Source : Laboratoire du Dr B. Jill Venton – University of Virginia
L’objectif de nombreuses analyses chimiques est une analyse quantitative, où la quantité d’une substance dans un échantillon est déterminée. Afin de calculer avec précision la concentration d’un inconnu dans un échantillon, la préparation minutieuse est clé. Chaque fois qu’un échantillon est manipulé ou transféré, certains de l’échantillon peuvent être perdus. Il y a cependant, stratégies pour minimiser la perte de l’échantillon. Il y a aussi des stratégies pour faire face à la perte de l’échantillon et toujours en faisant des mesures précises de concentration.
Pour minimiser la perte de l’échantillon, l’idéal est de réduire au minimum le nombre d’étapes de manutention et de transfert échantillon. Par exemple, sa masse d’un échantillon solide directement dans une fiole qu’une solution se fera en réduit une étape de transfert. S’il est nécessaire de transférer d’un ballon à l’autre et une dilution est faite, puis triple rincer la verrerie permet de garantir que tout l’échantillon est transféré. Autres stratégies sont plus spécifiques à l’échantillon. Par exemple, les échantillons qui s’adsorber sur verre, comme les protéines, pourraient mieux être manipulés dans des tubes jetables en polypropylène. Les tubes ne sont pas hydrophiles, donc si une petite quantité d’échantillon doit être reversé dans l’eau, il est préférable d’avoir déjà ajouté l’eau dans le tube, donc l’échantillon peut être distribué directement dans le solvant. Il peut être préférable de se concentrer, plutôt que de les sécher complètement un échantillon, en raison de pertes d’insolubilities après réhydratation.
Une autre source de perte d’échantillon est par des manipulations échantillon incomplet. Par exemple, si une procédure de dérivation est utilisée et la dérivation est incomplète, alors la totalité de l’échantillon n’est pas observée. Les erreurs comme celle-ci sont des erreurs systématiques et peuvent être résolus en corrigeant le problème, comme la modification de la procédure de dérivation. Une autre cause de l’erreur systématique des mesures est des effets de matrice. Ceux-ci peuvent interférer avec la mesure de certaines substances et étalonnages performants dans la même matrice que l’échantillon peut réduire cet effet.
L’analyse quantitative est généralement effectuée à l’aide de normes soit externes ou internes. Pour des normes extérieures, une courbe d’étalonnage est faite en mesurant les différentes concentrations connues de l’analyte d’intérêt. Ensuite, l’échantillon est exécutée séparément de la norme. Pour les étalons internes, la norme est dans le même échantillon que l’analyte d’intérêt, ce qui permet la mesure à prendre en même temps. En règle générale, une espèce différente est ajoutée à l’appelé de l’étalon interne et le rapport de la réponse de l’étalon interne et l’analyte est calculé. L’idée est que le ratio de la réponse, appelé le facteur de réponse, est proportionnel à leur concentration. Alors que la méthode doit être en mesure de distinguer entre l’analyte d’intérêt et de l’étalon interne, les pertes d’échantillon qui se produisent après que l’étalon interne est ajouté devraient être similaires pour les deux substances et donc le ratio de la réponse reste la même. Un cas particulier de l’utilisation de normes internes est la méthode des ajouts dosés, où les quantités croissantes de l’analyte sont ajouté à la solution et le montant initial de l’analyte est calculée. Normes internes peuvent être utilisés en chromatographie, électrochimie et la spectroscopie.
Internal standards are used in many fields, including spectroscopy and chromatography. In spectroscopy, internal standards can help correct for random errors due to changes in light source intensity. If a lamp or other light source has variable power, it will affect the absorption and consequently, emission of a sample. However, the ratio of an internal standard to analyte will stay constant, even if the light source does not. One example of this is using lithium (Li) as an internal standard for the analysis of sodium in a blood sample by flame spectroscopy. Li is chemically similar to sodium but is not natively found in blood.
For chromatography, internal standards are often used in both gas chromatography and liquid chromatography. For applications with mass spectrometry as the detector, the internal standard can be an isotopically-labeled analyte, so that the molecular weight (MW) will be different than the analyte of interest. Internal standards are commonly used in pharmaceutical or environmental analyses.
Sample loss can occur every time a sample is handled or transferred, thereby making accurate calculations of concentration difficult.
To ensure accuracy, the effects of sample loss must be minimized using careful sample preparation and by limiting the number of sample handling and transfer steps. However, sample loss can also occur due to systematic errors, such as incomplete sample manipulation, matrix effects, and variations in analytic procedure.
These sources of loss can be accounted for by adding a known concentration of a species similar, but not identical, to the compound of interest. This is called an internal standard. Any sample losses that occur to the internal standard should be similar for the analyte, allowing for the concentration to be accurately calculated.
This video will illustrate the use of an internal standard and proper lab technique to account for sample loss when determining the concentration of an unknown.
An internal standard is a substance added in a known amount to standards, samples, and blanks during an analysis.
