade‑off: viscosity/conductivity and density change with concentration; accurate volumetry/gravimetry is needed.

• Container choice

  • Select recyclable HDPE or glass; avoid unnecessary secondary plastics. Ensure closures are halogen‑compatible and low‑leachables.

• Process and waste

  • Aqueous halide waste is generally benign compared to organic halogenated solvents; avoid creating oxidized bromine species (Br2/BrO−) by segregating from oxidants. Neutral, salt‑rich aqueous waste may be amenable to down‑the‑drain disposal where permitted.

Illustrative comparison (general)

• Ready‑to‑use aqueous Br− solution
  • Pros: Lot‑certified concentration; time savings; reduced analyst variability.
  • Cons: Cold shipping (as specified here), more packaging/shipping mass per mole of Br−.
• Solid bromide salt + on‑site preparation
  • Pros: Minimal shipping mass; flexible concentrations; no cold chain.
  • Cons: Requires high‑purity water, cleanroom/controlled environment to match analytical grades; documentation burden for regulated labs.

Pharmaceutical Uses

No therapeutic claims are made. The product is for research use only (per Product Data).

Formulation/manufacturing context (general/literature):

• Analytical standards: Aqueous bromide solutions are used in QC laboratories as calibration/linearity standards for ion chromatography, titrimetric or potentiometric assays that quantify bromide as an impurity or residual from manufacturing processes.
• Process reagents: Halide ions are sometimes employed in process development to modulate catalyst speciation or reaction rates; bromide activity may be adjusted in aqueous stages to influence phase behavior or extraction efficiency.
• Excipient status: Bromide salts are not common pharmaceutical excipients in modern formulations; where halides are present, chloride is far more typical. Any use of bromide in GMP settings requires appropriate pharmacopeial conformance and documentation.

Practical notes

• For validated methods, use lot‑specific CoA values for concentration and uncertainty; bracketing standards should be prepared gravimetrically where possible.
• Confirm counter‑ion identity, bioburden/endotoxin, and leachables from packaging if the solution is used near drug substance operations.

Item-specific note: Grade/purity and concentration are not specified for this item; consult the CoA/Spec Sheet to determine suitability for regulated applications.

Physical Properties

Item-specific physico-chemical specifications (bp, mp, density, concentration, refractive index, conductivity, pH, counter‑ion identity) are not specified for this item; refer to CoA/Spec Sheet.

General/literature context for aqueous bromide solutions (non‑spec, qualitative unless noted):

• Physical state: Clear, colorless aqueous solution when uncontaminated; any yellow/brown tint may indicate oxidation to molecular bromine or tribromide.
• Solubility: Bromide salts of alkali metals are highly water‑soluble; solubility and activity coefficients depend on the counter‑ion and temperature.
• pH: Neutral to slightly acidic/basic depending on preparation; Br− itself is the conjugate base of a strong acid (HBr) and does not hydrolyze appreciably (literature).
• Density and refractive index: Increase with concentration; often used empirically to estimate concentration with a calibration curve (literature practice).
• Boiling/freezing behavior: As an electrolyte solution, exhibits boiling‑point elevation and freezing‑point depression proportional to molality (colligative properties, literature).
• Vapor pressure: Essentially that of water; volatile bromine is not present unless oxidized.
• Partitioning: Br− is strongly hydrophilic; negligible partition into nonpolar phases (literature).
• Conductivity: Increases with concentration; molar conductivity follows Kohlrausch’s law at low ionic strength, deviating at higher concentrations (literature).

Practical notes

• If precise physical values are required (e.g., for refractometric or densimetric standardization), obtain the lot‑specific concentration and counter‑ion from the CoA and consult corresponding property tables.

Quality & Grades

• Item-specific grade/purity: Not specified for this item; refer to CoA/Spec Sheet.

