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Acid and Base ppt

Acids and bases are effected both chemistry and everyday living. Both of these compounds can easily recognise with their taste. Acids have sour taste, and bases are bitter to the taste. Do you know why an orange or lemon is sour in taste? Have you tasted mustard seeds, what your mom is using for making delicious food? Orange and lemon are sour in test because of presence of acid in that, while Mustards and medicines are examples of a base. Acids can be found in many substances, including food. Mainly it’s present in fruits. The most common example is citric acid present in citrus fruits like orange, lemon and vinegar contains acetic acid. Some acids are invariably used in laboratory, like; hydrochloric acid, sulphuric acid and nitric acid. The water soluble bases are called alkalis.  

In general, these are usually found in grime cleaners which help in cleaning grease from metallic frames and floors and are found in the soap, toothpaste, egg whites, dish washing liquids and household ammonia. Have you ever thought the presence of any acid or base in your body? Yes, our body contain some very common acid like dilute hydrochloric acid in stomach, which involve in the digestion of food. If stomach contents of ours become little acidic, we usually end up in indigestion and burning sensation in stomach. Acids and bases are also regulating many metabolic activities in human body carried out by equilibrium processes and effect. Stings of bees are found to be acidic in nature while wasp stings are supposed to be alkaline in nature.

We can explain the concept of acids and bases with the help of ppt presentation which must start with introduction and moves to general properties of acid and base. Let’s discuss few of the properties of these compounds. All acids characterised by H+ in solution and base by hydroxide ion OH-. The best way to identify the presence of acid and base is to use litmus paper which shows a color change in acidic and basic medium. Now explain some more indicators which can be used to identify the acidic and basic nature of compounds. Red litmus paper turns blue if exposed to an acid, and blue litmus paper turns red when a base is present. Other natural detectors, besides taste, are red onions, red cabbage and grape juice. In very acidic conditions, the colour is red. In alkaline solutions, it will be go from blue to green. Red cabbage juice which is purple in color changes to red in acidic medium and yellow in basic medium.

Therefore an indicator is a chemical that shows change in color in acidic and alkaline medium. Many other indicators change color when the medium fluctuates. One such is phenolphthalein. It shows deep pink color in a basic medium and colorless in an acidic medium. The addition of phenolphthalein solution in sodium hydroxide changes the color of solution to pink. Now addition of any acid to this pink solution turns it to colorless. Methyl red is another most commonly used as an indicator in laboratory for titrations. In a basic solution, methyl red turns yellow in colour. When we chop an onion, we are breaking some open onion's cells which release enzymes. These enzymes act on one of the flavouring components of onions and contain mainly allicin which is a S-containing compound. It is responsible for volatile irritant "fumes" up from the onion and irritates our eyes.

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Acids and Bases ACIDS AND BASES

