Principles of Instrumental Analysis
7th Edition
ISBN: 9781305577213
Author: Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Question
Chapter 33, Problem 33.8QAP
Interpretation Introduction
Interpretation:
The flow diagram for the following points is to be drawn-
First point is that the solvent peak is separated from the two analyte which has the lower volatility in comparison of the solvent.
Second point is that the solvent peak should not reach to the analytical column.
Third point is that the analytes which are different in polarity should be separated and determined quantitatively.
Concept introduction:
The flow diagram is depicted as the representation of workflow which includes the step-by-step approach to solve the complete task or to fulfill the given requirements.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
From a 10-mL sample, a 1-mL aliquot was taken and diluted to 100mL. From this, a 5-mL aliquot was taken and diluted to 20mL.The final 20mL was found to have a concentration of 0.004M analyte X.What is the concentration of analyte X in the 10-mL sample?
Introductlon
In Part (a) of this experiment you will prepare a primary standard. Potassium hydrogen phthalate
(KHP) is a monoprotic acid with the formula KHC,H.O. In this experiment KHP is used as the primary
standard. A standard solution is one whose solute concentration is accurately known. If a solute can
be obtained in a very pure, stable, weighable form, a primary standard solution of it can be
prepared directly. You will then use the standardized sodium hydroxide solution to determine the
acetic acid content of a dilute unknown solution.
Procedure
(0) Preparation of a Primory Standard
Potassium hydrogen phthalate (KHP) is a primary standard. Weigh accurately by difference,
approximately 0.8 g of KHP in a clean, dry weighing bottle and transfer it into a 250 ml conical
flask. Add 75 ml of distilled water. Swirl gently. Cover the flask and leave to dissolve, swirling
periodicaly. Cautlon: KHP is not highly soluble and care must be taken to ensure it is all
dissolved before you…
Briefly describe the principles for separating the components of a mixture by solvent extraction.
Knowledge Booster
Similar questions
- 16) Which of the following(s) is/are correct? I- Selectivity factor is the amount of time a solute spends in the stationary phase relative to the time it spends in mobile phase II- The retention time for an analyte is the time interval between its injection onto a column and its appearance at the detector at the other end of the column. III- Distribution constant is the ratio of the total solute concentration in the stationary phase to that in the mobile phase. A) I, II and III B) Only II C) I and III D) II and III E) Only III for GC2arrow_forward25 ml of pickled brine was taken from an apple pickled with vinegar and diluted to 500 ml, 25 ml of this was taken and acidity was determined with 0.2 N (Factor: 1.05) NaOH. In the main trials, 6.3 ml - 6.5 ml - 6.9 ml, respectively, 0.1 ml base was used in the analysis without using the sample.For example, how many ppm is its acidity?arrow_forwardYou find that for your analysis, your response factor (adjusted for internal standard) for a particular analyte was 0.0104 ppm. When you run a sample mixture, the integration for that component is 2,186, and the integration for the internal standard is 14,139. What is the concentration of the component in ppm? (Enter the numerical value without units.)arrow_forward
- 2. What is the basis for the separation of components of mixtures by paperchromatography?arrow_forwardBriefly explain the principles involved in the separation of the components of a mixture by solvent extraction.arrow_forwardA student was careful to make and stir all of her standard solutions immediately before measuring their turbidity for her calibration curve. However, she let her tap water solutions sit for 10 minutes prior to measuring their turbidity. If she measured the top portion of the solution, would her experimental sulfate ion concentration be higher or lower than it should be?arrow_forward
- Which of the following statements is true? A Liquids can be weighed using a weighing paper. B In weighing hygroscopic substances, containers should always be kept close when not in use. After drying a sample in the oven, you can place it immediately inside the analytical balance. D Place solid reagents / precipitates directly on top of the balance pan.arrow_forwardYou have 1000 μl of 1M NaCl stock solution (aq). How you would perform serial dilution to obtain 10-1, 10-2,…,10-5, 10-6M of NaCl solutions.arrow_forward(Concentration) You are tasked to prepare 300.000 ppb of a sodium carbonate standard for a titrimetric analysis. If you need to prepare 1000.00 (±0.06) mL of this solution, how much (in grams) solid, pure Na2CO3 are you supposed to dissolve? What absolute uncertainty is associated with your mass measurement if the prepared solution has a 0.1% percent relative uncertainty? Write your answer using the appropriate number of digits. Note that the formula mass of Na2CO3 is 105.9888 g/mol with negligible error. Assume that instrument precision is not a limitation in your lab. g (absolute error) How many significant figures does your reported mass have? (number of sig. figs.)arrow_forward
- 1. You begin by measuring 10.00 mg of dye on a precise analytical balance and dissolve the dye in 1.000 1 of water having density 998.25 kg/m³. What is the concentration of the dye in mg/l, kg/m³, mg/kg, and ppm?arrow_forwardWhich statement about the determination of the percentage purity of benzoic acid is correct? * A- Only sodium hydroxide solution can be used as the titrant in the volumetric analysis of benzoic acid. B- Analysing a benzoic acid sample that still contains some hydrochloric acid may yield an analyte percentage that is less than expected. C- Analysing a wet benzoic acid sample may yield an analyte percentage that is more than expected. D- All these statements are correct. E- None of these statements are correct.arrow_forwardWe obtain the value of the ebulloscopic increase of a solution with respect to the solvent. The measured boiling point for the solvent, with its absolute error, is 177±2°C; and that of the solution, 183±4°C. Indicate the statement that is correct.(A). From this experiment it is not possible to give a significant value for the ebulloscopic increase.(B). The ebulloscopic increase is 6±4°C.(C). The relative error in the measurement of the boiling temperature of the solution is twice the relative error in the measurement of the boiling temperature of the pure solvent.(D). The relative error of ebulloscopic magnification is, in round numbers, 2%.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Principles of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning