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Acids & Bases: more books (100)

Water, Electrolyte, and Acid-Base Balance;: Normal and Pathologic Physiology as a Basis for Therapy by M. D. Harry F Weisberg, 1953
Acid-Base Balance by Alan Y. Cohen, 1989-01-15
Acid and Basics: A Guide to Understanding Acidbase Disorders by Jerome Lowenstein, 1993-01-15
The Regulation of Acid-Base Balance by Donald W. Seldin, 1989-01
Fluid, Electrolyte, and Acid-Base Balance: A Case Study Approach (Fluid, Electrolyte, & Acid-Base Balance) by Mima M. Horne, Ursula Easterday Heitz, 1991-01
Acid-base regulation; its physiology and pathophysiology [by] Edward J. Masoro [and] Paul D. Siegel by Edward J. Paul D. Siegel Masoro, 1971-01-01
Acids, Bases and the Chemistry of the Covalent Bond (Selected Topics in Modern Chemistry) by C.A. Vanderwerf, 1965-03
Acid-Base Regulation: The Pathophysiology of Acid-Base Balance by Jack L. Keyes, 2002-01-01
Fluid, Electrolyte and Acid-Base Disorders
Acids and Bases: Their Quantitative Behaviour (Science Paperbacks) by Ronald Percy Bell, 1971-09-30
Acid-base and Potassium Homeostasis (Contemporary issues in nephrology)
Body Fluids and the Acid-base Balance by Halvor Christensen, 1965-01-01
Blood Gases and Acid-Base Physiology by Norman L. Jones, 1987-04
Equilibrium: Acids and Bases Bk. II (ILPAC Physical)

lists with details

Acids Bases Salts
acids, bases, and Salts. This page leads you to different areas of interest.
http://www.sciencebyjones.com/acids_bases_salts.htm

Extractions: Acids, Bases, and Salts This page leads you to different areas of interest. Acids Definitions pH math Bases ... Quiz Acids In everyday life we deal with many compounds that chemists classify as acids. For example, orange juice and grapefruit juice contain citric acid. These juices, and others, also contain ascorbic acid, a substance more commonly known as Vitamin C. Salads are often flavored with vinegar, which contains dilute acetic acid. Boric acid is a substance that is sometimes used to wash the eyes. In any chemistry laboratory, we find acids such as hydrochloric acid, sulfuric acid, and nitric acid. These acids are called mineral acids because they can be prepared from naturally occurring compounds called minerals. Mineral acids are generally stronger than household acids, and should be handled with great care because they can burn skin and clothing. Properties of Acids: Acids taste sour . Citric acid is responsible for the sour taste of lemons, limes, grapefruits, and oranges. Acetic acid is responsible for the sour taste of vinegar. Acids turn litmus (or indicator papers) red.
Acids And Bases
acids and bases. Despite its shortcomings the theory is widely used to calculateequilibrium data for weak electrolytes, including acids and bases, in water.
http://www.tannerm.com/acidbase.htm

Extractions: Acids and bases The Arrhenius dissociation model The Arrhenius theory defines acids and bases as isolated species in solution giving rise respectively to hydrogen ions H and hydroxyl ions OH . Interaction with solvents is ignored. The theory cannot begin to explain acidic and alkaline properties in non-aqueous solvents. Despite its shortcomings the theory is widely used to calculate equilibrium data for weak electrolytes, including acids and bases, in water. For a generalized binary weak electrolyte MX (e.g., HCl) at concentration C, a fraction a ionizes. There will be an equilibrium mixture of (1-a)C of MX and aC of both M and X . The equilibrium for the dissociation process MX = M + X is given by K = ( [M ] [X ] ) / [MX] = a C / (1- a If a a C. This is called the Ostwald Dilution Law. The Bronsted-Lowry concept of acids and bases Acids are defined as proton donors and bases as proton acceptors regardless of whether the species are are ionic or neutral. In general acid = base + proton Specific examples are H SO = HSO + H HSO = SO + H H O = H O + H OH = O + H The species on the right, along with the proton is known as the conjugate base. Conjugate acids are defined in a similar way. In aqueous solution the concept includes solvent interaction.
Identifying Acids And Bases
Identifying acidbase species. Being able to readily identify a specieswith regards to a acid/base behavior is a very useful skill.
http://www.psigate.ac.uk/newsite/reference/chemlecs/acidorbase.html
Chemical Sciences Ionization Constants Of Acids And Bases
acids and bases Ionization Constants of acids and bases. The ionization constantsof acids and bases other than water are dealt with in a similar way.
http://www.psigate.ac.uk/newsite/reference/plambeck/chem1/p01133.htm
Learn.co.za : Chemistry
Characteristics of acids and bases. Note Solutions indicators. acidsand bases react to neutralise each other. Points to remember !
http://www.learn.co.za/content/grade12/Science/chem_acidsbases/bass/Unit1/

Extractions: You are here: Classroom Grade 12 Science Chemistry : Acids and Bases ... Acids and Bases : 1. Characteristics of Acids and Bases Other units in this lesson: 2. Acid/Base models 3. Conjugate Acid/Base pairs 4. Acid/Base terminology 5. pH scale and calculations ... 9. Hydrolysis Characteristics of acids and bases
Acids And Bases
http://www.harcourtschool.com/activity/acids/
Chem - Topic 9 - Acids And Bases
Topic 9 acids and bases. 9.1 Properties of acids and bases. Examples ofbases NaOH, NH 3 , CH 3 COO - . 9.2 Bronsted-Lowry acids and bases.
http://homepage.mac.com/stray/ib/chem/SSC/topic9.html

Extractions: Topic 9 - Acids and Bases 9.1 Properties of acids and bases 9.1.1 : Properties of acids and bases in aqueous solutions on stuff...nb...the term alkali refers to a base dissolved in water. Indicators...they change color depending on whether they're in acidic or basic conditions...each one's different, so I suppose I'd better list some common ones... Methyl orange Bromophenol blue Methyl red Bromothymol blue Phenolphtalein Acid red yellow red yellow colorless Base yellow blue yellow blue red Each one change color as a different pH, and so there will be cases where one is useful and others are not. (not really necessary is SL?) O + NaCl. + H Acids with carbonates...will produce water and CO ie 2HCl + CaCO + H O + CaCl 9.1.2 : Experimental properties of acids and bases...when acids and bases neutralize, the reaction is noticeably exothermic (ie heat can be felt coming from the reaction). Obviously, they will have an effect on the color of indicators as described above. The hydrogen produced in the reaction of acids with metal will produce a 'pop' sound if a match is held to it, and the CO from the carbonate reaction will turn limewater a milky white when bubbled trough it.
Laboratory - PH Of Acids And Bases :pKa And PKb Values
Here you can select the acids and bases on their pKa values. There s also ashort explanation about pH calculations. acids and bases pKa and pKb.
http://home.planet.nl/~skok/techniques/laboratory/pka_pkb.html

Extractions: When the concentrations of the salt and acid are equal, the pH of the system equals the pKa of the acid. The percentage ionisation from a given pKa value can be calculated at Reall Make your choice: Table of pKa values for acids or Table of pKb values for bases . Click here for the abbreviations used in the tables. You can always return to this index by mouse-double click. Acids T(°C) pKa Acetic acid ACES ADA Benzoic acid Bicine BIS-TRIS Propane o-Boric acid (1) o-Boric acid (2) o-Boric acid (3) Carbonic acid (1) Carbonic acid (2) CAPS CHES Citrate (1) Citrate (2) Citrate (3) Acids T(°C) pKa Diethylmalonic acid Formic acid Glycylglycine HEPES HEPPS Imidazole MES MOPS PIPES
The Basics Of Acids And Bases
The Basics of acids and bases acids and bases play a key role in the chemistry thataffects your daily life. Many manufacturing processes use acids and bases.
http://www.scs.k12.tn.us/STT99_WQ/STT99/Bolton_HS/tippette/WEBQUEST/WQUEST.HTM

Extractions: The Process To do this project, you will first need to assemble into groups of 3. This project can basically (ha-ha) be broken down into 4 assignments: Assignment 1 In this assignment, your group will construct a visual poster presentation that compares the properties of acids and bases. In addition, you will construct a visual presentation that compares three models of acids and bases: Arrhenius, Bronsted -Lowry, and Lewis. You should be extremely thorough and as detailed as possible. Be as creative as you can, gathering materials from the Internet and outside journal sources . Be prepared to present your findings to the rest of the class. As a group, you may divide up the assignment responsibilities as you decide. Also
Acids And Bases Quiz 2 - PH, Litmus
pH, Litmus Grade 6 quiz - Covers pH, Boyle s law, litmus color changesfor acids and bases, etc 1001 acids and bases Quiz 2.
http://www.1001-periodic-table-quiz-questions.com/quiz/k-12/acids_and_bases_2.ht
Polyprotic, Arrhenius - Acids And Bases Quiz 4 -
polyprotic, Arrhenius Grade 6 quiz - Covers polyprotic, Arrhenius, litmuscolor changes for acids and bases, etc acids and bases Quiz 4.
http://www.1001-periodic-table-quiz-questions.com/quiz/k-12/acids_and_bases_4.ht
Acids And Bases
1. 2. 3. 4. 5, acids and bases. Introduction. The fact that acids and bases havedifferent strength is explained as a result of a different degree of dissociation.
http://utenti.lycos.it/Pasquale_Petrilli/ionicequ/electrol.htm

Extractions: Acids and bases Introduction The classification of substances as acids was at first suggested by their sour taste (Latin acidus = sour; acetum = vinegar). Alkalis (Arabic al kali = ashes of a plant) were taken as those substances that could reverse or neutralize the action of acids. It was also believed that oxygen is a necessary constituent of acids (Greek oxus = sour; gennae = I produce). After Davy, that in 1810 demonstrated that hydrochloric acid contained only hydrogen and chlorine, hydrogen was taken as an essential constituent of acids. According to Arrhenius theory , the proton (H ) is responsible for acidic properties while the hydroxyl ion (OH ) is responsible for basic (alkaline) properties. Acids are thought as compounds which dissociate giving a proton (and its counter ion) such as: HCl = H + Cl CH COOH = H + CH COO Bases are thought as compounds which dissociate giving an hydroxyl ion (and its counter ion) such as: NaOH = Na + OH The fact that acids and bases have different strength is explained as a result of a different degree of dissociation. Thus HCl which is a strong electrolyte (fully dissociated) is a strong acid and acetic acid (a weak electrolyte, i.e., partially dissociated) is a weak acid. However, The following considerations, led in 1923 to a more general concept of acids and bases (Lowry-Bronsted theory): There are many evidences indicating that proton does not exist free in aqueous solution but it is bound to water (hydrated). Normally this hydrated proton is indicated as H
Acids And Bases
acids and bases. Weak acids and bases only partially dissociate to form some ionsand there is still some of the original acid or base present in solution.
http://wwwchem.csustan.edu/chem3070/3070M07.HTM

Extractions: ACIDS donate protons to water to form hydronium ions taste sour turn cabbage juice red turn litmus paper red donate hydroxyl groups accept protons taste bitter feel slimey turn cabbage juice yellow, green or blue depending upon the solution concentration turn litmus paper blue The concentration of hydrogen ions is measured on a logrithmic scale: pH = - log [H O Table 1 shows the correlation between hydrogen ion concentration and pH. A solution with a low pH is acidic, and a solution with a high pH is basic. Solutions at a pH of 7 are neutral. fill a blender with pieces of red (purple) cabbage add water blend to smithereens filter cabbage juice using a coffee filter The juice can be used to make a rainbow of colors corresponding to various (approximate) pH values. Strong acids and bases completely dissociate to form ionic species. There is none of the original acid or base left in solution. Weak acids and bases only partially dissociate to form some ions and there is still some of the original acid or base present in solution. For example, a .1M solution of HCl has a pH of 1, because all of the HCl reacts with water to form H O ions. Therefore all the moles that were once HCl are now H
Bronsted-Lowry Acids And Bases
next up previous Next Lewis acids and bases Up Some classifications of acidsPrevious Arrhenius acids and bases BronstedLowry acids and bases.
http://www.nyu.edu/classes/tuckerman/honors.chem/lectures/lecture_21/node3.html

