SI #11
•Download as DOC, PDF•
0 likes•339 views
The document contains 10 chemistry problems related to calculating molarity and percent composition of solutions, osmotic pressure, boiling points of solutions, definitions of hydrophilic and hydrophobic colloids, and identifying examples of each. It also contains 10 chemistry nomenclature problems to identify chemical formulas and names.
Report
Share
Report
Share
Recommended
Recognition of simple sugars
This document discusses simple sugars and how to identify them using Benedict's test. It summarizes that monosaccharides and some disaccharides are reducing sugars that will change color in Benedict's solution, indicating their presence. Polysaccharides are non-reducing and will not change color. The document then describes an experiment where unknown solutions A and B changed color in Benedict's test, indicating they contain reducing sugars like monosaccharides, while solution C did not change color, showing it contains a polysaccharide.
#11 Key
The document contains a chemistry problem set with 10 questions:
1) It asks to calculate the molarity of three aqueous solutions.
2) It asks to calculate the percentage by mass of nitric acid in a 16 M commercial solution.
3) It asks to calculate the osmotic pressure of a solution formed by dissolving aspirin in water.
4) It asks to order solutions by increasing boiling point.
5) It defines hydrophobic and hydrophilic colloids and provides examples.
6) It asks to identify colloids as hydrophobic or hydrophilic.
Preparation of tetraaminecopper(ii) sulphate complex
This document provides instructions for preparing tetraaminecopper(II) sulfate complex in 3 steps:
1) Dissolving copper sulfate in water and adding ammonium hydroxide to form an intense blue solution.
2) Adding ethanol and heating the solution to obtain a clear deep blue solution.
3) Allowing the hot solution to crystallize for an hour, filtering and drying the blue-purple tetraaminecopper(II) sulfate crystals. Yield of the product is then determined.
Coagulation
This document discusses the water treatment process of coagulation. Coagulation involves adding chemicals called coagulants to water to neutralize surface charges on particles and allow them to stick together and form larger particles that settle out via gravity. Key coagulants discussed are aluminum sulfate and ferric sulfate. The document also covers colloid stability, the coagulation process, properties of effective coagulants, and coagulant aids which add density and strength to the settling floc particles.
CHEMICAL TEST OF CARBOHYDRATES
This presentation includes chemical test of carbohydrates .
For more download PHARMACY INDIA APP or follow us on YOUTUBE & INSTAGRAM
Identification of sugars by molisch (1)
The document describes several tests used to identify different types of sugars:
1. Molisch's test identifies all carbohydrates using α-naphthol reagent to produce a purple color.
2. Fehling's test identifies reducing sugars by forming a brownish-red copper precipitate.
3. The osazone test identifies monosaccharides like glucose and fructose by forming characteristic needle or flower-shaped crystals.
4. Benedict's test also identifies reducing sugars, forming a copper precipitate under alkaline conditions.
5. Seliwanoff's test specifically identifies ketoses like fructose using resorcinol to form a red complex.
CRYSTAL_POSTER_FINAL_AMINOPHENOLS
1) The document describes experiments to grow single crystals of 4-amino-2,6-dichlorophenol and 3-diethylaminophenol through various methods like slow evaporation, vapor diffusion, and slow cooling to determine their crystal structures using X-ray diffraction.
2) Trials with 4-amino-2,6-dichlorophenol yielded single crystals that were analyzed via X-ray diffraction, revealing a monoclinic unit cell and hydrogen bonding interactions.
3) Efforts to grow 3-diethylaminophenol crystals faced challenges around solubility but some progress was made through slow evaporation of acidic solutions.
Liquid crystals
Liquid crystals were first discovered in the 1890s when observing cholesterol, they flow like liquids but have a repeating crystalline pattern and two melting points. There are three main types of liquid crystals - thermotropic which are the most common and flow like liquids, useful in displays; lyotropic which use a solvent and contain both hydrophobic and hydrophilic parts; and metallotropic which are similar to lyotropic but contain metals affecting melting points. Liquid crystals find applications in electronic displays like televisions, watches, phones and more through liquid crystal displays, as well as in soap, conducting foams and observing cholesterol.
Recommended
Recognition of simple sugars
This document discusses simple sugars and how to identify them using Benedict's test. It summarizes that monosaccharides and some disaccharides are reducing sugars that will change color in Benedict's solution, indicating their presence. Polysaccharides are non-reducing and will not change color. The document then describes an experiment where unknown solutions A and B changed color in Benedict's test, indicating they contain reducing sugars like monosaccharides, while solution C did not change color, showing it contains a polysaccharide.
#11 Key
The document contains a chemistry problem set with 10 questions:
1) It asks to calculate the molarity of three aqueous solutions.
2) It asks to calculate the percentage by mass of nitric acid in a 16 M commercial solution.
3) It asks to calculate the osmotic pressure of a solution formed by dissolving aspirin in water.
4) It asks to order solutions by increasing boiling point.
5) It defines hydrophobic and hydrophilic colloids and provides examples.
6) It asks to identify colloids as hydrophobic or hydrophilic.
Preparation of tetraaminecopper(ii) sulphate complex
This document provides instructions for preparing tetraaminecopper(II) sulfate complex in 3 steps:
1) Dissolving copper sulfate in water and adding ammonium hydroxide to form an intense blue solution.
2) Adding ethanol and heating the solution to obtain a clear deep blue solution.
3) Allowing the hot solution to crystallize for an hour, filtering and drying the blue-purple tetraaminecopper(II) sulfate crystals. Yield of the product is then determined.
Coagulation
This document discusses the water treatment process of coagulation. Coagulation involves adding chemicals called coagulants to water to neutralize surface charges on particles and allow them to stick together and form larger particles that settle out via gravity. Key coagulants discussed are aluminum sulfate and ferric sulfate. The document also covers colloid stability, the coagulation process, properties of effective coagulants, and coagulant aids which add density and strength to the settling floc particles.
CHEMICAL TEST OF CARBOHYDRATES
This presentation includes chemical test of carbohydrates .
For more download PHARMACY INDIA APP or follow us on YOUTUBE & INSTAGRAM
Identification of sugars by molisch (1)
The document describes several tests used to identify different types of sugars:
1. Molisch's test identifies all carbohydrates using α-naphthol reagent to produce a purple color.
2. Fehling's test identifies reducing sugars by forming a brownish-red copper precipitate.
3. The osazone test identifies monosaccharides like glucose and fructose by forming characteristic needle or flower-shaped crystals.
4. Benedict's test also identifies reducing sugars, forming a copper precipitate under alkaline conditions.
5. Seliwanoff's test specifically identifies ketoses like fructose using resorcinol to form a red complex.
CRYSTAL_POSTER_FINAL_AMINOPHENOLS
1) The document describes experiments to grow single crystals of 4-amino-2,6-dichlorophenol and 3-diethylaminophenol through various methods like slow evaporation, vapor diffusion, and slow cooling to determine their crystal structures using X-ray diffraction.
