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A primary standard in metrology is a standard that is sufficiently accurate such that it is not calibrated by or subordinate to other standards. Primary standards are defined via other quantities like length, mass and time. Primary standards are used to calibrate other standards referred to as working standards.^[1]^[2] See Hierarchy of Standards.

In chemistry

[edit]

Standards are used in analytical chemistry.^[3] In this field, primary standard is typically a reagent that can be weighed easily, and which is so pure that its weight is the number of moles of substance contained. Features of a primary standard include:

High purity
Stability (low reactivity)
Low hygroscopicity (to minimize weight changes due to humidity)
High equivalent weight (to minimize weighing errors)^[4]
Long lasting molar solution i.e. concentration remains unchanged for long periods of time

Some examples of primary standards for titration of solutions, based on their high purity, are provided:^[5]^[6]

Arsenic trioxide for making sodium arsenite solution for standardisation of sodium periodate solution (until Ph. Eur. 3, Appendix 2001 also for iodine and cerium(IV) sulfate solutions, since Ph. Eur. 4, 2002 standardised by sodium thiosulfate)
Benzoic acid
Potassium bromate (KBrO₃) (for standardisation of sodium thiosulfate solutions) and potassium iodate
Potassium hydrogen phthalate (usually called KHP) for standardisation of aqueous base
Sodium carbonate for standardisation of aqueous acids: hydrochloric, sulfuric acid and nitric acid solutions (but not acetic acid)
Sodium chloride for standardisation of silver nitrate solutions
Sulfanilic acid for standardisation of sodium nitrite solutions
potassium ferrocyanide, a reductant
potassium dichromate, an oxidant

Such standards are often used to make standard solutions. These primary standards are used in titration and are essential for determining unknown concentrations^[1] or preparing working standards.

References

[edit]

^ ^a ^b Skoog, Douglas A., Donald M. West and F. James Holler. "Fundamentals of Analytical Chemistry 8th ed." Harcourt Brace College Publishers. 1995 ISBN 0-03-035523-0
^ Holt Science and Technology: Physical Science. Ed. Rinehart and Winston, Inc. Holt. Holt McDougal (July 2000). ISBN 978-0-03-051957-4.
^ "Standard Solution". International Union of Pure and Applied Chemistry. Retrieved January 24, 2026.
^ "Primary standards – Criteria, Properties and Examples – Pharmawiki.in". 13 January 2014.
^ Khopkar, S. M. (2012). Basic Concepts of Analytical Chemistry (3rd ed.). New Academic Science. p. 32. ISBN 9788122411591.
^ European Pharmacopoeia, chapter 4.2.1

External links

[edit]

Analytical Standards. Department of Chemistry, University of Adelaide, Australia.

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A primary standard is a term with distinct meanings in metrology and analytical chemistry. In metrology, a primary standard (or primary measurement standard) is a measurement standard established using a primary reference measurement procedure, or an artifact, that constitutes a primary reference and has the highest metrological quality in a given measurement context; it is directly traceable to the International System of Units (SI).^[1] In analytical chemistry, a primary standard is a highly pure, stable reagent that can be weighed accurately to prepare a solution of known concentration, serving as a reference for standardizing other reagents in quantitative analyses such as titrations.^[2] These standards are essential for ensuring the precision and accuracy of measurements by providing a reliable benchmark with minimal uncertainty in their composition.^[3] Key properties of primary standards include high purity to allow for exact quantification without impurities affecting results.^[2] They must exhibit long-term stability under storage conditions, resisting decomposition or chemical change, and are generally non-hygroscopic to prevent moisture absorption that could alter their mass during weighing.^[3] Additionally, primary standards often have known stoichiometry, high molecular weight for easier accurate dispensing, and the ability to react completely and rapidly with the analyte in the analytical procedure.^[2] Common examples of primary standards include potassium hydrogen phthalate (KHP), used for standardizing bases like sodium hydroxide due to its stability and precise molar mass of 204.23 g/mol.^[3] Other frequently employed substances are oxalic acid dihydrate for acid-base titrations and potassium dichromate (K₂Cr₂O₇) for redox analyses, where 0.1250 g yields a 1.700 × 10⁻³ M solution in 250 mL.^[2] These compounds are selected based on their purity and reactivity, ensuring they function effectively without hydration issues that complicate anhydrous forms.^[3] Primary standards play a critical role in the standardization process, where they are used to determine the exact concentration of secondary standards or unknown solutions, thereby calibrating analytical methods and minimizing systematic errors.^[2] This foundational step is vital in fields like pharmaceutical testing, environmental monitoring, and quality control, where precise concentration determinations underpin reliable results and compliance with regulatory standards.^[3]