Extractions: Next: Lewis acids and bases Up: Some classifications of acids Previous: Arrhenius acids and bases The Bronsted-Lowry definition is named for Johannes Bronsted and Thomas Lowry, who independently proposed it in 1923. A Bronsted-Lowry (BL) acid is defined as any substance that can donate a hydrogen ion (proton) and a Bronsted-Lowry base is any substance that can accept a hydrogen ion (proton). Thus, according to the BL definition, acids and bases must come in what is called conjugate pairs . For example, consider acetic acid dissolved in water:
Acids And Bases
acids and bases. Introduction and Definitions acids and bases are encounteredfrequently both in chemistry and in everyday living.
http://www.elmhurst.edu/~chm/vchembook/180acidsbases.html

Extractions: Acids and Bases Elmhurst College Acids Acid-Base Strength ... Virtual ChemBook Acids and Bases Introduction and Definitions: Acids and bases are encountered frequently both in chemistry and in everyday living. They have opposite properties and have the ability to cancel or neutralize each other. Acids and bases are carefully regulated in the body by the lungs, blood, and kidneys through equilibrium processes. What are acids and bases? Observational definitions: Acids: Bases: Taste sour. Taste bitter. Give sharp stinging pain in a cut or wound. Feels slippery Turn blue litmus paper red. Turn red litmus paper blue. Turn phenolphthalein colorless. Turn phenolphthalein pink. React with metals to produce hydrogen gas. React with carbonates or bicarbonates to produce carbon dioxide gas. See the graphic on the left as a base is wiped over the paper which already has the indicator phenolphthalein on it. The drawing changes to pink. What are Acids and Bases - on a molecular level?
Acids, Bases And Indicators
acids and bases are two different types of chemicals that have interestingproperties. acids, bases and Indicators. acids and bases
http://www.kidscastle.si.edu/channels/science/articles/sciencearticle3.html

Extractions: Acids, Bases and Indicators Acids and bases are two different types of chemicals that have interesting properties. You can do experiments with some of the common acids and bases, and you can even use some of these experiments in a magic show. Many acids and bases are corrosive; that is, they can dissolve or eat away substances by chemical action. For example, you can often see what looks like a white fungus around the wires of a car battery. This is corrosion caused by the extremely strong acid inside the battery. So you will have to be careful to use only the weak acids and bases described in these experiments. For your experiments you will need an indicator, a chemical that changes color when it is mixed with certain other chemicals such as acids and bases. Ordinary tea is a good indicator. Make a cup of very dark tea, then squeeze fresh lemon juice into the tea as you stir it. Notice that the tea becomes lighter and lighter in color. This is caused by adding an acid. In this case it is citric acid, which causes the sour taste in the lemon. Red cabbage is another very good indicator. You will also need several glasses, white vinegar (a weak acid), limewater (a weak base you can buy at the drugstore), a straw, and a pot for boiling some red cabbage leaves.
Chem1 Acids And Bases
Chem1 acids and bases. If you teach base reactions; Recognizing commonacids and bases; Reactions of acids and bases; salts; The pH scale; Acid
http://www.chem1.com/lessondesc/CB14.html
Dissociation Constants Of Organic Acids And Bases
Dissociation Constants Of Organic acids And bases, This table liststhe acidbase dissociation constants of over 600 organic compounds
http://www.zirchrom.com/organic.htm

