Chapter 19 instrument components
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This document summarizes the major components of instrumentation used in absorption and emission spectroscopy experiments. It discusses common light sources, wavelength selectors like monochromators and filters, sample containers, detectors such as phototubes and photodiode arrays, and examples of single beam and double beam spectrophotometers. Key components are the light source, wavelength selector to produce monochromatic radiation, sample holder, and detector to measure the detectable output over the wavelength region of interest.
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Topic 2 print
The accountant provided tax advice to a client on December 1, 20X3 but would not be paid until January 15, 20X4. Under accrual accounting, the accountant should record the revenue in 20X3 because accrual accounting records revenue in the period the service is provided, regardless of when payment is received. Accrual accounting attempts to record the financial effects of transactions in the period they occur rather than when cash is exchanged.
Topic 1 print (1)
This document provides an introduction to accounting. It defines accounting as a discipline that measures and communicates financial information about a business. It explains the accounting equation, the four core financial statements, and how to analyze business transactions by determining their impact on the accounting equation and each financial statement. Several examples of transaction analysis are provided and summarized.
Jr chapter 1
This document outlines the topics to be covered in a biochemistry course taught by Professor Jim Roesser. The course will discuss the importance of biochemistry in fields like agriculture, medicine, history and forensic science. It will also examine the composition and interactions of biological macromolecules like proteins, nucleic acids, carbohydrates and lipids, and how they carry out functions within living organisms. Students will learn about figures and tables illustrating key concepts like biomolecular structure, interaction and recognition.
Chapter 24 gc
Gas chromatography is a technique used to separate and analyze mixtures that rely on differences in volatility and affinity of compounds for a mobile and stationary phase. The key components of a gas chromatography system are a carrier gas, sample injection system, column, and detector. Factors like carrier gas type, column temperature, length, diameter, and stationary phase influence separation of compounds on the column. Common detectors include thermal conductivity, flame ionization, and electron capture detectors which have different properties in terms of sensitivity, selectivity, and response characteristics.
Chapter 25 lc harris
This document discusses liquid chromatography techniques. It describes liquid chromatography as using a liquid mobile phase and liquid or solid stationary phase. It then summarizes classical liquid chromatography and high performance liquid chromatography. High performance liquid chromatography uses smaller particle sizes in the stationary phase, stronger pumps, and detectors to allow for faster separations and better resolution compared to classical liquid chromatography. The document outlines the basic components of an HPLC system including the solvent delivery system, pump, injection port, analytical column, and various detector types. It also discusses different modes of liquid chromatography like normal phase and reverse phase.
Chromatography
This document provides an introduction and overview of chromatography. It discusses how chromatography separates a complex mixture into individual components based on interactions between a mobile and stationary phase. Different types of chromatography are described based on variations in the stationary and mobile phases used, including gas chromatography (GC), liquid chromatography (LC), high performance liquid chromatography (HPLC), thin layer chromatography (TLC), supercritical fluid chromatography (SFC), ion chromatography (IC), size exclusion, capillary zone electrophoresis (CZE), and affinity chromatography. Key terms used to describe chromatographic separations such as retention time, capacity factor, selectivity factor, resolution, number of theoretical plates, and plate height are also defined.
Solvent extraction
1) Solvent extraction is a technique used to separate components in a mixture based on differences in solubility between two immiscible liquid phases.
2) It involves transferring a solute from one liquid phase to another, such as transferring a compound from an aqueous phase to an organic phase like benzene.
3) The amount of solute extracted into each phase can be calculated using the partition coefficient K, which is a ratio of concentrations in the two phases at equilibrium.
Atomic spectroscopy ch 20
Atomic spectroscopy is used for qualitative and quantitative elemental analysis. It involves converting a sample into atoms, exciting the atoms, and measuring their absorption or emission of light. There are three main types of atomic spectroscopy: absorption, emission, and fluorescence spectroscopy. Samples are atomized using different heat sources like flames, furnaces, or plasma which convert the sample into gas phase atoms. The temperature of the heat source impacts the population of atoms in ground, excited, and ionized states. Instrumentation includes an atomization source, sample cell, monochromator, and detector. Detection limits range from parts-per-million to parts-per-trillion depending on the element and method used.