In Metrology

Definition and Purpose

In metrology, a primary standard is defined as a measurement standard established using a primary reference measurement procedure or created as an artifact, characterized by a primary method, which ensures it is not calibrated by or subordinate to any other standards. This positions it at the highest level in the metrological hierarchy, providing the utmost accuracy and stability for realizing units of measurement.^[4] The primary purpose of such standards is to define fundamental physical quantities, including length, mass, and time, thereby serving as the foundational reference for calibrating secondary and working standards. By establishing these uncalibrated benchmarks, primary standards enable the dissemination of measurement units with consistent precision worldwide, supporting scientific research, trade, and technology development.^[5] Primary standards underpin metrological traceability, linking everyday measurements to the International System of Units (SI) through an unbroken chain of calibrations overseen by the International Bureau of Weights and Measures (BIPM), established by the Metre Convention in 1875. Their historical origins trace to ancient civilizations' efforts to create unchanging references, such as the Egyptian cubit—a forearm-length unit standardized around 3000 BC for construction and trade—which evolved into modern SI realizations, exemplified by the meter's initial 1799 definition as a platinum bar's length, later redefined in 1983 using the speed of light in vacuum.^[6]^[7]^[8]

Characteristics and Examples

Primary standards in metrology exhibit the highest metrological qualities, including accuracy with associated uncertainties typically below 1 part in 10^9, long-term stability, and reproducibility under defined conditions. They are established using primary methods of measurement—procedures that allow a quantity to be measured without reference to another standard of the same kind—or created as artifacts chosen by international convention, often realized directly from fundamental natural constants or physical laws, thereby requiring no further calibration against subordinate references.^[9] This direct linkage ensures intrinsic stability, particularly for standards based on quantum phenomena, which maintain their properties over extended periods without degradation.^[9] Within the metrological hierarchy, primary standards occupy the apex of the measurement pyramid, providing the foundational reference for calibrating secondary standards (which are themselves calibrated against primaries) and, indirectly, working standards used in everyday applications. Traceability to a primary standard is achieved through an unbroken chain of calibrations, where the total combined standard uncertainty

u_c

propagates downward as

u_c = \sqrt{u_{\text{primary}}^2 + u_{\text{calibration}}^2 + \cdots}

uc=uprimary2+ucalibration2+⋯

, with the primary standard's uncertainty $u_{\text{primary}}$ being the smallest contributor to ensure overall reliability.^[10]^[11] Concrete examples illustrate these characteristics across key domains. For the unit of time, the second is realized as the primary standard through the unperturbed ground-state hyperfine transition frequency of the caesium-133 atom, fixed at exactly 9,192,631,770 Hz, enabling atomic clocks with relative uncertainties as low as 2 × 10^{-15}. For length, the metre serves as the primary standard, defined by assigning the fixed numerical value 299,792,458 to the speed of light in vacuum, allowing realization via interferometry with uncertainties below 10^{-11}. In mass metrology, the kilogram was historically embodied by the International Prototype of the Kilogram, a platinum-iridium artifact maintained at the International Bureau of Weights and Measures until 2019, with a stability of about 10^{-8} over decades but requiring periodic verification. The 2019 revision of the International System of Units (SI) represented a pivotal advancement, eliminating all artifact-based primary standards in favor of definitions tied exclusively to invariant constants, such as the Planck constant $h = 6.626\,070\,15 \times 10^{-34}$ J s for the kilogram. This shift enhances universality, reproducibility, and long-term invariance by grounding realizations in fundamental physics rather than physical objects susceptible to environmental influences.^[12]