2) Trials with 4-amino-2,6-dichlorophenol yielded single crystals that were analyzed via X-ray diffraction, revealing a monoclinic unit cell and hydrogen bonding interactions.
3) Efforts to grow 3-diethylaminophenol crystals faced challenges around solubility but some progress was made through slow evaporation of acidic solutions.
Liquid crystals
Liquid crystals were first discovered in the 1890s when observing cholesterol, they flow like liquids but have a repeating crystalline pattern and two melting points. There are three main types of liquid crystals - thermotropic which are the most common and flow like liquids, useful in displays; lyotropic which use a solvent and contain both hydrophobic and hydrophilic parts; and metallotropic which are similar to lyotropic but contain metals affecting melting points. Liquid crystals find applications in electronic displays like televisions, watches, phones and more through liquid crystal displays, as well as in soap, conducting foams and observing cholesterol.
LCR Hallcrest Handbook of Liquid Crystal Technology RT006 rev01 usa
This document provides an introduction to thermochromic liquid crystals (TLCs), including the different types of TLC mixtures, their color change properties, applications, and Hallcrest's product range. TLCs are mixtures of organic chemicals that change color reversibly with temperature. The three major types are cholesteric, chiral nematic, and combination mixtures. TLCs are used in temperature indicators, cosmetics, research, and other applications. Hallcrest offers TLC products, a custom microencapsulation service, and tailors products to specific customer needs.
The Characterization of Carbohydrates
Benedict's reagent is used to test for reducing sugars like glucose, lactose, and fructose. It contains copper sulfate that is reduced to copper oxide when heated with reducing sugars, causing a color change from blue to green, brick red, or brown. Benedict's reagent can also detect glucose in urine samples to test for diabetes. Barfoed's reagent is similar but uses acetic acid, allowing it to distinguish between mono- and disaccharides. Disaccharides do not react for up to 10 minutes while monosaccharides form a blue or green precipitate. Sucrose is hydrolyzed using acid or enzyme to form glucose and fructose in the inversion test.
Chemistry
Sulphuric acid is an important chemical used to make fertilizers like ammonium sulphate and potassium sulphate through reactions with ammonia and potassium hydroxide respectively. It is also used to make detergents, synthetic fibers, paint pigments, and as an electrolyte in car batteries. Sulphuric acid is manufactured through the contact process, which involves burning sulfur with air to produce sulfur dioxide, converting the sulfur dioxide to sulfur trioxide using a vanadium catalyst, and dissolving the trioxide in concentrated sulfuric acid to produce oleum and then diluting it to make concentrated sulfuric acid. Burning of fossil fuels produces sulfur dioxide pollution which dissolves in water to form acidic rain
Test For Carbohydrate
This document summarizes several common chemical tests used to detect carbohydrates, including Fehling's reagent, Benedict's reagent, Barfoed's reagent, and the Molisch test. It also describes methods for reducing sugars using sodium amalgam, strong acids, and dilute alkalies. These tests and reduction methods allow distinguishing between mono- and disaccharides and identifying "reducing" sugars that give positive tests without prior hydrolysis.
Qualitative tests to identify functional groups of carbohydrates
test for carbohydrates, molisch's test, benedict's test, iodine test, seliwanoff's test, osazone tests
CHEMICAL TEST & IMPORTANCE OF CARBOHYDRATES
The document discusses tests used to identify carbohydrates from unknown sources, including the Molisch test, Benedict's test, Barfoed's test, and Seliwanoff's test. It also describes how to distinguish between glucose and fructose using bromine water oxidation and lists pharmaceutical uses of glucose and fructose such as in foods, medicines, and supplements.
Tests for Carbohydrates
This document describes several common tests used to identify different types of carbohydrates:
- Molisch test is a general test for all carbohydrates that involves using concentrated sulfuric acid and α-naphthol to form colored compounds.
- Benedict's test uses copper sulfate and heat to detect reducing sugars, forming a red copper (II) oxide precipitate.
- Bial's test detects pentoses using orcinol and ferric ions to form a blue color.
- Osazone tests form characteristic crystal shapes when reducing sugars are heated with phenylhydrazine.
- Mucic acid test detects galactose by forming a white precipitate of mucic acid with nitric
Chemical List
This document lists 35 different chemicals including reagents like Fehling's solution, indicators such as starch paper, metals such as calcium, solvents like hexane and propanol, and laboratory equipment including a thermometer.
BIO201: Chlorine Chemistry
Chlorine is effective as both a sanitizer and oxidizer in pools. As a sanitizer, chlorine kills bacteria and microorganisms. As an oxidizer, it chemically breaks down and removes contaminants from the water. The primary sanitizing agent resulting from chlorine products is hypochlorous acid. Hypochlorous acid exists in equilibrium with hypochlorite ions, and the ratio depends on pH. At a pH of 7.5 the ratio is equal, favoring HOCl at lower pH and OCl- at higher pH. Hypochlorous acid is the most effective form of chlorine sanitizer. Stabilized chlorine products contain isocyanurates that bond chlorine
SMART WORK FOR GEAT SUCCESS (SHIRISHA REDDYMALLA)
This document contains short answer questions about surface chemistry concepts including different types of adsorption and their characteristics, the classification of emulsions with examples, how catalysis is classified with two examples, the mechanism of micelle formation and cleaning action of soap, how colloids are classified based on interaction between dispersed and dispersion phases, identifying dispersed and dispersion phases in various colloid systems, what coagulation is with an example, how colloidal solutions are classified with examples, and explaining the terms electrophoresis, coagulation, and Tyndall effect.
Reactions of lactose & maltose
The document describes several tests used to identify carbohydrates and sugars:
- Molisch's test uses α-naphthol to detect the presence of carbohydrates, forming a reddish-violet ring.
- Benedict's test uses copper sulfate to detect reducing sugars, forming different colored precipitates.
- Barfoed's test distinguishes monosaccharides from disaccharides by their reaction speed.
- Phenylhydrazine forms characteristic crystals (osazones) with different sugars that can be viewed under a microscope.
Adhesion guideline
The document discusses the use of silanes as adhesion promoters. It describes how silanes work by forming covalent bonds between substrates and polymeric resins. This improves adhesion, which is often poor without chemical bonding. The document outlines the basic chemistry of silanes, including their hydrolysis reaction and how they can form monolayers or multilayers on surfaces. It discusses different types of silanes and their properties. Examples are given of how silanes can promote alignment of liquid crystals and interact with active substrate surfaces like glass. The document provides figures to illustrate the mechanisms and chemistry of silane deposition and crosslinking. It also lists some potential reactions of functionalized silane surfaces.
