81. SOLUTIONS AND SOLUBILITY acids and bases that are strong electrolytes (completely ionized in solution) A strong acid yields a weak conjugate base. Strong bases examples include http://educ.queensu.ca/~science/main/concept/chem/c10/c10cdmo3.htm

82. Acids & Bases: Acids, Bases, & Water - Definitions http://www.mhhe.com/physsci/chemistry/chang7/esp/folder_structure/ac/m1/s1/

83. Bronsted-Lowry Acids And Bases Thus, according to the BL definition, acids and bases must come in what is calledconjugate pairs. For example, consider acetic acid dissolved in water http://www.nyu.edu/classes/tuckerman/honors.chem/lectures/lecture_21/node3.html

Next: Lewis acids and bases Up: Some classifications of acids Previous: Arrhenius acids and bases Bronsted-Lowry 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: Notice that we have written explicitly in these reactions. The reason is that acid/base dissociation occurs by a proton transfer reaction from an acid species to a specific water molecule. The transfer occurs through a hydrogen bond between the acid molecule and a solvating water molecule. Here, CH COOH is a BL acid because it can donate a proton, and CH COO its conjugate base because it can accept a proton. Note that and also form such a conjugate pair.

84. Acids And Bases acids and bases. The Arrhenius dissociation model. The Arrhenius theory definesacids and bases as isolated species in solution giving rise respectively to http://www.tannerm.com/acidbase.htm

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.

85. Chemistry: Acids And Bases When dealing with weak acids and weak bases, you also might have to deal with This is when you add a salt to a weak acid or base which contains one of http://www.shodor.org/unchem/basic/ab/

HOME Course Chapters Calculator Fundamentals Mathematics Review Basic Concepts Chemical Nomenclature (REQUIRED FOR CREDIT!) Atomic Structure Stoichiometry Acid Base Chemistry Advanced Concepts Section Tests Pre-test Post-test Useful Materials Glossary Online Calculators Redox Calculator Kinetics Arrhenius Calculator Thermodynamics Calculator Nuclear Decay Calculator ... Nomenclature Calculator Related Information Links Texas Instruments Calculators Casio Calculators Sharp Calculators Hewlett Packard Calculators ... Contact Webmaster Acid-Base Chemistry Water pH Definitions of acids and bases Salts ... Acid-Base Titrations Water We typically talk about acid-base reactions in aqueous-phase environments that is, in the presence of water. The most fundamental acid-base reaction is the dissociation of water: In this reaction, water breaks apart to form a hydrogen ion (H ) and a hydroxyl ion (OH ). In pure water, we can define a special equilibrium constant (K w ) as follows: Where K w is the equilibrium constant for water (unitless) [H ] is the molar concentration of hydrogen [OH is the molar concentration of hydroxide An equilibrium constant less than one (1) suggests that the reaction prefers to stay on the side of the reactants in this case, water likes to stay as water. Because water hardly

86. Unit Plan For Acids And Bases In this unit students examine the qualitative and quantitative aspects of acidsand bases. They learn how these two classes of compounds ionize or http://www.michigan.gov/scope/0,1607,7-155-13515_13521_13524-36289--,00.html

Skip Navigation Michigan.gov Home Scope Home Site Map ... Contact Us document.form2.SearchCriteria.size=10; Ninth Grade Tenth Grade English Language Arts Mathematics ... [Text Version] Unit Plan for Acids and Bases Curriculum Unit Plan Science Tenth Grade Chemistry Unit 4: Acids and Bases Abstract In this unit students examine the qualitative and quantitative aspects of acids and bases. They learn how these two classes of compounds ionize or dissociate in water. Students learn to determine the degree of acidity or alkalinity of solutions of pH. Three theories are investigated to add to their understanding of the properties of acids and bases. Students also investigate neutralization reactions, i.e., the result of acids combining with bases. They learn titration as a procedure that can be used to find the concentration of an acid or base. Students are asked to examine common household materials and determine if they are acidic or basic in nature. They research common causes of acid rain and conclude their studies by writing about how weather patterns affect the distribution of environmental damage caused by acid rain. Unit Title Acids and Bases Grade Level/Course Title Tenth Grade/Chemistry Focus Questions What distinguishes acids from bases How do we measure the strengths of acids and bases How are acids and bases used in our daily lives Benchmarks Students will: gather and synthesize information about how to identify the properties of acids and bases and how to analyze them (I.1.HS.4

87. Acids And Bases acids and bases, two related classes of chemicals; the members of each class havea number of common properties when dissolved in a solvent, usually water. http://www.factmonster.com/ce6/sci/A0802335.html

Home U.S. People Word Wise ... Homework Center Fact Monster Favorites Hurricane Katrina Ramadan Children Inventors The Doctor's In ... 2006 TFK Almanac Reference Desk Atlas Almanacs Dictionary Encyclopedia ... Encyclopedia acids and bases acids and bases, two related classes of chemicals; the members of each class have a number of common properties when dissolved in a solvent, usually water. Sections in this article: Introduction Properties Classification Acid-Base Theories The Columbia Electronic Encyclopedia, Page Tools: Cite Print See more Encyclopedia articles on: Chemistry: General AD AD AD ADS Business Cards Link to Fact Monster Add Fact Monster search ... Privacy Brought to you by: Information Please

88. Chemistry - Acids & Bases ACID, +, BASE, acids bases, SALT, +, WATER. Hydrochloric Acid, +, Sodium Hydroxide,acids bases, Sodium Chloride, +, Water. HCl, +, NaOH, acids bases http://qldscienceteachers.tripod.com/junior/chem/acid.html

setAdGroup('67.18.104.18'); var cm_role = "live" var cm_host = "tripod.lycos.com" var cm_taxid = "/memberembedded" Search: Lycos Tripod Dukes of Hazzard Share This Page Report Abuse Edit your Site ... Next PROPERTIES OF ACIDS Corrosive ('burns' your skin) Sour taste (e.g. lemons, vinegar) Contains hydrogen ions (H ) when dissolved in water Has a pH less than 7 Turns blue litmus paper to a red colour Reacts with bases to form salt and water Reacts with metals to form hydrogen gas Reacts with carbonates to form carbon dioxide, water and a salt EXAMPLES OF ACIDS Hydrochloric acid (HCl) in gastric juice Sulphuric acid (H SO Nitric acid (HNO Carbonic acid in softdrink (H CO Uric acid in urine Ascorbic acid (Vitamin C) in fruit Citric acid in oranges and lemons Acetic acid in vinegar Tannic acid (in tea and wine) Tartaric acid (in grapes) PROPERTIES OF BASES AND ALKALIS Corrosive ('burns' your skin) Soapy feel Has a pH more than 7 Turns red litmus paper to a blue colour Many alkalis (soluble bases) contain hydroxyl ions (OH Reacts with acids to form salt and water EXAMPLES OF BASES AND ALKALIS Sodium hydroxide (NaOH) or caustic soda Calcium hydroxide ( Ca(OH) ) or limewater Ammonium hydroxide (NH OH) or ammonia water Magnesium hydroxide ( Mg(OH) ) or milk of magnesia Many bleaches, soaps, toothpastes and cleaning agents

89. LHS | ChemMystery | Properties Of Acids, Bases And Neutrals What are some common acids, bases and neutrals? These are some acids you may be You may be wondering what acids and bases do to other chemicals. http://www.lawrencehallofscience.org/ChemMystery/actacidbase.html

Play ChemMystery Make Your Own Acid/Base Indicator See related GEMS teacher's guide Of Cabbages and Chemistry See related School Program Of Cabbages and Chemistry Properties of Acids, Bases and Neutrals Taste: Have you ever taken a bite out of a sour lemon? When you taste something sour, your face kind of looks like this - *. Lemon juice is an acid and acids can taste sour. Baking soda has a bitter taste that most people don't like - *. It is an example of a base and bases can taste bitter. Water is not an acid or a base, it is neutral and has no particular taste. Please don't ever taste strong acids or strong bases or any other chemicals that are not food! Feel: What happens if you're slicing lemons and some juice get into a cut on your finger? YOW! It stings. Acids sting cuts. If you've ever spilled bleach or soap on the floor, you may have noticed that it is slippery. Bases such as bleach and soap are slippery. Our neutral substance, water, would be a good choice for cleaning up acids and bases because it doesn't sting and it's not slippery. Please don't ever touch strong acids or strong bases because they can be harmful to your skin and may damage sensitive tissues such as your eyes. Examples of acids, bases and neutrals

90. 1.2 Acids & Bases A more general definition of acids and bases is the approach of Lewis in 1923 . In reality, most physicians have a basic knowledge of acids and bases http://www.anaesthesiamcq.com/AcidBaseBook/ab1_2.php

Acid-base Physiology Previous Index Next 1.2.1 What is an acid? The term is derived from the Latin word ‘acidus’ which means sour. Early chemists had a list of properties that were common to the substances that they considered to be acids or bases [eg acids had a sour taste, turned litmus red, reacted with some metals to produce a flammable gas (hydrogen) ..etc.. ]. They would assess a new substance as an acid or as a base (or as neither) by comparing the properties of the new substance against the list of properties. The Arrhenius Theory The first modern approach to acid-base chemistry was by Arrhenius in 1887. He defined an acid as a substance which was capable of dissociating in water solution to produce hydrogen ions. This definition identified most of the substances which were considered to be acids at that time. A base was defined as a substance which dissociated in water solution to produce hydroxide ions. The theory was not totally satisfactory for several reasons. For example, some substances which had acidic properties did not contain hydrogen and some bases did not contain hydroxide ions. The theory also applied only to aqueous solutions. The Bronsted-Lowry Theory The next development was the Bronsted-Lowry Theory (1923) and this is the approach which is generally accepted in biological and medical fields. An acid is defined as a substance which donates a hydrogen ion to another substance. This does not require an aqueous solution or dissociation into ions as in the Arrhenius definition. The substance which accepts the H

91. Acids And Bases (Organic Chemistry) - Wikibooks The first and earliest definition of acids and bases was proposed in the 1800 sby Swedish BrønstedLowry acids and bases Proton donors and acceptors http://en.wikibooks.org/wiki/Acids_and_bases

Acids and bases (Organic chemistry) From Wikibooks (Redirected from Acids and bases Foundational concepts Contents Proton donors and acceptors Br¸nsted-Lowry Acids and Bases: Proton donors and acceptors Br¸nsted-Lowry definiton of acid and base Lewis Acids and Bases: Electron donors and acceptors ... edit Proton donors and acceptors The first and earliest definition of acids and bases was proposed in the 1800's by Swedish scientist Svante Arrhenius, who said that an acid was anything that dissolved in water to give up H ions , Such as hydrochloric acid, and a base was anything that dissolved in water to give up OH ions , such as sodium hydroxide. The Br¸nsted-Lowry definiton of 1923 broadened this idea a bit: edit Br¸nsted-Lowry Acids and Bases: Proton donors and acceptors edit Br¸nsted-Lowry definiton of acid and base An acid is any proton donor and a base is any proton acceptor The focus of this definition is on donating and accepting protons, and is not limited to aqueous solution. For example, the hypothetical acid HA will dissasociate into H and A The Br¸nsted-Lowry definiton of acids and bases is one of two definitions we commonly use. The second definition deals not with protons but with electrons, and has a slightly different emphasis.

92. Acids And Bases Neutralize Each Other (General Chemistry) - Wikibooks Notice that this definition limits acids and bases to substances that can The most general definition of acids and bases is the Lewis definition. http://en.wikibooks.org/wiki/Acids_and_bases_neutralize_each_other_(General_Chem

Acids and bases neutralize each other (General Chemistry) From Wikibooks General Chemistry Intro Matter Measurement ... Science bookshelf An acid (from Latin acidus , meaning sour or tart) is a en:chemical compound generally defined by its reactions with complementary chemicals, designated bases (see en:Acid-base reaction theories ). An acid tends to give a proton and can be represented by the generic formula AH. In water, there is the following reaction: There is a distinction between en:weak acids and en:strong acids . For a strong acid, no AH remains in solution: Some of the stronger acids include the hydrohalic acids - HCl, HBr, and HI - and the oxyacids, which tend to contain central atoms in high oxidation states surrounded by oxygen - including HNO H SO HClO Acidity is typically measured using the en:pH scale. Acidic (chemistry), the opposite to basic, reacting with basics to form salts. Acidic (geology), of rock: containing more than 65% of silica. Contents Characteristics Acids are generally: Acids in Food Different Definitions of Acid/Base ... edit Characteristics edit Acids are generally: Taste : sour when dissolved in water Touch : strong acids have a stinging feeling Reactivity : acids react violently with many en:metals Electrical Conductivity : acids are en:electrolytes edit Acids in Food en:citric acid : found in en:citrus fruits en:lactic acid : found in en:dairy products such as en:yoghurt and sour en:milk en:carbonic acid : found in en:carbonated beverages en:acetic acid : found in en:vinegar edit Different Definitions of Acid/Base

93. Acids And Bases Many common fluids are acids or bases, yet they do not harm us. Be advised thateither an acid or a base, if too strong, can cause serious injury. http://www.engineering.usu.edu/jrestate/workshops/acid/acids.php

Last Updated Graduate Credit Workshop Acids and Bases Home Classroom Activity How Acids and Bases are Made Water will naturally "break up" into H and OH in a process known as dissociation When water dissociates the hydrogen atom breaks its bond with oxygen and leaves behind its electron. The hydrogen atom is now positively charged and properly called a hydrogen ion . The remaining hydrogen is still connected to the oxygen, which now has an extra electron, giving this pair a negative charge. The OH molecule is properly called a hydroxide ion . The amount of dissociated water molecules in relation to all the water molecules is very small, and since the overall amounts of H and OH are equal, they cancel each other out. If, for some reason, the H and OH are not balanced, an acid or base is formed. The acidity or alkalinity (baseness) of the solution is rated on the pH scale. The range of this scale is from to 14 with 7 being the neutral point. Numbers below seven are acidic, while numbers above seven are basic. It is important to note that this scale is logarithmic. Thus, a pH of 2 is not twice as acidic as a 4, but rather 100 times as acidic. That same pH of 2 is not three times as acidic as a pH of 6, but rather 10,000 times as acidic. Acids are aqueous solutions that have more H than OH . This can be caused by adding H ions or by taking away OH ions (actually, the process is far more complicated than this, but for what you will need to do this definition will work fine). Acids are characterized by their sour taste and their ability to dissolve metals. Many of the foods you eat, such as oranges, green apples, and rhubarb, taste sour due to the acids which they form. Many cleaners have acids in them. It is important that you read the warning labels on your household cleaners as we do not advise that you use acidic solutions to clean water pipes in your home.

94. CHM 1046 acids and bases that ionize completely in solution are strong electrolytes, Observations about acids and bases. The commonly used acids, hydrochloric, http://wine1.sb.fsu.edu/chm1046/notes/AquaRxns/Acidsetc/Acidsetc.htm

CHM 1046 General Chemistry II Dr. Michael Blaber Aqueous Reactions Acids, Bases and Salts Acids Acids are substances that are able to ionize in aqueous solutions to form H ions (and an associated anion) A Hydrogen atom consists of a single proton and a single electron (no neutron) Thus, an H ion is just a proton Acids are often referred to as " proton donors Different types of acids can ionize to release one or more protons A monoprotic acid releases a single proton when it ionizes (e.g. hydrochloric acid): A diprotic acid can release two protons when it ionizes (e.g. sulfuric acid): For sulfuric acid, the first ionization is complete (as indicated by the single arrow), therefore it is a strong electrolyte However, only some of the molecules of HSO undergo a second ionization. Thus, the deprotonization of HSO , and the protonization of SO are significant reactions (as indicated by the double arrows) Aqueous solutions of sulfuric acid will therefore contain some mixture of protons (H ), HSO and SO ions Bases Bases are substances that react with (or accept) H ions A common example of a base is the hydroxide ion (OH (Note that this represents the formation of a chemical bond between the ions to produce a water molecule) Any substance that increases the concentration of OH (aq) is a base Some of the most common bases are metal hydroxides (e.g. NaOH, KOH, Ca(OH)

95. Lewis In the BronsteadLowry description of acids and bases GNLewis thought aboutacids and bases in terms of donation and acceptance of unshared pairs of http://wine1.sb.fsu.edu/chm1046/notes/AcidBase/Lewis/Lewis.htm

CHM 1046 General Chemistry II Dr. Michael Blaber Acid-Base Equilibria Lewis Acids and Bases Recall the Arrhenius description of acids and bases: An Arrhenius acid reacts in water to release a proton An Arrhenius base reacts in water to release a hydroxide ion In the Bronstead-Lowry description of acids and bases: A B-L acid reacts to donate a proton A B-L base accepts a proton A B-L base, therefore, is a compound with an unshared pair of electrons that can from a bond with a proton: G.N.Lewis thought about acids and bases in terms of donation and acceptance of unshared pairs of electrons A Lewis acid is defined as an electron-pair acceptor A Lewis base is defined as an electron-pair donor In the above example with ammonia, the ammonia is acting as a Lewis base (donates a pair of electrons), and the proton is a Lewis acid (accepts a pair of electrons) The description of an acid and a base by Lewis is consistent with the description by Arrhenius, and with the definition by Bronstead-Lowry. However, the Lewis description, a base is not restricted in donating its electrons to a proton, it can donate them to any molecule that can accept them

96. Title Of Lesson: Acids And Bases Benchmark Lesson The student knows the properties and behavior of acids and bases. acids andbases are an important part of our dayto-day lives. The term acid rain http://www.edb.utexas.edu/insite/iste-test/pbiprojects/Fall2000/GrnChem/content/

Title of lesson: Acids and Bases Benchmark lesson Course title and level: 1 st nd , or 3 rd year Chemistry TEKS addressed: Scientific processes. The student, for at least 40% of instructional time, conducts field and laboratory investigations using safe, environmentally appropriate, and ethical practices. The student is expected to: (A) demonstrate safe practices during field and laboratory investigations; and (B) make wise choices in the use and conservation of resources and the disposal or recycling of materials. (2) Scientific processes. The student uses scientific methods during field and laboratory investigations. The student is expected to: B) collect data and make measurements with precision; (C) express and manipulate chemical quantities using scientific conventions and mathematical procedures such as dimensional analysis, scientific notation, and significant figures; (D) organize, analyze, evaluate, make inferences, and predict trends from data; and (E) communicate valid conclusions. (14) Science concepts. The student knows the properties and behavior of acids and bases. The student is expected to:

97. PASCO Chemistry Experiment - Dec. 2001 acids and bases. Equipment - Equipment Set-up - Software Set-up To increasethe pH of a solution, what substance (acid, base, neutral) must be added http://www.pasco.com/experiments/chemistry/december_2001/home.html

home resources experiments chemistry ... print page Online Chemistry Experiments December 2001, Chemistry Experiment: Acids and Bases Equipment Equipment Set-up Software Set-up Data Collection Procedure ... Conclusions and Extensions Purpose: Equipment: pH Sensor PASPORT (PS-2102) ScienceWorkshop (CI-6507A) Computer Interface PASPORT Xplorer (PS-2000) PASPORT USB Link (PS-2100) ScienceWorkshop 500 (CI-6400) ScienceWorkshop 750 (CI-6450) 10 Test Tubes (small beakers or plastic cups may also be used) and a Test Tube Rack. Wash bottle filled with distilled water and large beaker (or use a sink), to rinse off the pH sensor between measurements. Solutions: Windex, Cola, Lemon Juice, Coffee, Vinegar, Salt Water, Orange Juice, Ammonia, Milk, and Distilled Water. Back to top Equipment Setup: Label each of the 10 test tubes with the names of the various solutions.

98. Welcome To GEMS Alien Juice Bar This activity is based on the acids and Aliens activity from the book Of to explore the properties of acids and bases using red cabbage juice. http://scienceview.berkeley.edu/showcase/flash/juicebar.html

LHS Interactive Activity Showcase See GEMS website Don't see the activity? This activity is based on the "Acids and Aliens" activity from the book Of Cabbages and Chemistry , published by Great Explorations in Math and Science (GEMS) Of Cabbages and Chemistry is an engaging series of science activities for grades 4-8 that enables students to explore the properties of acids and bases using red cabbage juice. LHS Interactive Activity Showcase See GEMS website Lawrence Hall of Science Home Comments, questions, suggestions? Updated Fri, Dec 8, 2000

99. Acids And Bases Lewis Vs. Bronsted acids and bases play vital roles in many organic chemical reactions. This pageexamines two complementary definitions of acids and bases, and explores some http://www.personal.psu.edu/faculty/t/h/the1/acidbase.htm

100. Brønsted BrønstedLowry acids and bases A Brønsted-Lowry acid is defined as anything thatreleases This definition includes all Arrhenius acids and bases but, http://facultyfp.salisbury.edu/dfrieck/htdocs/212/rev/acidbase/Bronst.htm

Brønsted-Lowry Acids and Bases A Brønsted-Lowry acid is defined as anything that releases H ions; a Brønsted-Lowry base is defined as anything that accepts H ions. This definition includes all Arrhenius acids and bases but, as we will soon see, it is a bit more general. The Brønsted-Lowry concept is based on the transfer of a proton from one substance to another. The ionization of HCl in water can be viewed as a Brønsted-Lowry acid-base reaction with HCl behaving as the acid (H ion donor) and water serving as the base (H ion acceptor). Just as we saw with Arrhenius acids, the acidic hydrogens are usually written at the beginning of the chemical formula of a Brønsted-Lowry acid. So, for instance, we can tell from the formulas that HCl, HNO , and HCH O are monoprotic acids, each liberating one H ion per acid molecule, whereas H SO is diprotic, and H PO is triprotic. The reaction of HCl with water can be called either an Arrhenius acid-base reaction or a Brønsted-Lowry acid-base reaction. There are many acid-base reactions, however, for which the Arrhenius definition is inappropriate. Let's consider the gas phase reaction of HCl with ammonia, NH , which occurs as shown in the chemical equation below. The arrows represent the movement of electron pairs as bonds are formed and broken.

A  B  C  D  E  F  G  H  I  J  K  L  M  N  O  P  Q  R  S  T  U  V  W  X  Y  Z

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