How to interpret grade for aqueous bromide solutions (general guidance):

• Analytical/Volumetric grade
  • Tight concentration tolerance (e.g., ±0.5–1.0%), low trace metal and organic carbon background, and low UV absorbance—suited for IC, ISE calibration, or spectrophotometric assays.
• ACS/AR grade base salt (used to prepare solution)
  • Meets ACS specifications for impurities; when dissolved with high‑purity water (18 MΩ·cm) and filtered, yields solutions appropriate for many analytical tasks.
• ICP/Trace metal grade
  • Controlled sub‑ppm metal background for trace analyses; containers and processing are metal‑free to minimize contamination.
• Biochemistry/Molecular biology grade
  • Low bioburden and endotoxin; sterile filtration and preservative policies vary by supplier.

What matters for this product type

• Counter‑ion identity and concentration accuracy directly affect ionic strength, activity coefficients, and analytical response in ion chromatography or potentiometry.
• Trace impurities (iodide, chloride, sulfate, organic carbon, and transition metals) can bias methods that rely on redox or complexation chemistry.
• Microbial control: Cold storage (2–8°C, as specified) and closed sterile processing reduce bioburden and degradation from microbial byproducts.
• Documentation: For regulated or validated workflows, request the lot‑specific CoA detailing concentration, uncertainty, counter‑ion, grade definition, and impurity profile.

Reaction & Applications

Applications for aqueous bromide (general/literature; verify suitability for your use):

• Analytical chemistry
  • Calibration standards for bromide determination by ion chromatography (IC), capillary electrophoresis, or ion‑selective electrodes (ISE). Ready‑to‑use solutions reduce preparation variability; confirm concentration and counter‑ion on the CoA.
  • Matrix matching/ionic strength adjustment in potentiometry and electrophoresis to improve precision.
• Redox and photochemistry
  • Br− is readily oxidized (E° ≈ +1.07 V for Br2/Br− vs NHE, literature) to Br2/Br3−; exploited in bromination reactions or as a redox mediator.
  • In photocatalysis, Br− can serve as a halide reservoir, forming Br•/Br2 under irradiation/oxidation, enabling selective benzylic or allylic bromination in aqueous or biphasic media.
• Phase-transfer catalysis (PTC)
  • With quaternary ammonium/phosphonium salts, aqueous Br− participates in SN1/SN2 substitutions and halide exchanges by shuttling Br− into the organic phase.
• Kinetics/mechanistic studies
  • Acts as a nucleophile or scavenger; used to probe radical or electrophilic intermediates; tribromide formation offers convenient UV–vis signatures (λmax ~266–270 nm, literature) for monitoring.

Practical tips

• Maintain inert conditions and exclude oxidants when Br− should remain reduced; conversely, introduce controlled oxidants (e.g., bromine generation in situ) in a hood when bromination is desired.
• Control pH and ionic strength; buffer components can complex oxidants and suppress bromination pathways.
• Verify metal content if using in catalysis sensitive to halides/trace metals (e.g., Pd, Cu).

Reaction Conditions

The following are general, literature‑based conditions where aqueous bromide is employed; they are NOT product‑specific specifications.

• In situ bromination (aqueous)

  • Reagents: Br− (aqueous), oxidant (e.g., H2O2 with acid, or bromine generated electrolytically), optional buffer.
  • Solvent: Water or water/MeOH, water/MeCN.
  • Temperature: 0–40°C; cooling recommended to control exotherm and selectivity.
  • Notes: Monitor for Br2/Br3− by UV–vis (λmax ~266–270 nm). Quench residual oxidant with sulfite/thiosulfate.

• PTC halide exchange/substitution

  • Reagents: Aqueous Br−, organic substrate (alkyl chloride/tosylate), quaternary ammonium/phosphonium catalyst.
  • Solvent: Biphasic water/toluene, water/CH2Cl2, or water/MTBE.
  • Temperature: 20–80°C depending on substrate.
  • Notes: Vigorous stirring to maximize interfacial area; salt out with NaCl post‑reaction to facilitate phase separation.

• Photoredox benzylic bromination

  • Reagents: Aqueous Br−, photocatalyst (e.g., Ru/Ir complexes or organic dyes), oxygen or mild oxidant.
  • Solvent: Aqueous acetonitrile or alcohol/water mixtures.
  • Light: Blue LED (450–470 nm) typical; intensity tuned to avoid over‑oxidation.
  • Notes: Maintain halide concentration to balance radical chain length; control pH to suppress HOBr disproportionation.