Biomolecules ; CARBOHYDRATES
This document provides an overview of biomolecules and carbohydrates. It begins with an introduction to biomolecules, which are organic compounds that are essential for life. Biomolecules are then classified as either macromolecules or micromolecules. The document focuses on carbohydrates, discussing their classification into monosaccharides, oligosaccharides, and polysaccharides. Key aspects of carbohydrates covered include their chemical structure, isomerism, and common reactions. Finally, the biological roles of carbohydrates in the body are summarized.
Removal of chromium
Chromium is a metal that exists in several oxidation
• Chromium is a metal that exists in several oxidation or valence states, ranging from chromium (-II) to chromium (+VI).
• Chromium compounds are very stable in the trivalent state and occur naturally in this state in ores such as ferrochromite, or chromite ore.
• Chrome III is an essential nutrient for maintaining blood glucose levels
• The hexavalent, Cr(VI) or chromate, is the second most stable state. It rarely occurs naturally.
5th Lecture on Adsorption and Colloids | Chemistry Part II | 11th Std
The document discusses emulsions and colloids. It defines emulsions as a colloidal system where one immiscible liquid is dispersed in another. There are two types of emulsions: oil-in-water and water-in-oil. Oil-in-water emulsions have oil as the dispersed phase in water, like milk. Water-in-oil emulsions have water as the dispersed phase in oil, like cod liver oil. Colloids find applications in electrical precipitation of smoke, purification of drinking water using alum, and medicines like argyrol which use the large surface area of colloidal particles.
Qualitative tests for carbohydrates
1. The document describes various qualitative tests that can be used to identify different types of carbohydrates, including monosaccharides, disaccharides, and polysaccharides.
2. Key tests described include the Molisch test, Benedict's test, Barfoed's test, Seliwanoff's test, and the hydrolysis test for sucrose. Each test exploits a unique chemical property of carbohydrates to indicate their presence.
3. The tests allow identification of carbohydrates by the color change produced, crystalline structure of osazones formed, or ability to reduce copper or show color change with reagents like iodine. Taken together, the battery of tests can determine the identity of an unknown carbohydrate sample.
Qualitative analysis of carbohydrates
The document describes various chemical tests used to identify different types of carbohydrates. It provides details of the Molisch test, Iodine test, Benedict's test, Barfoed's test, Seliwanoff's test, and other reactions. These tests help identify carbohydrates based on properties of hydroxyl and carbonyl groups and whether they are reducing sugars, monosaccharides, polysaccharides, or disaccharides. Reaction results are provided to systematically identify and differentiate between glucose, fructose, lactose, maltose, sucrose, and starch.
Solutions and suspension worksheet answer
This document provides answers to solutions and suspension worksheet questions. Section A lists multiple choice answers. Section B defines key terms like solute and solvent, and lists factors that increase dissolving rates. Section C discusses experiments comparing how surface area and physical state impact dissolving rates, and defines the difference between a solution and suspension.
#23
The document contains a chemistry practice exam with 10 multiple-choice and short-answer questions testing concepts such as how the percent dissociation of a weak acid changes with concentration, calculating percent dissociation and acid dissociation constants given various parameters, determining pH and pOH values of solutions, and identifying chemical reactions between acids and bases in aqueous solutions.
SI #3 Key
1. The document discusses key concepts from general chemistry including:
- The van der Waals equation accounting for non-zero particle volumes and interparticle interactions.
- Using the ideal gas law to calculate changes in volume with temperature changes.
- The value of the gas constant R at standard temperature and pressure.
- Conversions between various pressure and volume units.
- Calculating moles, pressure, volume, and number of molecules using the ideal gas law.
Information Page
This page details my contact info, office hours, SI session hours and has some additional information.
SI #9
The document is a practice exam for general chemistry II that contains 10 multiple choice questions testing knowledge of intermolecular forces, phase changes, concentrations, vapor pressure, and nomenclature. It asks about the forces between molecules, which substance experiences only dispersion forces, the process of molecules sticking to a surface, the energy required to expand a liquid's surface area, the vapor pressure at the normal boiling point, the concentration of nitrate ions in a solution, the direct change of a solid to a gas, and the phase changes of water freezing and drying and frost forming. It concludes by listing the names and symbols of 10 chemical substances and compounds.
More Related Content
What's hot
LCR Hallcrest Handbook of Liquid Crystal Technology RT006 rev01 usa
This document provides an introduction to thermochromic liquid crystals (TLCs), including the different types of TLC mixtures, their color change properties, applications, and Hallcrest's product range. TLCs are mixtures of organic chemicals that change color reversibly with temperature. The three major types are cholesteric, chiral nematic, and combination mixtures. TLCs are used in temperature indicators, cosmetics, research, and other applications. Hallcrest offers TLC products, a custom microencapsulation service, and tailors products to specific customer needs.
The Characterization of Carbohydrates
Benedict's reagent is used to test for reducing sugars like glucose, lactose, and fructose. It contains copper sulfate that is reduced to copper oxide when heated with reducing sugars, causing a color change from blue to green, brick red, or brown. Benedict's reagent can also detect glucose in urine samples to test for diabetes. Barfoed's reagent is similar but uses acetic acid, allowing it to distinguish between mono- and disaccharides. Disaccharides do not react for up to 10 minutes while monosaccharides form a blue or green precipitate. Sucrose is hydrolyzed using acid or enzyme to form glucose and fructose in the inversion test.
Chemistry
Sulphuric acid is an important chemical used to make fertilizers like ammonium sulphate and potassium sulphate through reactions with ammonia and potassium hydroxide respectively. It is also used to make detergents, synthetic fibers, paint pigments, and as an electrolyte in car batteries. Sulphuric acid is manufactured through the contact process, which involves burning sulfur with air to produce sulfur dioxide, converting the sulfur dioxide to sulfur trioxide using a vanadium catalyst, and dissolving the trioxide in concentrated sulfuric acid to produce oleum and then diluting it to make concentrated sulfuric acid. Burning of fossil fuels produces sulfur dioxide pollution which dissolves in water to form acidic rain
Test For Carbohydrate
This document summarizes several common chemical tests used to detect carbohydrates, including Fehling's reagent, Benedict's reagent, Barfoed's reagent, and the Molisch test. It also describes methods for reducing sugars using sodium amalgam, strong acids, and dilute alkalies. These tests and reduction methods allow distinguishing between mono- and disaccharides and identifying "reducing" sugars that give positive tests without prior hydrolysis.