The name "acid" calls to mind vivid sensory images—of tartness, for instance, if the acid in question is meant for human consumption, as with the citric acid in lemons. On the other hand, the thought of laboratory-and industrial-strength substances with scary-sounding names, such as sulfuric acid or hydrofluoric acid, carries with it other ideas—of acids that are capable of destroying materials, including human flesh. The name "base," by contrast, is not widely known in its chemical sense, and even when the older term of "alkali" is used, the sense-impressions produced by the word tend not to be as vivid as those generated by the thought of "acid." In their industrial applications, bases too can be highly powerful. As with acids, they have many household uses, in substances such as baking soda or oven cleaners. From a taste standpoint, (as anyone who has ever brushed his or her teeth with baking soda knows), bases are bitter rather than sour. How do we know when something is an acid or a base? Acid-base indicators, such as litmus paper and other materials for testing pH, offer a means of judging these qualities in various substances. However, there are larger structural definitions of the two concepts, which evolved in three stages during the late nineteenth and early twentieth centuries, that provide a more solid theoretical underpinning to the understanding of acids and bases. Prior to the development of atomic and molecular theory in the nineteenth century, followed by the discovery of subatomic structures in the late nineteenth and early twentieth centuries, chemists could not do much more than make measurements and observations. Their definitions of substances were purely phenomenological—that is, the result of experimentation and the collection of data. From these observations, they could form general rules, but they lacked any means of "seeing" into the atomic and molecular structures of the chemical world. The phenomenological distinctions between acids and bases, gathered by scientists from ancient times onward, worked well enough for many centuries. The word "acid" comes from the Latin term acidus, or "sour," and from an early period, scientists understood that substances such as vinegar and lemon juice shared a common acidic quality. Eventually, the phenomenological definition of acids became relatively sophisticated, encompassing such details as the fact that acids produce characteristic colors in certain vegetable dyes, such as those used in making litmus paper. In addition, chemists realized that acids dissolve some metals, releasing hydrogen in the process. The word "alkali" comes from the Arabic al-qili, which refers to the ashes of the seawort plant. The latter, which typically grows in marshy areas, was often burned to produce soda ash, used in making soap. In contrast to acids, bases—caffeine, for example—have a bitter taste, and many of them feel slippery to the touch. They also produce characteristic colors in the vegetable dyes of litmus paper, and can be used to promote certain chemical reactions. Note that today chemists use the word "base" instead of "alkali," the reason being that the latter term has a narrower meaning: all alkalies are bases, but not all bases are alkalies. Originally, "alkali" referred only to the ashes of burned plants, such as seawort, that contained either sodium or potassium, and from which the oxides of sodium and potassium could be obtained. Eventually, alkali came to mean the soluble hydroxides of the alkali and alkaline earth metals. This includes sodium hydroxide, the active ingredient in drain and oven cleaners; magnesium hydroxide, used for instance in milk of magnesia; potassium hydroxide, found in soaps and other substances; and other compounds. Broad as this range of substances is, it fails to encompass the wide array of materials known today as bases—compounds which react with acids to form salts and water. The reaction to form salts and water is, in fact, one of the ways that acids and bases can be defined. In an aqueous solution, hydrochloric acid and sodium hydroxide react to form sodium chloride—which, though it is suspended in an aqueous solution, is still common table salt—along with water. The equation for this reaction is HCl(aq ) + NaOH(aq ) →H2O + NaCl(aq ). In other words, the sodium (Na) ion in sodium hydroxide switches places with the hydrogen ion in hydrochloric acid, resulting in the creation of NaCl (salt) along with water. But why does this happen? Useful as this definition regarding the formation of salts and water is, it is still not structural—in other words, it does not delve into the molecular structure and behavior of acids and bases. Credit for the first truly structural definition of the difference goes to the Swedish chemist Svante Arrhenius (1859-1927). It was Arrhenius who, in his doctoral dissertation in 1884, introduced the concept of an ion, an atom possessing an electric charge. His understanding was particularly impressive in light of the fact that it was 13 more years before the discovery of the electron, the subatomic particle responsible for the creation of ions. Atoms have a neutral charge, but when an electron or electrons depart, the atom becomes a positive ion or cation. Similarly, when an electron or electrons join a previously uncharged atom, the result is a negative ion or anion. Not only did the concept of ions greatly influence the future of chemistry, but it also provided Arrhenius with the key necessary to formulate his distinction between acids and bases. Arrhenius observed that molecules of certain compounds break into charged particles when placed in liquid. This led him to the Arrhenius acid-base theory, which defines an acid as any compound that produces hydrogen ions (H+) when dissolved in water, and a base as any compound that produces hydroxide ions (OH−) when dissolved in water. This was a good start, but two aspects of Arrhenius's theory suggested the need for a definition that encompassed more substances. First of all, his theory was limited to reactions in aqueous solutions. Though many acid-base reactions do occur when water is the solvent, this is not always the case. Second, the Arrhenius definition effectively limited acids and bases only to those ionic compounds, such as hydrochloric acid or sodium hydroxide, which produced either hydrogen or hydroxide ions. However, ammonia, or NH3, acts like a base in aqueous solutions, even though it does not produce the hydroxide ion. The same is true of other substances, which behave like acids or bases without conforming to the Arrhenius definition. These shortcomings pointed to the need for a more comprehensive theory, which arrived with the formulation of the Brønsted-Lowry definition by English chemist Thomas Lowry (1874-1936) and Danish chemist J. N. Brønsted (1879-1947). Nonetheless, Arrhenius's theory represented an important first step, and in 1903, he was awarded the Nobel Prize in Chemistry for his work on the dissociation of molecules into ions. The Brønsted-Lowry acid-base theory defines an acid as a proton (H+) donor, and a base as a proton acceptor, in a chemical reaction. Protons are represented by the symbol H+, and in representing acids and bases, the symbols HA and A−, respectively, are used. These symbols indicate that an acid has a proton it is ready to give away, while a base, with its negative charge, is ready to receive the positively charged proton. Though it is used here to represent a proton, it should be pointed out that H+ is also the hydrogen ion—a hydrogen atom that has lost its sole electron and thus acquired a positive charge. It is thus really nothing more than a lone proton, but this is the one and only case in which an atom and a proton are exactly the same thing. In an acid-base reaction, a molecule of acid is "donating" a proton, in the form of a hydrogen ion. This should not be confused with a far more complex process, nuclear fusion, in which an atom gives up a proton to another atom. The most fundamental type of acid-base reaction in Brønsted-Lowry theory can be symbolized thus HA(aq ) + H2O(l ) →H3O+(aq )

