Featured products

Acids and bases

• The Arrhenius definition which is based on the idea that acids are substances that ionize (dissociate) in an aqueous solution to release hydrogen ions or protons (H⁺) while bases release hydroxide ions (OH⁻) in solution. This led to Arrhenius receiving the Nobel Prize in Chemistry in 1903.
• The Brønsted-Lowry definition defines acids as substances that donate protons (H⁺) whereas bases are substances that accept protons. The advantage of this definition is that it is not limited to aqueous solutions. Brønsted-Lowry acids and bases always occur in pairs called conjugate acid-base pairs. The pairs are related through the transfer of a proton.
• The Lewis theory of acids and bases states that acids are electron-pair acceptors (to form a covalent bond) while bases are electron-pair donors (to form a covalent bond). This definition is the most inclusive and encompasses species not included in the Brønsted-Lowry definition.

Brief summary - the three concepts of acid and bases:

Arrhenius – the first modern approach
Acid: produces H⁺ (protons) in aqueous solution
Base: produces OH^- (hydroxide ions) in aqueous solution

Brønsted-Lowry – the most generally accepted
Acid: proton donor
Base: proton acceptor

Lewis – the most inclusive
Acid: electron-pair acceptor (to form a covalent bond)
Base: electron-pair donor (to form a covalent bond)

Acids and bases combine or neutralize each other by acid-base reactions to form salts (see also more information on our salts & minerals page).

pH
The hydrogen ion concentration, [H⁺], is a measure of both Arrhenius and Brønsted-Lowry defined acids, a measure of the acidity or basicity (alkalinity) of a substance or solution. This is generally expressed as pH. The pH of a solution equals the negative of the logarithm to the base 10 of its hydrogen ion concentration:

pH = -log [H⁺] = log 1/[H⁺]

The pH offers a convenient mechanism of expressing a wide range of [H⁺] in small positive numbers. The letter, p, is used to denote the negative logarithm to the base of 10.

Likewise, the hydroxide ion concentration may be expressed as pOH:

pOH = -log [OH^-]

The pH scale from 0 to 14 covers usually all the hydrogen ion concentrations found in diluted aqueous solutions and biological systems. Pure water has a pH of 7 at 25 °C (as pH value depends on temperature), which is considered to be neutral, because the concentration of hydrogen ions [H⁺] equals the concentration of hydroxide ions [OH⁻].

When pH < 7, the solution is acidic and when pH > 7, the solution is basic or alkaline. Because of the logarithmic function a change of one pH unit represents a tenfold difference in hydrogen ion concentration.

pH is the parameter most often measured in chemistry, particularly in analytical chemistry. It is also important in pool maintenance and water purification, agriculture, medicine, engineering, oceanography, biology, and other sciences.

Measurements of pH can be easily performed using a pH-meter, a color-changing indicator, or pH indicator papers.

Find also more information on:

Buffer

Dyes, Stains & Indicators


Acid/Base Strengths - Dissociation Constants – K_a, K_b and K_w

Strong acids and bases

Strong acids and bases are those that completely dissociate into their component ions in aqueous solution.

In water, one mole of a strong monoprotic acid HA dissolves yielding one mole of H⁺ (as hydronium ion H₃O⁺) and one mole of the conjugate base, A⁻. Essentially, none of the non-ionized acid HA remains, each of these essentially ionizes 100%.

Strong acid: HA + H₂O → A^-_(aq) + H₃O⁺_(aq)
Strong base: BOH + H₂O → B⁺_(aq) + OH^-_(aq)

For simplicity, H₃O⁺ can be written as H⁺, although this free H⁺ does not exist in aqueous solutions, since in all acid ionization reactions a proton is transferred to H₂O to form hydronium ions, H₃O⁺.

Strong acid: HA_(aq) → A^-_(aq) + H⁺_(aq)
Strong base: BOH_(aq) → B⁺_(aq) + OH^-_(aq)

Examples of strong acids and bases:

Weak acids and bases

Weak acids and bases are those that only partially dissociate in aqueous solution. At equilibrium, both the acid and the conjugate base are present in solution. The dissociation of an acid or a base is expressed by the following reaction:

Weak acid: HA_(aq) ⇋ A^-_(aq) + H⁺_(aq)
Weak base: BOH_(aq) ⇋ B⁺_(aq) + OH^-_(aq)

The acid dissociation constant, K_a, is a measure of the degree of dissociation of the acid.