Analytical use conditions

• IC/ISE calibration: Prepare bracketing dilutions gravimetrically with 18 MΩ·cm water; use plasticware/glassware confirmed halide‑clean. Equilibrate to room temperature before use to minimize density‑related bias.

Item-specific caution: Exact concentration, counter‑ion, and pH of this product are not specified; consult the CoA to adapt these general conditions.

Safety & Handling

Item-specific GHS classification, signal word, hazard and precautionary statements, and pictograms are not specified for this item; consult the product SDS and CoA for authoritative safety information.

General safety considerations for aqueous bromide solutions (literature/practice):

• Intrinsic hazards: Aqueous bromide salts are typically of low acute hazard; however, risk profile depends on the counter‑ion (e.g., heavy‑metal bromides can be more hazardous). Avoid ingestion and prolonged skin/eye contact.
• Oxidation risk: Br− can be oxidized by strong oxidizers (e.g., chlorine, hypochlorite, permanganate, nitric acid) to form bromine (Br2) or tribromide (Br3−), which are corrosive and can release irritating vapors. Prevent contact with oxidizing agents and acids that may generate halogen.
• Incompatibilities: Strong oxidizers, strong acids in presence of oxidants, nitrosating agents; avoid halogenating conditions in open systems.
• PPE: Laboratory coat, safety glasses or splash goggles, and appropriate chemical‑resistant gloves (e.g., nitrile). Use in a fume hood if procedures could generate bromine (e.g., intentional oxidation) or aerosols.
• First aid (overview):
  • Skin/eye contact: Rinse with water for ≥15 minutes; remove contaminated clothing; seek medical attention if irritation persists.
  • Inhalation of vapors (from unintended bromine formation): Move to fresh air and seek medical attention.
  • Ingestion: Rinse mouth; do not induce vomiting; seek medical attention.
• Spills: Absorb small spills with inert material; for large volumes, contain and collect for disposal. Avoid oxidizing cleanup agents.
• Disposal: Follow local regulations; aqueous halide solutions can often be sewered only if permitted and uncontaminated—verify with institutional EHS.
• Storage (per Product Data): Store at 2–8°C. Keep tightly closed to minimize microbial growth and evaporation; protect from light and oxidizers. Shipped on wet ice.

Solvent Selection

This product is not a solvent but an aqueous electrolyte solution supplying bromide ion.

Selection considerations (general/literature):

• Polarity and medium: Highly polar, water‑based; miscible with water. Not miscible with nonpolar solvents without a phase‑transfer agent.
• Role in mixtures: Used to adjust halide activity, ionic strength, or redox properties in aqueous systems; can form biphasic systems when combined with immiscible organics for PTC chemistry.
• When to choose
  • Analytical calibration: As a bromide standard for ion chromatography or ion‑selective electrode methods when a ready‑to‑use solution is preferred (verify concentration on CoA).
  • Reaction medium modifier: To modulate reactivity/selectivity in aqueous redox or photochemical systems where Br− acts as a quencher or halogen source upon oxidation.
• Alternatives
  • Solid alkali bromide (e.g., NaBr, KBr) dissolved freshly in high‑purity water to the desired molarity for maximum control and to minimize shipping mass.
  • Non‑aqueous bromide sources (e.g., tetraalkylammonium bromides) for reactions in organic solvents.

Comparison (general)

• Aqueous Br− vs. Cl−: Bromide is a softer nucleophile and more readily oxidized; choose Br− to facilitate bromination pathways or when chloride interference must be avoided.
• Aqueous Br− vs. I−: Bromide is less reducing and less light‑sensitive than iodide; suitable where iodide would over‑reduce or introduce higher blank signals.