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. Properties Acids in water solutions exhibit the following common properties: they taste sour; turn litmus paper red; and react with certain metals, such as zinc, to yield hydrogen gas. Bases in water solutions exhibit these common properties: they taste bitter; turn litmus paper blue; and feel slippery. When a water solution of acid is mixed with a water solution of base, water and a salt are formed; this process, called neutralization , is complete only if the resulting solution has neither acidic nor basic properties. Classification Acids and bases can be classified as organic or inorganic. Some of the more common organic acids are: citric acid , carbonic acid , hydrogen cyanide , salicylic acid, lactic acid , and tartaric acid . Some examples of organic bases are: pyridine and ethylamine. Some of the common inorganic acids are: hydrogen sulfide , phosphoric acid , hydrogen chloride , and sulfuric acid . Some common inorganic bases are: sodium hydroxide , sodium carbonate , sodium bicarbonate , calcium hydroxide , and calcium carbonate . Acids, such as hydrochloric acid, and bases, such as potassium hydroxide, that have a great tendency to dissociate in water are completely ionized in solution; they are called strong acids or strong bases. Acids, such as acetic acid, and bases, such as ammonia, that are reluctant to dissociate in water are only partially ionized in solution; they are called weak acids or weak bases. Strong acids in solution produce a high concentration of hydrogen ions, and strong bases in solution produce a high concentration of hydroxide ions and a correspondingly low concentration of hydrogen ions. The hydrogen ion concentration is often expressed in terms of its negative logarithm, or p H (see separate article). Strong acids and strong bases make very good electrolytes (see electrolysis ), i.e., their solutions readily conduct electricity. Weak acids and weak bases make poor electrolytes. See buffer ; catalyst ; indicators, acid-base ; titration . Acid-Base Theories There are three theories that identify a singular characteristic which defines an acid and a base: the Arrhenius theory, for which the Swedish chemist Svante Arrhenius was awarded the 1903 Nobel Prize in chemistry; the Brönsted-Lowry, or proton donor, theory, advanced in 1923; and the Lewis, or electron-pair, theory, which was also presented in 1923. Each of the three theories has its own advantages and disadvantages; each is useful under certain conditions. The Arrhenius Theory When an acid or base dissolves in water, a certain percentage of the acid or base particles will break up, or dissociate (see dissociation ), into oppositely charged ions. The Arrhenius theory defines an acid as a compound that can dissociate in water to yield hydrogen ions, H + , and a base as a compound that can dissociate in water to yield hydroxide ions, OH -  . For example, hydrochloric acid, HCl, dissociates in water to yield the required hydrogen ions, H + , and also chloride ions, Cl -  . The base sodium hydroxide, NaOH, dissociates in water to yield the required hydroxide ions, OH - , and also sodium ions, Na + . The Brönsted-Lowry Theory Some substances act as acids or bases when they are dissolved in solvents other than water, such as liquid ammonia. The Brönsted-Lowry theory, named for the Danish chemist Johannes Brönsted and the British chemist Thomas Lowry, provides a more general definition of acids and bases that can be used to deal both with solutions that contain no water and solutions that contain water. It defines an acid as a proton donor and a base as a proton acceptor. In the Brönsted-Lowry theory, water, H 2 O, can be considered an acid or a base since it can lose a proton to form a hydroxide ion, OH - , or accept a proton to form a hydronium ion, H 3 O + (see amphoterism ). When an acid loses a proton, the remaining species can be a proton acceptor and is called the conjugate base of the acid. Similarly when a base accepts a proton, the resulting species can be a proton donor and is called the conjugate acid of that base. For example, when a water molecule loses a proton to form a hydroxide ion, the hydroxide ion can be considered the conjugate base of the acid, water. When a water molecule accepts a proton to form a hydronium ion, the hydronium ion can be considered the conjugate acid of the base, water. The Lewis Theory Another theory that provides a very broad definition of acids and bases has been put forth by the American chemist Gilbert Lewis. The Lewis theory defines an acid as a compound that can accept a pair of electrons and a base as a compound that can donate a pair of electrons. Boron trifluoride, BF 3 , can be considered a Lewis acid and ethyl alcohol can be considered a Lewis base.