K_a = [HA⁺] [A^- ] / [HA] or
pK_a = -log [HA⁺] [A^- ] / [HA] = log [HA] / [HA⁺] [A^- ]

where quantities in square brackets represent the concentrations of the species at equilibrium.

Stronger acids have a larger acid dissociation constant (K_a) and a smaller logarithmic constant (pK_a = −log K_a) than weaker acids. The stronger an acid is, the more easily it loses a proton, H⁺.
Acids with a K_a value less than one, or consequently pK_a greater than 0, are considered weak.
K_a or pK_a can therefore be used to distinguish between strong acids and weak acids.

Strong acids: K_a > 1 or pK_a < 0
Weak acids: K_a < 1 or pK_a > 0

Similarly, a weak monovalent base, BOH, dissociates to give B⁺ and OH^-.

The base dissociation constant, K_b, is a measure of the degree that the base dissociates.

K_b = [B⁺] [OH^-] / [BOH]

Examples of weak acids and bases:

The dissociation of water

K_w - The water ionization constant
Water partially dissociates into ions according to the equation:

H₂O ⇋ H⁺ + OH^-

The equilibrium constant K for this reaction can be written as follows:

K = [H⁺] [OH^-] / [H₂O]

When pure liquid water is in equilibrium with hydrogen and hydroxide ions at 25 °C, the concentrations of the hydrogen ion and the hydroxide ion are equal: [H⁺] = [OH⁻] = 1.0 × 10⁻⁷ mol/L.
Thus, the number of dissociated water molecules is very small indeed, approximately 2 ppb. One can calculate [H₂O] at 25 °C from the density of water at this temperature (0.997 g/mL):

[H₂O] = mol/L = 1 mol/18.02 g x 0.997 g/mL X 1000 mL/L = 55.3 mol/L

With so few water molecules dissociated, the equilibrium of the autoionization reaction lies far to the left. Consequently, [H₂O] is essentially unchanged by the autoionization reaction and can be treated as a constant. Incorporating this constant into the equilibrium expression allows us to rearrange the equation to define a new equilibrium constant.

K [H₂O] = [H⁺] [OH^-]

As K is a constant and [H₂O] is a constant we can replace both with a new constant K_w called the ion-product constant of liquid water (also called the ionic product of water, water autoprotolysis constant, water (auto)ionization constant or water-dissociation equilibrium constant).

K_w = [H⁺] [OH^-]

As in pure water, at 25 °C, the [H⁺] and [OH^-] ion concentrations are 1.0 x 10^-7 mol/L. The value of K_w at 25 °C is therefore 1.0 x 10^-14.

K_w = (1.0 x 10^-7) (1.0 x 10^-7) = 1.0 x 10^-14 (at 25 °C)

Although K_w is defined in terms of the dissociation of water, this equilibrium constant expression is equally valid for solutions of acids and bases dissolved in water. Regardless of the source of the H⁺ and OH^- ions in water, the product of the concentrations of these ions at equilibrium at 25 °C is always 1.0 x 10^-14.

Consequently if:

[H⁺] [OH^-] = 10^-14

And taking the negative log on both sides of the equation gives:

-log [H⁺] – log [OH^-] = 14

As pH = −log [H⁺] and pOH = −log [OH⁻]

then:

pH + pOH = 14

The sum of pH and pOH is always 14 for any aqueous solution at 25 °C.

Conjugate acid-base pairs
According to Brønsted-Lowry definition, any acid and base exists as conjugate acid-base pair. Every time an acid acts as a H⁺ donor, it forms a conjugate base. When a generic acid HA donates a H⁺ to water, one product of the reaction is the A^- ion, which is a hydrogen-ion acceptor, or Brønsted base.

Relationship between K_a and K_b for conjugate acid-base pair:

HA ⇋ A^- + H⁺
acid base

K_a = [H⁺] [A^- ] / [HA]

Since A⁻ is a base, we can also write the reversible reaction for A⁻ acting as a base by accepting a proton from water:
A^- + H₂O ⇋ HA + OH^-

Then:

K_b = [B⁺] [OH^-] / [BOH]

If we multiply K_a for HA with the K_b for its conjugate base A^-, that gives:

K_a x K_b = [H⁺] [A^- ] / [HA] x [HA] [OH^-]/[A^-] = [H⁺] [OH^-] = K_w

where Kw is the water dissociation constant. This relationship is very useful for relating K_a and K_b for a conjugate acid-base pair. We can also use the value of K_w at 25 °C to derive other handy equations:

K_a x K_b = K_w
K_w= 10^-14 at 25 °C
K_a x K_b = 10^-14

If we take the negative logarithm of both sides of the equation, we get:

pK_a + pK_b = 14

We can use these equations to determine K_b (or pK_b) of a weak base given K_a of the conjugate acid. We can also calculate the K_a (or pK_a) of a weak acid given K_b of the conjugate base.