Qualitative tests to identify functional groups of carbohydrates
test for carbohydrates, molisch's test, benedict's test, iodine test, seliwanoff's test, osazone tests
CHEMICAL TEST & IMPORTANCE OF CARBOHYDRATES
The document discusses tests used to identify carbohydrates from unknown sources, including the Molisch test, Benedict's test, Barfoed's test, and Seliwanoff's test. It also describes how to distinguish between glucose and fructose using bromine water oxidation and lists pharmaceutical uses of glucose and fructose such as in foods, medicines, and supplements.
Tests for Carbohydrates
This document describes several common tests used to identify different types of carbohydrates:
- Molisch test is a general test for all carbohydrates that involves using concentrated sulfuric acid and α-naphthol to form colored compounds.
- Benedict's test uses copper sulfate and heat to detect reducing sugars, forming a red copper (II) oxide precipitate.
- Bial's test detects pentoses using orcinol and ferric ions to form a blue color.
- Osazone tests form characteristic crystal shapes when reducing sugars are heated with phenylhydrazine.
- Mucic acid test detects galactose by forming a white precipitate of mucic acid with nitric
Chemical List
This document lists 35 different chemicals including reagents like Fehling's solution, indicators such as starch paper, metals such as calcium, solvents like hexane and propanol, and laboratory equipment including a thermometer.
BIO201: Chlorine Chemistry
Chlorine is effective as both a sanitizer and oxidizer in pools. As a sanitizer, chlorine kills bacteria and microorganisms. As an oxidizer, it chemically breaks down and removes contaminants from the water. The primary sanitizing agent resulting from chlorine products is hypochlorous acid. Hypochlorous acid exists in equilibrium with hypochlorite ions, and the ratio depends on pH. At a pH of 7.5 the ratio is equal, favoring HOCl at lower pH and OCl- at higher pH. Hypochlorous acid is the most effective form of chlorine sanitizer. Stabilized chlorine products contain isocyanurates that bond chlorine
SMART WORK FOR GEAT SUCCESS (SHIRISHA REDDYMALLA)
This document contains short answer questions about surface chemistry concepts including different types of adsorption and their characteristics, the classification of emulsions with examples, how catalysis is classified with two examples, the mechanism of micelle formation and cleaning action of soap, how colloids are classified based on interaction between dispersed and dispersion phases, identifying dispersed and dispersion phases in various colloid systems, what coagulation is with an example, how colloidal solutions are classified with examples, and explaining the terms electrophoresis, coagulation, and Tyndall effect.
Reactions of lactose & maltose
The document describes several tests used to identify carbohydrates and sugars:
- Molisch's test uses α-naphthol to detect the presence of carbohydrates, forming a reddish-violet ring.
- Benedict's test uses copper sulfate to detect reducing sugars, forming different colored precipitates.
- Barfoed's test distinguishes monosaccharides from disaccharides by their reaction speed.
- Phenylhydrazine forms characteristic crystals (osazones) with different sugars that can be viewed under a microscope.
Adhesion guideline
The document discusses the use of silanes as adhesion promoters. It describes how silanes work by forming covalent bonds between substrates and polymeric resins. This improves adhesion, which is often poor without chemical bonding. The document outlines the basic chemistry of silanes, including their hydrolysis reaction and how they can form monolayers or multilayers on surfaces. It discusses different types of silanes and their properties. Examples are given of how silanes can promote alignment of liquid crystals and interact with active substrate surfaces like glass. The document provides figures to illustrate the mechanisms and chemistry of silane deposition and crosslinking. It also lists some potential reactions of functionalized silane surfaces.
Biomolecules ; CARBOHYDRATES
This document provides an overview of biomolecules and carbohydrates. It begins with an introduction to biomolecules, which are organic compounds that are essential for life. Biomolecules are then classified as either macromolecules or micromolecules. The document focuses on carbohydrates, discussing their classification into monosaccharides, oligosaccharides, and polysaccharides. Key aspects of carbohydrates covered include their chemical structure, isomerism, and common reactions. Finally, the biological roles of carbohydrates in the body are summarized.
Removal of chromium
Chromium is a metal that exists in several oxidation
• Chromium is a metal that exists in several oxidation or valence states, ranging from chromium (-II) to chromium (+VI).
• Chromium compounds are very stable in the trivalent state and occur naturally in this state in ores such as ferrochromite, or chromite ore.
• Chrome III is an essential nutrient for maintaining blood glucose levels
• The hexavalent, Cr(VI) or chromate, is the second most stable state. It rarely occurs naturally.
5th Lecture on Adsorption and Colloids | Chemistry Part II | 11th Std
The document discusses emulsions and colloids. It defines emulsions as a colloidal system where one immiscible liquid is dispersed in another. There are two types of emulsions: oil-in-water and water-in-oil. Oil-in-water emulsions have oil as the dispersed phase in water, like milk. Water-in-oil emulsions have water as the dispersed phase in oil, like cod liver oil. Colloids find applications in electrical precipitation of smoke, purification of drinking water using alum, and medicines like argyrol which use the large surface area of colloidal particles.
Qualitative tests for carbohydrates
1. The document describes various qualitative tests that can be used to identify different types of carbohydrates, including monosaccharides, disaccharides, and polysaccharides.
2. Key tests described include the Molisch test, Benedict's test, Barfoed's test, Seliwanoff's test, and the hydrolysis test for sucrose. Each test exploits a unique chemical property of carbohydrates to indicate their presence.
3. The tests allow identification of carbohydrates by the color change produced, crystalline structure of osazones formed, or ability to reduce copper or show color change with reagents like iodine. Taken together, the battery of tests can determine the identity of an unknown carbohydrate sample.
Qualitative analysis of carbohydrates
The document describes various chemical tests used to identify different types of carbohydrates. It provides details of the Molisch test, Iodine test, Benedict's test, Barfoed's test, Seliwanoff's test, and other reactions. These tests help identify carbohydrates based on properties of hydroxyl and carbonyl groups and whether they are reducing sugars, monosaccharides, polysaccharides, or disaccharides. Reaction results are provided to systematically identify and differentiate between glucose, fructose, lactose, maltose, sucrose, and starch.
Solutions and suspension worksheet answer
This document provides answers to solutions and suspension worksheet questions. Section A lists multiple choice answers. Section B defines key terms like solute and solvent, and lists factors that increase dissolving rates. Section C discusses experiments comparing how surface area and physical state impact dissolving rates, and defines the difference between a solution and suspension.
What's hot (18)
LCR Hallcrest Handbook of Liquid Crystal Technology RT006 rev01 usa
LCR Hallcrest Handbook of Liquid Crystal Technology RT006 rev01 usa
Qualitative tests to identify functional groups of carbohydrates
Qualitative tests to identify functional groups of carbohydrates
5th Lecture on Adsorption and Colloids | Chemistry Part II | 11th Std
5th Lecture on Adsorption and Colloids | Chemistry Part II | 11th Std
Viewers also liked
#23
The document contains a chemistry practice exam with 10 multiple-choice and short-answer questions testing concepts such as how the percent dissociation of a weak acid changes with concentration, calculating percent dissociation and acid dissociation constants given various parameters, determining pH and pOH values of solutions, and identifying chemical reactions between acids and bases in aqueous solutions.