Storage & Reconstitution

• Storage conditions (item-specific): Store at 2–8°C (per Product Data). Shipments are on wet ice.
• Container handling: Keep tightly closed to prevent evaporation and contamination. Minimize headspace if long‑term storage is expected to limit CO2 ingress and pH drift where relevant.
• Light/oxidants: Protect from light and segregate from oxidizers and acids that could generate bromine.
• Freeze/thaw: Avoid freezing unless specified on the CoA; freezing can change concentration distribution via ice fractionation and may stress the container.
• Reconstitution: Not applicable—this item is supplied as a solution. If dilution is required, use freshly produced 18 MΩ·cm water and halide‑clean glassware or plasticware. Mix thoroughly and verify concentration by conductivity, density/refractive index correlation, or ion chromatography as appropriate.
• Stability monitoring: Inspect periodically for discoloration (yellow/brown suggests oxidation to Br2/Br3−) or precipitate (could indicate contamination with metals forming insoluble bromides). If observed, do not use for analytical purposes.
• Shelf life: Not specified for this item; refer to CoA/Spec Sheet. For critical work, adopt an in‑house expiry based on risk assessment and storage history.

Structure & Identity

Brief description: This product is an aqueous solution of bromide ion (Br−). Exact concentration, counter‑ion, and any additives are not specified for this item; refer to CoA/Spec Sheet.

• Item-specific identifiers

  • CAS: Not specified for this item; refer to CoA/Spec Sheet.
  • InChIKey: Not specified for this item; refer to CoA/Spec Sheet.
  • Molecular formula: Not specified for this item; refer to CoA/Spec Sheet. (Note: bromide ion is Br− in general literature.)
  • Molecular weight: Not specified for this item; refer to CoA/Spec Sheet. (Literature atomic weight of Br ≈ 79.904 g/mol for Br−.)
  • SMILES: [Br-] (literature, for the bromide anion)

• Structural features (general/literature)

  • Monatomic halide anion derived from bromine; closed‑shell, spherical anion with filled 4p subshell; no stereochemistry.
  • In water, Br− exists as a solvated ion within a hydrogen‑bonded network; can form weak ion pairs depending on counter‑ion and ionic strength.

• 2D structure in words (general)

  • A single bromide anion represented as Br with a negative charge; in aqueous solution, surrounded by a primary solvation shell of water molecules oriented by electrostatics.

• Notes on identity in solution

  • The functional chemical entity is Br−; performance and compatibility will depend on the unspecified counter‑ion (e.g., Na+, K+, etc.) and concentration. Confirm these on the product’s CoA before use in quantitative or method‑validated workflows.

Synthetic Utility

General/literature perspectives on bromide ion in synthesis:

• Nucleophilicity and softness: Br− is a moderate, polarizable nucleophile; it participates in SN1 and SN2 substitutions to form alkyl bromides. In aqueous media, nucleophilicity is reduced by solvation; phase‑transfer catalysts or mixed solvents can enhance reactivity.
• Halide exchange: Finkelstein‑type exchanges (R–Cl to R–Br) are favored in polar aprotic solvents; aqueous Br− may still effect exchange for activated substrates or under PTC.
• Redox mediator and bromination source: Oxidation of Br− generates Br2 or Br3− in situ for electrophilic bromination of electron‑rich aromatics, enones, and allylic positions. Controlled generation minimizes handling of neat bromine.
• Catalysis: Bromide can coordinate to or inhibit transition‑metal catalysts (e.g., Pd, Cu, Au), altering rates and selectivity. Intentional bromide addition can stabilize certain catalytic resting states or, conversely, be removed to accelerate turnover.
• Photoredox systems: Under visible light with suitable photocatalysts and oxidants, Br− can form Br• radicals enabling C–H functionalization; aqueous conditions can improve selectivity for benzylic/allylic sites.

Practical guidance

• Choose counter‑ion to match solvent system (e.g., tetraalkylammonium bromides for organic phases; Na+/K+ for aqueous).
• Control pH and oxidant dosing to avoid over‑bromination or bromate formation.
• Remove excess halide post‑reaction via aqueous washes or silver salt treatments, considering waste management for AgBr solids.

Target Specificity

Not applicable to this product. This is an inorganic aqueous reagent (bromide ion in water), not an antibody or affinity reagent. There are no antigens, epitopes, species reactivity, clones, or isotypes associated with this item.