In Analytical Chemistry

Definition and Requirements

In analytical chemistry, a primary standard is defined as a highly pure and stable reagent that can be used directly to prepare standard solutions of accurately known concentration, serving as a reference for standardizing other solutions or for the quantitative determination of unknown concentrations in titration procedures.^[13] These standards ensure traceability in measurements by providing a reliable basis for calibration, where the concentration is calculated from the weighed mass of the pure substance dissolved in a known volume of solvent.^[14] The key requirements for a compound to qualify as a primary standard include exceptional purity, typically exceeding 99.9%, to minimize impurities that could affect concentration accuracy.^[15] It must also exhibit high chemical stability, remaining unreactive toward air, light, carbon dioxide, or water under normal storage conditions to prevent decomposition or alteration.^[16] Additionally, the substance should be non-hygroscopic, avoiding absorption of atmospheric moisture that could lead to errors in mass determination during weighing.^[16] A high molecular weight, generally above 100 g/mol, is preferred to reduce the relative error in weighing small quantities, as the percentage error decreases with larger masses.^[15] The compound must dissolve readily and completely in the intended solvent without side reactions, and while non-toxicity and low cost are desirable for practical use, they are not strictly mandatory.^[15] The use of primary standards in analytical chemistry developed in the 19th century alongside the development of volumetric analysis, pioneered by Joseph Louis Gay-Lussac in the 1820s through his work on acid-base titrations and standardization methods. Further advancements were made by Karl Friedrich Mohr in the 1850s, who introduced oxalic acid as one of the early primary standards for alkalimetric determinations.^[17] In contrast to primary standards in general metrology, which often rely on physical artifacts or fundamental constants, chemical primary standards in analytical chemistry establish concentration references that are traceable to the SI base units of mass and volume via calibrated balances and volumetric equipment, resulting in measurement uncertainties typically ranging from 0.01% to 0.1%.^[14] This traceability integrates into the broader metrological hierarchy, ensuring comparability of chemical measurements across laboratories.^[11]

Examples and Applications

In analytical chemistry, primary standards are selected based on their high purity and stability, serving as reference materials for standardizing titrants in various types of volumetric analyses. Common examples are categorized by titration type, with specific compounds chosen for their well-defined stoichiometry and ease of handling. For acid-base titrations, potassium hydrogen phthalate (KHP, C₈H₅KO₄) is widely used to standardize bases such as sodium hydroxide (NaOH).^[18] Anhydrous sodium carbonate (Na₂CO₃) serves as a primary standard for standardizing acids like hydrochloric acid (HCl). In redox titrations, potassium dichromate (K₂Cr₂O₇) is employed in acidic medium to standardize reducing agents, leveraging its stability and precise equivalent weight.^[2] Arsenic trioxide (As₂O₃) acts as a primary standard for oxidizing agents like potassium bromate (KBrO₃), often certified by NIST as SRM 83d for high accuracy.^[19] Oxalic acid (H₂C₂O₄) is commonly used to standardize potassium permanganate (KMnO₄) solutions, where it undergoes oxidation to carbon dioxide in sulfuric acid medium. For precipitation titrations, sodium chloride (NaCl) is utilized to standardize silver nitrate (AgNO₃) solutions, forming insoluble silver chloride (AgCl) via the reaction AgNO₃ + NaCl → AgCl + NaNO₃. These primary standards find essential applications in direct titrations and the preparation of secondary standards, ensuring precise concentration determinations. In direct titration, for instance, KHP is titrated with NaOH according to the reaction NaOH + C₈H₅KO₄ → C₈H₄KNaO₄ + H₂O, allowing calculation of the NaOH concentration as

C_{\text{NaOH}} = \frac{n_{\text{KHP}} \times M_{\text{KHP}}}{V_{\text{NaOH}}}

, where

n_{\text{KHP}}

is the moles of KHP,

M_{\text{KHP}}

is its molar mass (204.22 g/mol), and

V_{\text{NaOH}}

is the volume of NaOH used.^[18] Similarly, Na₂CO₃ standardizes HCl by titration, producing CO₂, H₂O, and NaCl, which is critical for preparing secondary acid solutions. Such processes underpin accuracy in industries, including pharmaceuticals for drug purity assays and environmental testing for pollutant quantification in water samples.^[20] Preparation of primary standards requires careful handling to preserve purity. For example, KHP must be dried at 110°C for 2 hours to remove moisture before use, as it is hygroscopic.^[21] Other standards like Na₂CO₃ are dried at higher temperatures (e.g., 250–300°C) to ensure anhydrous form.^[22] Post-drying, they are stored in desiccators over silica gel or phosphorus pentoxide to prevent reabsorption of atmospheric moisture, maintaining their integrity for extended periods.^[2] Failure to follow these steps can introduce errors up to 0.5% in concentration calculations. Compared to secondary standards, such as NaOH solutions, primary standards offer superior stability and do not require frequent re-standardization; secondaries are titrated against primaries due to their susceptibility to CO₂ absorption or decomposition, making primaries the foundation for reliable chemical analyses.^[23]

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