SI #3 Key
1. The document discusses key concepts from general chemistry including:
- The van der Waals equation accounting for non-zero particle volumes and interparticle interactions.
- Using the ideal gas law to calculate changes in volume with temperature changes.
- The value of the gas constant R at standard temperature and pressure.
- Conversions between various pressure and volume units.
- Calculating moles, pressure, volume, and number of molecules using the ideal gas law.
Information Page
This page details my contact info, office hours, SI session hours and has some additional information.
SI #9
The document is a practice exam for general chemistry II that contains 10 multiple choice questions testing knowledge of intermolecular forces, phase changes, concentrations, vapor pressure, and nomenclature. It asks about the forces between molecules, which substance experiences only dispersion forces, the process of molecules sticking to a surface, the energy required to expand a liquid's surface area, the vapor pressure at the normal boiling point, the concentration of nitrate ions in a solution, the direct change of a solid to a gas, and the phase changes of water freezing and drying and frost forming. It concludes by listing the names and symbols of 10 chemical substances and compounds.
SI #10
This document contains 11 multiple choice and short answer questions about concepts in general chemistry including: solvent-solute interactions, hydration, enthalpy of solution, colligative properties, molality calculations, definitions of colloid and miscibility, concentration calculations involving mass percent and ppm, and molality calculations for solutions.
#17
This document contains 7 questions regarding chemical equilibrium calculations. The questions involve writing equilibrium constants, calculating equilibrium constants based on given partial pressures or concentrations at equilibrium, and determining unknown values at equilibrium given some known values. Specifically, it asks the student to:
1) Write the equilibrium constant expression for a dissolution reaction.
2) Write the equilibrium constant expression for a complex ion formation reaction.
3) Calculate the equilibrium constant for a decomposition reaction given partial pressures at equilibrium.
4) Calculate the equilibrium constant for a decomposition reaction given partial pressures at equilibrium.
5) Calculate the equilibrium constant for a reaction given partial pressures in a container at equilibrium.
6) Calculate unknown concentrations and the equilibrium constant for a reaction given initial
#23 Key
The document discusses chemical reactions and calculations involving acids, bases, and their dissociation in solution. It begins by explaining that the percent dissociation of a weak acid decreases as its concentration increases. It then shows examples of calculating percent dissociation and acid dissociation constants (Ka) for hydrocyanic acid solutions. Similarly, it demonstrates calculating percent dissociation and pKa for ammonia solutions. Finally, it asks and answers questions about whether and why certain acid-base reactions will or will not occur when the solutions are mixed, such as sodium chloride dissolving in water.
Si #13
This document contains 7 questions about chemical kinetics and equilibrium concepts. Question 1 involves calculating amounts of N2O5 remaining and half-life during its decomposition reaction. Question 2 concerns rate laws and reaction orders. Question 3 provides rate data and asks about rate laws and rates for the decomposition of N2O5. Question 4 gives a rate law and asks about reaction rates. Question 5 asks about the law of mass action. Question 6 asks to write equilibrium constants for 3 reactions. Question 7 asks which reactions favor products or reactants based on given equilibrium constants.
SI #1 Key
The document provides information about key concepts in general chemistry including the definitions of matter, homogeneous mixtures, and pressure. It also summarizes several gas laws including Boyle's law that pressure and volume are inversely proportional at constant temperature and amount, Charles' law that volume is directly proportional to temperature at constant pressure and amount, and Avogadro's law relating volume and amount of gas particles. Sample problems are provided to demonstrate how to use the gas laws and equations of state to calculate pressure, volume, temperature and amount in gas systems.
SI #7
This document contains questions about chemistry concepts and definitions. It asks to define critical temperature and strong electrolyte, and explains that hydration refers to water molecules surrounding ions when strong electrolytes dissolve in water. It also asks how temperature, molecular weight, and intermolecular forces affect a molecule's viscosity. Finally, it lists the names or formulas of 20 chemical substances.
#19
This document covers Bronsted-Lowry acids and bases, conjugate acids and bases, and acid-base equilibrium. It defines Bronsted-Lowry acids as proton donors and bases as proton acceptors. Conjugate acids are formed when a base gains a proton, and conjugate bases are formed when an acid loses a proton. Several examples of conjugate acid-base pairs are given. The document also discusses how the strength of an acid or base determines the position of acid-base equilibrium and the autoionization process and ion product constant for water.
#10 Key
This document provides definitions and examples of key concepts in general chemistry including:
1. Solvation refers to the attractive interaction between solvent molecules and a solute. Hydration describes the interaction when water is the solvent.
2. The overall enthalpy change of a solution can be either positive (endothermic) or negative (exothermic).
3. A saturated solution is one in equilibrium with undissolved solute where dissolution and crystallization occur at equal rates. Unsaturated and supersaturated solutions contain less or more solute respectively.
4. Colligative properties include vapor pressure depression, freezing point depression, boiling point elevation, and osmotic pressure.
#26
The document discusses solubility and solubility products, oxidation-reduction reactions, and voltaic cells. It defines key concepts like reducing agents, oxidizing agents, and half-reactions. It also discusses standard reduction potentials, how to determine if a reaction involves oxidation-reduction, and how to balance half-reactions to indicate oxidation or reduction. Sample problems are provided to calculate equilibrium constants from solubility products and oxidation states in reactions.
#25
The document provides 10 questions related to general chemistry concepts including:
1) Defining the common ion effect and buffer capacity
2) Providing the Henderson-Hasselbalch equation
3) Calculating the pH of different buffer solutions
#24
1. The document provides 7 chemistry problems involving calculations of pH, concentrations of products and reactants from acid-base reactions involving strong acids and bases, and identification of types of acids.
2. Problems 1-3 involve calculating the pH of strong acid solutions given molar concentrations.
3. Problems 4-6 require using given volumes, molarities, and extent of ionization to calculate concentrations of products and reactants.
4. Problems 7-9 ask about common weak bases, relationships between types of acids, and identification of more acidic salt solutions.
Key SI #6
Intermolecular forces exist between molecules, while intramolecular forces exist within molecules. Melting points increase as intermolecular forces strengthen. Polar molecules have partial charges and can form ion-dipole attractions. The main intermolecular forces are London dispersion, dipole-dipole, and hydrogen bonding. Ionic and covalent bonds are stronger than any intermolecular force within a molecule. A flow chart determines the dominant intermolecular force based on whether ions or polar molecules are present.