In chromatography and spectroscopy, the ratio of the signal for the internal standard and the analyte is calculated. This ratio, called the response factor, is proportional to the ratio of the analyte and standard concentrations.
Response factor, R, can be expressed by the following equation, where A represents the analytical signals of the sample and internal standard and C represents the concentrations of the sample and internal standard.
An internal standard can compensate for both systematic and random errors. For example, random errors—such as inconsistencies when measuring a sample—will be the same for both the internal standard and the analyte. Therefore, the ratio of their signals will not change.
For systematic errors, such as matrix effects in solution, the ratio will be unaffected as long as the matrix effect is equal for both the standard and the analyte.
While internal standards provide great benefit, it can be difficult to choose one that is suitable. An internal standard must have a signal that is similar, but not identical, to the analyte. It also cannot affect the measurement of the analyte in any way.
Finally, the concentration must be well known. This is achieved by ensuring that the internal standard is not natively present in the sample; thus, the only source of it in solution is the known concentration added.
In the following experiment, the concentration of caffeine in an unknown sample will be determined by gas chromatography.
This is achieved by creating a calibration curve using known caffeine solutions, with adenine as the internal standard. The slope of the calibration curve is equal to the response factor.
Once the response factor is known, the concentration of the unknown can be calculated from its measured chromatogram area ratio.
Now that you understand the basics of internal standards, let’s take a look at the procedure.
To begin the procedure, accurately weigh 100 mg of the internal standard, adenine, into a clean beaker.
Next, dissolve it in roughly 20 mL of dimethyl sulfoxide, and mix the solution.
Once the adenine has dissolved, pour the solution into a 50-mL volumetric flask.
Rinse the beaker and stir bar with 10 mL of DMSO, and pour the rinse into the flask. Repeat this rinse twice, to ensure proper solution transfer. Fill to the calibration mark, resulting in an internal standard with a concentration of 2 mg/mL.
Next, weigh 100 mg of caffeine into a beaker to prepare a stock solution. Dissolve the caffeine with a small amount of methanol. Then, use 3 rinses to transfer this solution to a fresh 25 mL volumetric flask. This is the 4 mg/mL stock solution. Use it to create 3 caffeine standards.
Next, add 0.2 mL of the internal standard, adenine, to each flask. Fill each to the final volume with methanol. Transfer each solution to a sample vial.
Run each caffeine standard through a gas chromatograph. Calculate the ratio of peak areas for the caffeine versus the adenine standard.
First, weigh 2 g of coffee into a 100-mL beaker, and record the weight.
Next, add 20 mL of methanol to extract the caffeine from the coffee. Allow the solution to stir for 20 min.
Using a Büchner funnel, filter out the coffee grounds. Rinse the beaker with a small amount of methanol, and pour this rinse into the funnel. Repeat the rinse twice.
Measure the final volume of the filtrate; it should be approximately 35 mL.
To prepare the sample for analysis, add 1 mL of the coffee extract to a sample vial. Then, add 0.2 mL of the adenine internal standard, and place the vial into the instrument’s auto-sampler rack.
Run a gas chromatography analysis of the sample, ensuring that the conditions are such that the caffeine and adenine are separate.
After completing the analysis, compute the peak area for both the internal standard and the analyte.
Once all the samples have been analyzed, the standard calibration curve can be determined for the caffeine/adenine solutions by plotting the ratios of the peak areas versus the ratios of the concentrations. The slope of this line, which represents the response factor, was 1.8.
Next, the GC data from the extracted coffee sample is analyzed. The ratio of the peak areas was calculated to be 1.78. Using the response factor and the known concentration of the internal standard, adenine, the concentration of caffeine in the unknown sample was calculated to be 0.33 mg/mL.
Many different types of reactions, across various scientific disciples, utilize internal standards to minimize the effects of errors and sample loss.
The effects of sample loss encountered during sample preparation can be minimized using internal standards, keeping their concentration ratio nearly constant.
In this example, bioactive lipids were extracted from lysed cells using a liquid-liquid extraction process. Stable isotope internal standards were added at the beginning of extraction to account for errors during sample preparation.
Internal standards were not only critical for the preparation of the bioactive lipids, but also for the analysis. The lipids were separated using high-performance liquid chromatography, and analyzed via mass spectrometry.
In spectroscopy, internal standards can help correct for random errors due to changes in light source intensity. If a lamp or other light source has variable power, it will affect the absorption and consequently, emission of a sample. However, the ratio of an internal standard to analyte will stay constant, even if the light source does not.
In chromatography, one of the largest sources of error is the injection. Auto-samplers help minimize this, but error can still be 1–2% relative standard deviation.
In this example, vapor standards containing an internal standard were analyzed using gas chromatography to establish a calibration curve. Once this was complete, the unknown sample could then be measured and the losses due to volatility of the sample accounted for.
You’ve just watched JoVE’s introduction to internal standards. You should now understand best practices for minimizing sample loss, internal standards, and response factors.
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