Extractions: Dissociation Constants Of Organic Acids And Bases This table lists the acid-base dissociation constants of over 600 organic compounds, including many amino acids. All data apply to dilute aqueous solutions and are presented in the form of pK a , which is the negative of the logarithm of the acid dissociation constant K a Molecular formula Name Step T I °C pK a CH O Formic acid CH N O Urea CH N Methylamine C HCl O Trichloroacetic acid C H Cl O Dichloroacetic acid C H O Glyoxylic C H O Oxalic acid C H BrO Bromoacetic acid C H ClO Chloroacetic acid C H IO Iodoacetic acid C H OS Thioacetic acid C H O Acetic acid C H O Glycolic acid C H N Ethyleneimine C H NO Acetamide C H NO Glycine C H O Ethylene glycol C H AsO Cacodylic acid C H N Dimethylamine C H N Ethylamine C H NO Ethanolamine C H NO S Taurine C H NS Cysteamine C H N 1,2-Ethanediamine C H NO Cyanoacetic acid C H NS Thiazole C H N 1H-Imidazole C H N S 2-Thiazolamine C H O Acrylic acid C H O Pyruvic acid C H O Malonic acid C H ClO 2-Chloropropanoic acid C H ClO 3-Chloropropanoic acid C H N Melamine C H O Propanoic acid C H O 3-Hydroxypropanoic acid C H O Lactic acid C H O Glyceric acid C H N Azetidine C H NO L -Alanine C H NO b -Alanine C H NO Methylglycine C H NO S Cysteine C H NO Serine C H NO S l -Cysteic acid C H N O Glycocyamine C H O Glycerol C H N Propylamine C H N Trimethylamine C H NO 1-Amino-2-methoxyethane C H NO Trimethylamine oxide C H N 1,2-Propanediamine
Conductivity Of Acids And Bases
DoChem 104 Conductivity of acids and bases. An LED device or a meter deviceis used to study the conductivity of solutions of acids and bases.
http://129.93.84.115/Chemistry/DoChem/DoChem104.html

Extractions: Set Free electrons (as in a metal), free ions, or some other mobile charge carrier must be available to sustain an electric current. A solution that contains ions will conduct electricity. The amount of electricity that will flow through a solution depends primarily on the numbers of ions present: the greater the number of ions, the greater the amount of electricity which will flow. This can be observed by using a conductivity apparatus. The amount of electricity flowing is indicated by the brightness of the light bulb, the LED, or the meter reading. A strong electrolyte ionizes to a large degree. When a strong electrolyte is also soluble, its solutions contain many ions, conduct electricity well, and cause the lamps in a conductivity apparatus to burn brightly. A weak electrolyte dissociates only slightly in solution, forms fewer ions, and causes the light bulb to glow dimly. A nonelectrolyte has very few ions, and the light bulb will not glow. In this experiment the conductivity apparatus allows us to distinguish between strong and weak acids or bases. Acids and bases react to form salts and water. Salts are nearly always strong electrolytes.
Standardization Of Acids And Bases
Return to DoChem Index EXPT DoChem 102 Standardization of acids and bases. DoChem102 Standardization of acids and bases. Titration Skills Checklist.
http://129.93.84.115/Chemistry/DoChem/DoChem102.html

Extractions: Set An acid solution reacts with a base solution in a "neutralization" reaction. The pertinent chemical reactions in this experiment are: O **Visual here. or Figure V102V1 H C O O + Na C O H SO O + Na SO H + OH O The volume of solution required for such a reaction to go to completion may be measured using a buret. A color change in an added chemical indicator signals an end point. It is selected to indicate that neutralization has taken place. This end point may not be the same as the stoichiometric or equivalence point; given an appropriate selection of indicator, the difference in volume between these two points should be negligible. In this experiment, a solid acid is titrated with sodium hydroxide to the faint pink phenolphthalein color. Once the concentration of the NaOH is known, it may be used to calculate the concentration of other acids.

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