Si #15
The document discusses reaction rates and kinetics. It defines reaction rate and states that the concentration of reactants is proportional to the rate of reaction. It also defines the rate constant and rate law formula. A catalyst affects the reaction rate by lowering the activation energy, increasing the frequency of collisions, and increasing the probability of successful collisions. Enzymes are biological catalysts and the collision theory states that for a reaction to occur, reactant particles must collide with adequate energy.
Si #15 Key
The document defines key concepts related to reaction rates in chemistry:
1) Reaction rate is defined as the change in concentration of a reactant or product with time.
2) The rate formula relates the rate of a reaction to the change in concentration of a reactant or product over time.
3) The concentration of reactants is directly proportional to the rate of reaction according to the rate formula.
4) A catalyst increases the reaction rate by participating in the reaction without being consumed and allowing collisions between molecules to result in reaction at lower energies.
SI #8
1. The document is a study guide for a General Chemistry II exam that covers topics like ionic bonding, covalent bonding, polarity, intermolecular forces, phase diagrams, vapor pressure, and nomenclature.
2. It includes multiple choice questions about the transfer of electrons in ionic bonding, shared electron pairs in covalent bonding, what defines a polar covalent bond, and properties of polar and nonpolar molecules.
3. Questions also address which substances have higher boiling points due to stronger intermolecular forces, defining a phase diagram, identifying the critical temperature on a phase diagram, and which solute will have the lowest vapor pressure in solution.
SI #2 Key
This document provides 13 multiple choice and calculation questions about key concepts in general chemistry including the ideal gas law, density, molar mass, reaction stoichiometry involving gases, and gas behavior. It tests understanding of gas laws, calculations using the ideal gas equation, and properties that affect how real gases deviate from ideal behavior. The final question indicates that an ideal gas is distinguished from real gases by the fact that ideal gas molecules have no attraction for one another.
Similar to SI #11
Solution and colligative numerical 2016
The document provides examples of calculating various properties of solutions such as percentage by mass, mole fraction, molarity, molality, vapor pressure depression, boiling point elevation, and Henry's law constant. It includes 18 examples involving dissolving various solutes like glucose, methyl alcohol, benzene, HCl, NaOH, urea, mannitol, and methane in solvents like water, xylene, chloroform to calculate related chemical properties.
#17 Key
This document provides sample chemistry problems and questions related to topics like:
- Writing balanced equations for neutralization reactions
- Defining terms like oxidation, reduction, concentration, and indicators
- Determining oxidation states of elements in compounds
- Identifying redox, precipitation, and acid-base reactions
- Performing calculations involving molarity, moles, and concentration
The problems cover a wide range of general chemistry concepts.
#13 Key
This document provides sample problems and questions for a general chemistry exam. It includes sample balanced equations for neutralization reactions and definitions of key terms like oxidation, reduction, concentration, and indicators. It also asks students to determine oxidation states, identify redox reactions, calculate molarity and amounts of substances in solutions, and determine concentrations of ions after mixing solutions.
#17
The document contains questions about chemistry concepts including:
1) Writing balanced molecular and net ionic equations for neutralization reactions.
2) Defining oxidation, reduction, concentration, molarity, and indicators.
3) Calculating molarity, moles, and volumes for various chemistry problems involving solutions.
#13
The document contains questions about chemistry concepts including:
1) Writing balanced molecular and net ionic equations for neutralization reactions between acids and bases.
2) Defining oxidation, reduction, concentration, molarity, and indicators.
3) Asking if oxidation can occur without accompanying reduction.
4) Calculating oxidation numbers of elements in compounds.
5) Identifying redox, precipitation, and acid-base reactions based on balanced equations.
6) Calculating molarity, moles of solute, and volumes of solutions.
Guided Practice - 8.3.pptx
This document provides a guided practice on calculating pH and related concentrations. It defines pH and asks the learner to calculate: (1) pH changes when an acid is diluted; (2) pH and hydrogen ion concentration for various acids and bases; (3) pH and hydroxide ion concentration using the water ion product constant; and (4) concentrations of acids and bases given their pH. The practice aims to help the learner understand and apply calculations involving pH and concentration.
#19
This document contains 10 chemistry problems involving calculations of molarity, moles, and mass in solutions. It asks the learner to calculate the grams of solute in a given volume of a solution, the molarity of a solution made by dissolving a mass of solute, the volume of a solution containing a given mass of solute, which of several solutions contains the highest concentration of a particular ion, which of two solutions contains the greater number of moles of an ion, the concentrations of individual ions or molecules in various solutions, the mass of one substance needed to precipitate another from a solution, the volume of one acid needed to neutralize a base solution, the volume of acid needed to neutralize a mass of
MATERI HIDROLISIS GARAM KIMIA XI IPA
Worksheet ini berisi teori hidrolisis garam, cara penurunan rumus hidrolisis dan latihan soal.
silahkan dipergunakan.
Comparison of the acidity of fruit juices
This document describes an experiment that compares the acidity of two fruit juices by determining the concentration of citric acid in each using titration. Sodium hydroxide solutions were standardized and used to titrate samples of each fruit juice along with an indicator. The molarity of citric acid was calculated for each using the titration data. The results showed that fruit juice 2 (Plus) had a higher average molarity of citric acid (0.0138 mol/L) than fruit juice 1 (Zest-O) (0.00721 mol/L), indicating it has a higher acidity.
Dpp 01 ionic_equilibrium_jh_sir-4169
1. This document contains two practice problem sets (DPP No. 48 and 49) on physical chemistry topics related to acids and bases, including:
2. Calculating pH, concentrations of ions, and degree of dissociation for solutions of weak acids and bases.
3. Questions involve acids like acetic acid, formic acid, hydrofluoric acid and bases like ammonia and calculating equilibrium constants.
4. The answer key provides the solutions to the questions in the two problem sets. Questions involve calculations for various acid/base equilibria, salt hydrolysis, and other equilibrium chemistry concepts.
#19 key
1. 18.9 grams of K2Cr2O7 are present in 50.0 mL of 0.360 M K2Cr2O7 solution.
2. The molarity of the (NH4)2SO4 solution formed from dissolving 4.28 grams of (NH4)2SO4 in 300 mL of water is 0.108 M.
3. 58.7 mL of 0.240M CuSO4 solution contains 2.25 grams of CuSO4 solute.
12 chemistry impq_ch02_solutions_01
This document contains chemistry questions related to solutions. It includes questions about types of solutions, properties of solutions like boiling point elevation and freezing point depression, and calculations involving molarity, molality, and vapor pressure. The questions cover topics like ideal and non-ideal solutions, Raoult's law, colligative properties, and van't Hoff factor.