Two key factors that contribute to the ease of deprotonation are the polarity of the H-A bond and the size of atom A, which determines the strength of the H-A bond. Acid strengths also depend on the stability of the conjugate base.

A conjugate acid is defined as the acid formed when a base gains a proton. Similarly, a conjugate base is formed when an acid loses a proton. For example, with HCO₃^-/CO₃^2- conjugate acid/base pair, the CO₃^2- is the conjugate base and HCO₃^- is the conjugate acid.
By adding the reactions of the conjugate acid and conjugate base with water, the net reaction is simply the dissociation of water. Thus, if you know the dissociation constant for one, the other can be determined:

K_a x K_b = K_w = 10^-14

Thus, K_a and K_b are inversely related. In other words, if K_a is large (the acid is strong), then K_b (base is weak) will be small and vice versa. From this relationship, one can see that when a conjugate acid/base pair form from a weak acid, the conjugate base is stronger than the acid.

(1) First dissociation

Polyprotic acids
Acids can donate one, two or more protons (H⁺). Typical examples are:

A monoprotic acid is characterized by a single acidity constant K₁ (= K_a), a diprotic acid by two acidity constants (K₁, K₂), and a triprotic acid by three acidity constants (K₁, K₂, K₃):

1^st dissociation step: H₃A = H⁺ + H₂A^- (K₁)
2^nd dissociation step: H₂A^- = H⁺ + HA^2- (K₂)
3^rd dissociation step: HA^2- = H⁺ + A^3- (K₃)

This can be extended to any N-protic acid with N dissociation steps.

Protons are released sequentially one after the other, with the first proton being the fastest and most easily lost, then the second, and then the third (which is most strongly bound). This yields the following ranking of acidity constants of a polyprotic acid:

K₁ > K₂ > K₃ or pK₁ < pK₂ < pK₃

For example, phosphoric acid has pK₁ = 2.147, pK₂ = 7.207, and pK₃ = 12.346.

Amphoteric substances
An amphoteric compound is a molecule or ion that can react both as an acid and as a base. One type of amphoteric species are amphiprotic molecules, which can either donate or accept a proton (H⁺). This is what "amphoteric" means in Brønsted–Lowry acid–base theory. Examples include amino acids and proteins, which have amine and carboxylic acid groups, and self-ionizable compounds such as water. Metal oxides which react with both acids as well as bases to produce salts and water are known as amphoteric oxides. Many metals form amphoteric oxides or hydroxides. Ampholytes are amphoteric molecules that contain both acidic and basic groups and will exist mostly as zwitterions in a certain range of pH. A zwitterion is a molecule with functional groups, of which at least one has a positive and one has a negative electrical charge. The net charge of the entire molecule is zero.

Calculating pH
To calculate the pH of an aqueous solution you need to know the concentration of the hydronium
ion in moles per liter (molarity). The pH is then calculated using the expression:

pH = - log [H⁺].

Strong Acid:
From the definition of pH, and assuming that, because the acid is strong, the analytical concentration of the acid (C_a) is equal to the concentration of H⁺.

pH = -log C_a

Strong Base:
When the base is strong, the analytical concentration of the base (C_b) is equal to the concentration of OH^–. Since pH= 14 – pOH, becomes,

pH = 14 + log C_b

Weak acid:
Only some small fraction of molecules in solution dissociates to anion and proton, being x its concentration at equilibrium:

As the acid is weak, the K_a is small, so the equilibrium lies well to the left, so we assume that
C_a – x ≅ C_a, then the equilibrium expression becomes:

K_a = x²/C_a = [H⁺]²/C_a

Then,

[H⁺] = SQRT (K_aC_a) = (K_a)^1/2 (C_a)^1/2

taking the negative logarithms,

pH = ½ pK_a – ½ log C_a

Weak base:
Only some small fraction of molecules in solution dissociates to anion and proton, being x its concentration at equilibrium:

As the base is weak, the K_b is small, so the equilibrium lies well to the left, so we assume that
C_b – x ≅ C_b, then the equilibrium expression becomes:

K_b = X²/C_b = [OH^-]²/C_b

Then:

[OH^-] = SQRT (K_bC_b) = (K_b)^1/2 (C_b)^1/2

taking the negative logarithms,

pOH = ½ pK_b – ½ log C_b

pH = 14 - pOH

Buffers
Weak acid plus the salt of the weak acid (i.e a weak acid in the presence of its conjugate base).