Chapter 17 spectroscopy
Spectroscopy involves the interaction of electromagnetic radiation with matter. Spectroscopic methods are used to elucidate molecular structure and quantify inorganic and organic compounds. There are several regions of the electromagnetic spectrum used including X-ray, UV, visible, and IR. Important concepts include Beer's law, which states absorbance is proportional to concentration, molar absorptivity, and path length. Spectrophotometry is used for qualitative and quantitative analysis in areas such as determining unknown concentrations. Fluorescence also provides a sensitive technique where molecules emit light at longer wavelengths after absorbing radiation.
Oxidation reduction titrations
This document discusses redox titration methods. It describes the Winkler method for determining dissolved oxygen in waste water and determining whether bacteria present are aerobic or anaerobic. The Karl Fischer method for determining water content is also outlined, using iodine, sulfur dioxide, and pyridine dissolved in methanol to quantitatively reduce iodine in the presence of water. Common oxidizing agents used in redox titrations include potassium permanganate, potassium bromate, cerium(IV), and potassium dichromate. Sodium thiosulfate is also described as a moderately strong standard reducing agent often used in indirect iodometric titrations to determine oxidizing agents.
Electrochemistry ch 14
This document provides an overview of electrochemistry concepts including oxidation-reduction reactions, oxidation numbers, balancing redox equations, and electrochemical cells. Key points are:
- Galvanic cells produce electrical energy from spontaneous redox reactions while electrolytic cells use electrical energy to drive non-spontaneous reactions.
- The standard cell potential (E°cell) is equal to the cathode potential minus the anode potential. All reactions must be written as reduction reactions.
- The Nernst equation relates cell potential to concentration and allows calculation of equilibrium constants.
- Memorable equations include ΔG° = -nFE° and E°cell = E°cathode - E°anode.
Statistics lectures
This document discusses experimental error in physical measurements. Every measurement has some degree of uncertainty. There are two main types of error - systematic errors which have an assignable cause and tend to be consistent in one direction, and random errors which are natural and unpredictable. Accuracy refers to how close a measurement is to the true value, while precision refers to the reproducibility of measurements. Proper evaluation of errors involves repetition of measurements, use of different methods, and statistical analysis to determine confidence intervals around results and identify outliers.
Edta
Here are the steps to solve this problem:
1) Volume of Ag+ solution = 25 mL
Moles of Ag+ = (0.0100 M) * (0.025 L) = 2.5 x 10-5 moles
2) Volume of EDTA solution = 15 mL
Moles of EDTA = (0.0200 M) * (0.015 L) = 3.0 x 10-5 moles
3) Ratio of Ag+ to EDTA is 1:1
Moles of AgEDTA formed = Minimum(Moles Ag+, Moles EDTA) = 2.5 x 10-5 moles
4) Kf' = α * Kf
Neutralization titrations
* HCl is a strong acid and will titrate first
* Its equivalence point was at 35.00 mL of NaOH
* NaOH concentration is 0.100 M
* Moles of NaOH used = Volume x Concentration
= 0.03500 L x 0.100 mol/L = 0.003500 mol
* Moles of HCl = Moles of NaOH used = 0.003500 mol
* H3PO4 is a weak acid and will titrate second
* Its equivalence point was at 50.00 mL of NaOH
* Additional NaOH used = 50.00 mL - 35.00 mL = 15.00 mL
* Moles of additional Na
Intro to titrations
The document discusses different types of titrations including acid-base, oxidation-reduction, complex formation, and precipitation reactions. It defines key terms like indicator, equivalence point, and endpoint. Examples are provided for calculating concentration using titration data from reactions like acid-base titrations for chloride in urine and carbon monoxide determination. Steps are outlined for the Kjeldahl method to determine nitrogen content through acid digestion and titration.
Complex equilbrium
This document discusses complex equilibrium in aqueous solutions involving multiple interacting species. It provides three examples of situations that can affect equilibrium: (1) when the solute interacts with itself or other species; (2) when the equilibrium constant is very small, requiring consideration of solvent contribution; and (3) in very dilute solutions where the solvent contribution is significant. Specific examples are worked through demonstrating how coupled equilibria and presence of other species can increase or decrease solubility compared to calculations considering only the main equilibrium reaction.