Exp 2 ac
This document describes an experiment to determine the percentage of ethanoic acid in a vinegar sample. Vinegar is made from the oxidation of ethanol and contains acetic acid as its main component. The experiment involves titrating a vinegar sample with a standardized NaOH solution using phenolphthalein as an indicator. Multiple titrations are performed and the data is used to calculate the molarity and concentration of acetic acid in the original vinegar sample. The percentage of acetic acid is determined to be 3.63% w/v.
Quantitative analysis and volumetric analysis
This document provides information on quantitative analysis and volumetric analysis techniques. It defines key terms like concentration, molarity, and standard solutions. It describes common volumetric apparatus and how to perform acid-base titrations using appropriate indicators. It also covers concepts like molar ratios, dilution calculations, and determining water of crystallization through titration reactions. The document provides examples of calculations for molarity, concentration, purity, and molar mass determinations.
Alcohols and Organic Acid
This document contains an organic chemistry homework assignment on alcohols and organic acids. It includes structured and free response questions testing knowledge of properties and reactions of alcohols, carboxylic acids, and their derivatives. Key concepts covered include physical properties of alcohols, combustion reactions, acid-base reactions of carboxylic acids, and organic synthesis reactions such as fermentation.
Structure of Matter seminar problems
1. The document discusses moles, molar mass, molarity, and provides example calculations involving these concepts. Molarity is defined as the number of moles of solute per liter of solution.
2. The document then provides 21 practice problems calculating things like the number of moles or grams of various substances, the molarity of different solutions, and multi-step dilution problems.
3. Students are asked to use the concepts of moles, molar mass, and molarity to solve quantitative chemistry problems involving substances in solutions.
10redox jntu pharmacy
Redox titrations involve adjusting the oxidation state of the analyte using an auxiliary oxidizing or reducing agent so that it can be titrated. Common reagents used in redox titrations include potassium permanganate, sodium thiosulfate, cerium sulfate, and potassium dichromate. Redox titrations are used to determine various analytes like ascorbic acid, hydrogen peroxide, iron, and calcium compounds. The document discusses the principles and procedures of important redox titrations like permanganometry, iodimetry, cerimetry, and dichrometry. It also describes the determination of water using the Karl Fischer reagent and reaction.
Chapter 7 acid & bases part 4
The document discusses neutralization reactions and acid-base titrations. It explains that neutralization is a reaction between acids and bases that produces salts and water. It provides examples of neutralization equations. It also describes acid-base titrations as a quantitative analysis involving gradually adding an acid or base from a burette to determine the endpoint, or point at which the indicator changes color. The document provides practice problems involving using molarity, volumes, and balanced equations to calculate concentrations or volumes in neutralization reactions.
Estimation of water of crystallization in mohr’s salt by titrating with stand...
The document describes an experiment to determine the water of crystallization in Mohr's salt, (NH4)2Fe(SO4)2.XH2O, by titrating a solution of the salt with standardized potassium manganate(VII). The experiment involves standardizing the KMnO4 solution using sodium oxalate, then titrating samples of Mohr's salt solution and calculating the iron content. Based on comparing the experimental iron percentage to theoretical percentages for different values of X, the water of crystallization is determined to be 6 moles, giving the formula (NH4)2Fe(SO4)2.6H2O.
Recitation before exam-student
1. This document contains notes from a chemistry TA for a 5.111 class in the fall of 2012. It provides information about an upcoming test, including that the professor writing it is Prof. Klibanov and students should study past problem sets. It also includes 6 practice problems for students to work through related to acid-base chemistry, thermodynamics, and colligative properties.
2. The practice problems cover calculating pH and pKa values of acids, estimating standard enthalpies and entropies of vaporization, predicting changes in entropy, calculating vapor pressures, and using freezing point depression to determine molar masses of solutes in different solvents.
3. Students are advised to practice these types
Similar to SI #11 (20)
Estimation of water of crystallization in mohr’s salt by titrating with stand...
Estimation of water of crystallization in mohr’s salt by titrating with stand...
More from jessieo387_1412
#27
This document contains questions about oxidation-reduction reactions and voltaic cells. It asks the student to identify oxidizing and reducing agents, write half reactions, identify anodes and cathodes, and determine the direction of electron and ion flow. It also contains questions about standard cell potentials, units of electrical potential, and a half reaction for a hydrogen electrode.
#26 Key
1. The document provides steps to convert between solubility in grams per liter, molar solubility in mol/L, molar concentrations of ions, and Ksp.
2. It gives the definitions of a reducing agent, oxidizing agent, and half-reaction. A reducing agent causes reduction, an oxidizing agent causes oxidation. Half-reactions involve electrons.
3. An anode is where oxidation occurs and a cathode is where reduction occurs in a voltaic cell. Electrons flow from the anode through the external circuit to the cathode.
#25 Key
1. The common ion effect decreases the ionization of a weak electrolyte when a strong electrolyte with a common ion is added to the solution.
2. Buffer capacity refers to how much acid or base can be neutralized before the pH begins to change significantly.
3. A buffer solution contains a weak acid or base and its salt. It has the ability to resist changes in pH.
4. The pH range of a buffer depends on the acid's Ka value and the relative concentrations of the acid and base in the buffer solution. It is the range over which the buffer acts effectively.
#24 Key
This document provides examples of calculating the pH of various strong acid solutions, including nitric acid, perchloric acid, hydrochloric acid, a mixture of hydrochloric acid and hydroiodic acid, and a solution of bromoacetic acid that is partially ionized. It also asks questions about weak acids, Lewis acids, and which compounds form more acidic solutions based on cation properties.
#20 Key
The document provides information about acid-base chemistry including:
1) Calculating the concentration of H+ ions and determining if solutions are acidic or basic based on the relative concentrations of H+ and OH- ions.
2) Defining pH as the negative logarithm of the H+ ion concentration and calculating pH values from given [H+] values.
3) Relating pH and pOH through the equation pH + pOH = 14.
4) Listing the 7 strong acids and their formulas as well as the 7 strong bases and their formulas.
#20
The document provides a chemistry problem set involving calculations of hydrogen ion (H+) and hydroxide ion (OH-) concentrations in solution, definitions and calculations of pH and pOH, and properties of strong acids, weak acids, and weak bases. It asks students to calculate pH and concentrations of H+ given OH- concentrations and vice versa. It also asks students to list strong acids and bases, properties of strong and weak acids, what weak acids and bases have in common, and why HCl is a strong acid but weak base.
#19 Key
This document discusses Bronsted-Lowry acid-base chemistry. It defines Bronsted-Lowry acids as proton donors and bases as proton acceptors. It explains that conjugate acids are formed by adding a proton to a base and conjugate bases are formed by removing a proton from an acid. Several examples of conjugate acid-base pairs are given. The document also states that the stronger the acid, the weaker its conjugate base, and the stronger the base, the weaker its conjugate acid. It describes how the position of equilibrium favors transfer of a proton to the stronger base. Finally, it provides the autoionization reaction of water and defines the ion product constant, Kw, for water.