In this case the weak acid, HA, with concentration C_a, is in solution with a salt of a common cation.
For example, if the salt NaA has concentration C_b, the [A^–] in the solution, due to the salt alone, is
also C_b, since NaA is 100% dissociated (all salts ionize completely in aqueous solutions).

Due to the presence of the common ion (from the salt), A^–, the equilibrium will be shifted even further left than suggested by the acid small K_a value. Consequently, it is safe to assume that,
C_a − x ≈ C_a and C_b + x ≅ C_b. The equilibrium expression becomes,

K_a = x C_b/C_a= [H⁺] C_b/C_a

[H⁺] = K_a C_a/C_b

Taking − log of both sides yields,

pH = pK_a + log C_b/C_a

This is called the Henderson-Hasselbalch equation and is useful for estimating the pH
of a buffer solution.

Weak base plus the salt of the weak base (i.e a weak base in the presence of its conjugate acid)
In this case the weak base, BOH, with concentration C_b, is in solution with a salt of a common anion, with concentration C_a.

Due to the presence of the common ion (from the salt), B⁺, the equilibrium will be shifted even further left than suggested by the base small K_b value. Consequently, it is safe to assume that,
C_b − x ≈ C_b and C_a + x ≅ C_a. The equilibrium expression becomes,

K_b = x C_a/C_b = [OH^-] C_a/C_b

[OH^-] = K_b C_b/C_a

Taking − log of both sides yields,
pOH = pK_b – log (C_b/C_a)

since pK_b = 14 - pK_a and pOH = 14 - pH

then:

pH = pK_a + log C_b/C_a

And we have again the Henderson-Hasselbalch equation. In this case, the pK_a is for the conjugate acid of the weak base and C_b and C_a are the concentrations of the weak base and its conjugate acid respectively.

Amphiprotic substance (i.e. HA^-, present in the solution of acidic salts)
The challenge is, HA^- hydrolyses and dissociates at the same time and it is not obvious which of these processes will be be responsible for the final pH, moreover, it is very likely that pH can be attributed to some equilibrium between both reactions.

K_a1 = [H⁺] [HA^-] / [H₂A]
K_a2 = [H⁺] [A^2-] / [HA^-]
C_HA^- = [H₂A] + [HA^-] + [A^2-]

C_HA^- is the concentration of the source of the amphiprotic substance

H⁺ ions are produced in the dissociation reaction (together with A^2-) and consumed in the hydrolysis (yielding H₂A), so their concentration is:

[H⁺] = [A^2-] - [H₂A]

we can rewrite it in the form:

[H⁺]=K_a2 [HA^-] / [H⁺] – [H⁺] [HA^-] / K_a1

or, after rearranging

[H⁺]² = K_a1 K_a2 [HA^-] / ([HA^-] + K_a1)

If neither dissociation nor hydrolysis goes too far, and [HA^-] = C_HA^-. If so

[H⁺] = SQRT (c_HA^- K_a1 K_a2 / (c_HA^- + K_a1)


If the C_HA^- is sufficiently larger than K_a1 we can neglect K_a1 and whole equation takes form

[H⁺] ≅ SQRT(K_a1 K_a2) = K_a1^½ K_a2^½

or

pH = ½ (pK_a1 + pK_a2)

Titration
Titration is a procedure used to determine the concentration of an acid or base. This is accomplished by reacting a known volume of a solution of an unknown concentration with a known volume of a solution of known concentration. When the number of acid molecules equals the number of base molecules added (or vice versa), the equivalence point is reached.
The equivalence point in a titration is estimated in two common ways: either by using a graphical method, plotting the pH of the solution as a function of added titrant by using a pH meter or by watching for a color change of an added indicator. Indicators are weak organic acids or bases that have different colors in their undissociated and dissociated states.
For further information about our titration products please visit our Titration page.