Chapter 7 activity
This document discusses how activity coefficients can explain the effect of inert salts on solubility and acid dissociation constants. It provides examples showing that a precipitate is more soluble and a weak acid dissociates more when the ionic strength is increased by adding an inert salt. This is because the activity coefficients of the ions are less than 1 and decrease with increasing ionic strength, making the activities higher than concentrations. The Debye-Huckel equation can be used to calculate activity coefficients based on ionic charge and strength.
Lecture 1 first day(1)
This document provides information about the Quantitative Analysis (CHEM 309) course including the instructor, textbook, grade breakdown, class objectives, and chapter overview. The grade is based on tests (70%), final (20%), and homework (10%). Students are expected to attend every class, participate daily with a clicker, and complete homework each night. The course covers topics like acid-base chemistry, analytical techniques, chemical measurements, and error analysis. Concentration units like molarity, formality, molality, and ppm/ppb are also discussed.
Weak acids and bases
This document contains several chemistry problems related to acids, bases, and pH calculations. It asks which weak acid would be the strongest in water between NH4+, HNO2, and HOCl based on their acid dissociation constants. It also asks about the conjugate base of HCO3- and whether KHCO3 produces an acidic, basic, or amphoteric solution in water. It provides several examples of calculating the pH of solutions containing HCl, NaF, acetic acid, HOCl, sodium acetate mixed with acetic acid, HClO4 with an organic acid, and sodium acetate on its own.
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Chapter 19 instrument components
- 1. Chapter 20: Instrumentation Major Components Depends on Type of Experiment Absorption Fluorescence Emission Source Wavelength Selector Sample Detector Signal Processor Most Common Placement depends on experiment
- 4. Instrument Components Light Source Detectable Output over wavelength region of interest Continuum Source Line Source From Skoog etal From Skoog, West, Holler
- 6. Common: Visible: Tungsten filament Lamp (320-2500 nm) UV- Deuterium Lamp (160-320 nm) IR: Heated Inert Solid (Globar, Nernst Glower) AA: Hollow cathode lamp (line source)
- 7. Instrument Components 2. Wavelength Selector Restrict radiation to a narrow band Two Types Filter – removes “wide” bands Monochromator
- 8. Monochromator A. Prism B. Grating •Lenses/mirrors to focus the radiation •Entrance and exit silts to restrict unwanted radiation •Dispersing Element to produce the “monochromatic” radiation
- 10. Instrument Components Bandwidth – wavelength range passed by selector High Quality: ~ 0.1 nm (monochromator) Filter 50 nm From Skoog, West, Holler
- 11. Sample Container Holds the sample Must be transparent in the region of interest UV: Quartz Vis: Glass IR: Salt Crystals
- 12. 1. In the equation, A = εbc, what quantity is represented by "ε" ? a) Absorptivity b) Molar absorptivity c) Path length d) Concentration 2. Can one measure a smaller amount of a compound if it has a high or low absorptivity a) higher b) lower
- 13. Instrument Components Radiation Detectors Stable Sensitive in region of interest Rapid Examples: Phototube Photomultiplier tube (most sensitive) Photodiode array (multichannel) CCD Heat detectors (IR)
- 14. Phototube From Skoog, West, Holler
- 15. PMT Why is it better then a phototube for measuring low light levels?
- 17. Types of Instruments Single Beam (Spectronic 20) Double Beam (separated in time or space) Multichannel Single Beam Spectrophotometer Simple, Inexpensive Wavelength range: 340 – 625 nm Bandwidth: 20 nm Wavelength accuracy: 2.5 nm
- 18. Spec 20 From Skoog, West, Holler
- 19. Double Beam Spectrophotometer More complex Compensates for drifts in detector/source Wavelength range: 195-850 nm Bandwidth: 4 nm Photometric accuracy: 0.5%T
- 22. Photodiode Array 200-1000 nm Resolution 1-2 nm Time: 0.1 s No scanning From Skoog, West, Holler Advantages/Disadvantages?
- 23. An 8.64 ppm solution of [FeSCN]Cl (149 g/mol) has a T of 0.295 at 580 nm when measured in a 1.00-cm cell. Calculate the molar absorptivity coefficient for the complex at this wavelength.
- 24. Cytochrome c has a molar absorptivity of 106,000 M-1 cm-1 . A solution is prepared by diluting a 10.0 uM solution by a hundred. What would be the absorbance of the diluted solution if measured in a 1.00 cm cell.