#18 Key
The document contains 6 chemistry problems involving gas phase chemical equilibria calculations:
1) Calculating the equilibrium partial pressure of N2O4 and the equilibrium constant Kp for the reaction N2O4 ⇌ 2NO2.
2) Calculating the equilibrium concentrations of H2, Br2, and HBr and the equilibrium constant Kc for the reaction H2 + Br2 ⇌ 2HBr.
3) Calculating the equilibrium constant Kc for the reaction SO2 + Cl2 ⇌ SO2Cl2 given the value of Kp.
4) Calculating the value of Kp for the reverse reaction of 2NO2 ⇌
#18
This document contains 6 chemistry problems involving gas phase chemical equilibria. Problem 1 involves calculating the equilibrium partial pressure and equilibrium constant for the reaction N2O4(g) ⇌ 2NO2(g). Problem 2 involves calculating equilibrium concentrations and the equilibrium constant for the reaction H2(g) + Br2(g) ⇌ 2HBr(g). Problem 3 asks to calculate the equilibrium constant for the reaction SO2(g) + Cl2(g) ⇌ SO2Cl2(g) given the value of Kp at a specific temperature.
#17 Key
1. The document contains 7 chemistry problems involving calculation of equilibrium constants (Keq and Kc) for various chemical reactions.
2. Problem 3 calculates Keq as 1.84x10-2 for the decomposition of HI gas into H2 and I2 gases at 425C, given the partial pressures of reactants and products at equilibrium.
3. Problem 7 involves a multiple step chemical equilibrium problem, calculating the initial and equilibrium partial pressures and concentrations of gases in a reaction between CO2, H2 and H2O, and determining the equilibrium constant Kp.
SI #16 Key
The document contains a chemistry exam with multiple choice questions about reaction rates and stoichiometry. Question 1 asks about the relationship between the rates of disappearance of H2 and appearance of HF in the reaction H2 + F2 → 2HF. Question 2 asks about the relationship between the average rate of appearance of product B and disappearance of reactant A in the reaction 3A → 2B. Question 3 asks about the order of reactants and overall order of the reaction for the hydrolysis of t-butyliodide.
SI #16
The document contains a chemistry practice problem set with 10 multiple choice questions about reaction rates and rate laws. The questions cover topics such as how the rates of reactants and products are related in a chemical reaction, how to write rate laws from reaction equations, determining reaction orders from rate equations, and calculating rate constants. It also includes a nomenclature list of 38 chemical species.
Practice Test 3
1. The document contains a practice test with multiple choice questions about chemical kinetics and equilibrium.
2. Questions cover topics like reaction rates, rate laws, reaction orders, equilibrium constants, Le Chatelier's principle, and the Haber process.
3. There is also a bonus section with chemical nomenclature questions matching names to formulas.
SI #13 Key
This document contains information about several chemistry concepts and example calculations:
1) It provides calculations to determine the amount of N2O5 remaining and reaction time for its decomposition reaction at 70°C.
2) It discusses how reaction rates change with changes in reactant concentrations for a reaction following a rate law.
3) It gives the rate law and calculates rates for the decomposition of N2O5 in carbon tetrachloride.
4) It provides the rate law and calculates rates for a reaction that is 1st order in H2 and 2nd order in NO.
5) It states that the law of mass action expresses the relationship between reactant and product concentrations at equilibrium.
Si #12 Key
1. Chemical kinetics is the study of time vs. the rate of chemical change. The three factors that affect chemical reactions are concentration, temperature, and catalysts.
2. Instantaneous rate is the slope of a line drawn tangent to the concentration-time curve at a specific time. Beer's Law states that absorption of electromagnetic radiation by a substance is directly proportional to its concentration.
3. A first-order reaction has a rate proportional to the concentration of a single reactant raised to the first power. The rate is equal to k[A] and a plot of ln[A] versus time gives a straight line with a slope of -k.
SI #12
Chemical kinetics describes the rates of chemical reactions. The three factors that affect reaction rates are concentration of reactants, temperature, and presence of a catalyst. An instantaneous rate is the rate of reaction at a specific moment in time. Beer's law relates the absorption of light to the concentration of an absorbing substance in a solution. First and second order reactions have rates dependent on the first or second power of the concentration of a reactant. Half-life is the time required for half of the reactants to be converted to products at a given reaction rate. Activation energy is the minimum energy that reactant molecules must possess for a reaction to occur.
#9 Key
London dispersion forces are the attractive force between two molecules with hydrogen bonded to the oxygen atom. CH4 has dispersion forces as its only intermolecular force. Adsorption is the process of a substance sticking to the surface of another. Surface tension is the energy required to expand the surface area of a liquid by a unit amount of area. The vapor pressure of any substance at its normal boiling point is 1 atm. The concentration of nitrate ion in a solution containing 0.900 M aluminum nitrate is 2.70 M. Sublimination is the direct conversion of a solid to a gas.
#8 Key
1. Ionic bonding involves the complete transfer of an electron from one element to another.
2. Covalent bonds have equally shared pairs of electrons between atoms.
3. Polar covalent bonds are defined as occurring when one atom exerts a greater attraction for the bonding electrons.
More from jessieo387_1412 (18)
SI #11
- 1. GENERAL CHEMISTRY-II (1412) S.I. # 11 1. Calculate the molarity of the following aqueous solutions. a. 0.540 g Mg(NO3)2 in 250.00 mL of solution b. 22.4 g LiClO4 x 3H2O in 175 mL of solution c. 25.0 mL 3.50 M HNO3 diluted to 0.250 L. 2. Commercial aqueous nitric acid has a density of 1.42 g/mL and is 16 M. Calculate the percent HNO3 by mass in the solution. 3. What is the osmotic pressure of solution formed by dissolving 44.2 mg of aspirin (C9H8O4) in 0.358 L of water 25°C.
- 2. 4. List the following aqueous solutions in order of increasing boiling point: 0.120 M glucose 0.050 M LiBr 0.050 M Zn(NO3)2 5. Define and describe hydrophobic and hydrophilic aqueous colloids: 6. Indicate whether the following is a hydrophilic or hydrophobic colloid: a. butter fat in homogenized milk - b. hemoglobin in blood - c. vegetable oil in salad dressing - d. colloid gold particles in water - NOMENCLATURE!! 1. Benzene 2. Methanol 3. Hexane 4. Cyclohexane 5. Acetic Acid 6. C7H8 7. CH3CH2Cl 8. C7H16 9. C3H8O2 10. C9H8O4