Our portfolio of Acids and Bases consists of:

• Inorganic acids such as hydrochloric acid, sulfuric acid, nitric acid, hydrofluoric acid, phosphoric acid or boric acid, etc.,
• Organic acids are acetic acid, formic acid, citric acid, lactic acid, oxalic acid, ascorbic acid, EDTA, etc.,
• Fatty acids such as octanoic acid (caprylic acid), oleic acid,
• Amino acids (see also Amino acids page), which are especially important in the field of biochemistry/Life Sciences such as aspartic acid, glutamic acid or lysine, among others. Amino acids are the building blocks of proteins and play a key role in most biological processes. In fact, they can have both acidic and basic (amphoteric) behavior, depending on the pH of the solution, because they have an amino group (basic) and a carboxylic group (acidic) in the same molecule,
• Inorganic bases, the most common ones are sodium hydroxide (caustic soda), potassium hydroxide (caustic potash), ammonia in solution, bicarbonates, calcium or magnesium hydroxides, etc,
• Organic bases, among them are pyridine, tetrabutylammonium hydroxyde, triethanolamine, triethylamine, etc.

It is of vital importance to choose the right product with the appropriate quality grade adapted to your requirements to achieve and obtain high-quality, reliable and accurate results. We offer a broad range of quality grades with strictly guaranteed specifications, enabling the selection of the right product for your specific application:

• Reagents for analysis (p.a.) according to ISO (International Organization for Standardization), ACS (American Chemical Society) and pharmacopoeia specifications for reagents (Reag. Ph. Eur., Reag. USP).
• Ultrapure acids for trace metal analysis (ppb, ppt) by AAS, GF-AAS, ICP-OES, ICP-MS.
• For HPLC or for UV applications.
• Pharma grade: raw materials for the pharmaceutical industry in manufacturing processes (e.g. for pH adjustments), and as excipients in the final formulation, complying with the pharmacopoeia specifications (monographs), such as US Pharmacopea/National Formulary (USP-NF), European Pharmacopoeia (EP or Ph. Eur.), British Pharmacopoeia (BP), etc., and GMP-IPEC grade, including regulatory documents.
• Reagents for Life Sciences: BioChemica, for molecular biology or for cell culture.
• Pure products for general use.
• Volumetric solutions (standards), concentrated and ready to use, for quantitative analysis.
• Solutions for volumetric analysis / titration and for the determination of nitrogen (proteins) by means of the Kjeldahl method.
• For clinical diagnosis, such as picric acid.
• Products for synthesis.
• Technical grade or industrial grade.
• Food grade according to European regulations (EC) or Food Chemicals Codex (FCC).
• VINIKIT, for wine analysis.

Acids and bases at ITW Reagents
At ITW Reagents we supply high quality acids and bases under the PanReac AppliChem brand for all relevant industries, such as pharmaceutical and food industry, testing in general analysis laboratories, quality control, research, life sciences, environmental analysis, and others. All products are manufactured using the Integrated Quality Management System according to ISO 9001, ISO 14001 and ISO 45001 standards. With our more than 80 years of experience as a manufacturer, you can benefit from our exceptional know-how in acids and bases under strict quality control, commercial and technical support strongly committed to our customers, constant stock level with a stable supply chain and a global distribution network.

Applications of acids and bases
In chemical quality control labs, research and development or in innovation departments of any industry or institution, also when using raw materials in industrial processes for production of pharmaceuticals or in any organic synthesis or purification processes.

Analytical reagents in standard procedures, pH adjustments, qualitative and quantitative analysis, instrumental analysis, wet chemistry analysis and testing, educational chemistry experiments, digestion of samples, catalysts in chemical reactions, sample preparation in trace metal analysis, wastewater testing, etc.

In water treatment, manufacturing of paper, fertilizers, soaps, detergents, cleaning agents, cleaning-in-place (CIP), synthesis of nylon, explosives, production of organic compounds (such as vinyl chloride and dichloroethane for PVC), manufacturing of synthetic resins, dyestuffs, pharmaceuticals, petroleum catalysts, insecticides and antifreeze, as well as in various processes such as oil well acidizing, aluminum reduction, refining metals, picking of steel, electroplating, battery production, etc.

Sectors

• Analytical Laboratories, Quality Control, Chemical and Biochemical labs
• Research, Development, and Innovation (R&D)
• Biopharmaceutical and Pharmaceutical development and manufacturing
• Life Sciences
• Cosmetics and Healthcare
• Food and Beverages
• Inorganic and Organic synthesis
• Educational or academic institutions
• Paper industry
• Soap and detergent industry
• Metallurgy
• Agriculture
• Pool maintenance

Pack sizes and packaging materials
From mg to tons for solids and from mL to 1000 L for liquids, in a large variety of packaging sizes and materials, we select the most convenient containers assuring the preservation of the product quality, the safety on transport and use, and the protection of the environment.

UN Certified packaging
The regulations for the transport of hazardous materials require the use of approved packaging. It defines the characteristics that containers and packaging must meet according to the product, its hazardousness and the maximum quantity it can contain. This information appears on UN approved containers.
All packaging used by PanReac AppliChem branded products scrupulously comply with the regulations in force (ADR, RID IMDG, ICAO-IATA).

Packaging materials

• Standard containers: Glass bottles, HDPE bottles, PC bottles, HDPE canisters, HDPE drums, PP pails/buckets.
• Special bottles/containers: For liquid corrosive products, such as acids and bases, we use special glass bottles with pouring ring. The pouring ring prevents from any drop sliding down the outside of the bottle that could damage the label, the surface area or could harm the user.
• Square plastic (HDPE) bottles for volumetric solutions, with a great stability, special for automatic titrators.
• We use specially selected teflon bottles for trace metal analysis ultra-pure acids. The material is controlled prior to the bottle manufacture. Every bottle is leached with hot acid during two weeks in order to eliminate any contamination material due to metallic traces.
• Sol-Pack (bag in box, cubitainer) consists of a 10 L-collapsible polyethylene bag and an outer cardboard box, forming a light, practical and easily disposable pack. It incorporates a tap, which allows convenient dosing down to the last drop. Main advantages: saving of up to 60% compared with 1 litre bottles. Air does not enter the collapsible bag, ensuring product preservation. Reduced risk of contamination or carbonatation. A more environmentally friendly alternative to plastic bottles, as less packaging waste is generated.
• Larger quantities: Sodium hydroxide solutions and hydrochloric acid are available in IBC containers (up to 1000 L). Obtain the maximum capacity with a minimum space. IBCs are used to transport and store large amounts of liquids, for chemical, food, cosmetics, and pharmaceutical industries. UN certified.
• Plastic (PP) pails/buckets for solids from 5 kg to 25 kg, UN certified, suitable for chemical, food, cosmetics and pharmaceutical industries.

We offer our customers several accessories and tools, such as taps, wrenches and adapters, to facilitate the opening and dispensing of containers.

See more info at Packaging

Safety
Both acids and bases are chemicals that present health hazards if improperly handled or stored. It is extremely important to handle and store chemicals safely to avoid spills in the workplace, fires, explosions, release of toxic gas and personal injuries. Safety Data Sheets (SDS) will provide information on how to protect yourself from potential adverse health effects, how to correctly handle the chemical, avoid possible dangers, properly dispose of the chemical, and more. It is critical to the safety of yourself and others to handle chemicals with caution and follow the proper protocols. Reading the entire SDS sheet can help avoid accidents and potential injuries from improper chemical usage. SDS or Safety Data Sheets, formally known as MSDS (Material Safety Data Sheets) are the internationally recognized format for communicating the use, handling, and storage of hazardous products. All Safety Data Sheet (SDS) are available on our webpage, please read carefully the SDS before using the product.

Purity
To minimize the risk of user exposure to acids and bases and save preparation time, we offer a wide range of prepared solutions in different concentrations with the highest quality raw materials and strict quality control to ensure exact concentration and maximum purity.

Examples of acids and bases in different concentrations

Hydrochloric acid, HCl, CAS number 7647-01-0:

Sodium hydroxide, NaOH, CAS number 1310-73-2:

Sulfuric acid, H₂SO₄, CAS number 7664-93-9:

Nitric acid, HNO₃, CAS number 7697-37-2:

Acetic acid, CH₃COOH, CAS number 64-19-7:

Ammonia, NH₃/NH₄OH, CAS number 1336-21-6:

Potassium hydroxide, KOH, CAS number 1310-58-3:

Phosphoric acid, H₃PO4, CAS number 1310-58-3:

Where can I buy acids and bases?
You can buy acids and bases via our global distribution network or in our web shop if you are a registered distributor of ITW Reagents. Please follow this link to find a distributor in your country.

Distributors
For orders within a regulative context (e.g. pharma, food, cosmetic applications) please contact our
dedicated process team directly by using our contact template.

Request a quote for raw materials