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Question:This is an acid base titration lab and I need to design an experiment. Please try to make instructions as detailed as possible. Will choose best answer.

Answers:Have you heard of Google? This will give you the information that you want without delay. Because I did not want to spend a long time typing up a detailed reply, I entered < acid/base titration> into Google and came up with: The key equipment used in a titration are: * Burette * White Tile - used to see a color change in the solution * Pipette * Acid/Base Indicator (use phenolphthalein) * Erlenmeyer flask (conical flask) * Standard Solution (a solution of known concentration, u=in your case HCl * Solution of unknown concentration I slightly edited the following to simplify it for you: The point at which the indicator changes color is called the end point. A suitable indicator should be chosen, preferably one that will experience a change in color (an end point) close to the equivalence point of the reaction. For strong base/ strong acid titrations the most convenient indicator is phenolphthalein First, the burette should be rinsed with the standard solution, the pipette with the unknown solution, and the conical flask with distilled water. Discard the rinsings. Secondly, a known volume of the unknown concentration solution should be taken with the pipette and placed into the conical flask, along with a small amount of the indicator chosen. The burette should always be filled to the top of its scale with the known solution for ease of reading. The known solution should then be allowed out of the burette, into the conical flask. At this stage we want a rough estimate of the amount of this solution it took to neutralize the unknown solution. The solution should be let out of the burette until the indicator changes color and the value on the burette should be recorded. This is the first (or rough) titre and should not be included from any calculations. Three more titrations should be performed, this time more accurately, taking into account roughly where the end point will occur. The readings on the burette at the end point should be recorded, and averaged to give a final result. The end point is reached when the indicator just changes color permanently. Now you have the volume of acid required to neutralise the known volume of NaOH. Calculate the molarity of the NaOH solution using the equation: M1V1 = M2V2 Where M1 = molarity of HCl - you have 1.50M V1 = volume of HCl used from burette M2 = molarity of unknown NaOH - what you are to determine V2 - volume of NaOH solution added to flask using burette. To simplify: M2 = M1V1/V2 Record the molarity of the NaOH solution as your answer.

Question:Acid and Bases Defentions Acids and Bases Examples What is the differance between them?

Answers:Acid is a proton donor. Base is a proton acceptor. Acids also always INCREASE hydrogen concentration. Bases always INCREASE hydroxide concentration Example of an acid: HCl Example of a base: NaOH Difference between them: pretty much is the definitions.

Question:What does an acid react with, what does a base react with? Also, are acids and bases electrolytes or molecules?

Answers:acids react with bases,metals or alkali. Bases react with acids

Question:ACIDS and BASES. Identify its color changes and classify it as an acid or a base. Substance tested: ACETIC ACID Red litmus paper: Blue litmus paper: Phenolphthalein: Is it an Acid or a Base?

Answers:ACIDS and BASES. Identify its color changes and classify it as an acid or a base. Substance tested: ACETIC ACID Red litmus paper: No Change Blue litmus paper: Pink/red Phenolphthalein: Pink Is it an Acid or a Base? ACID

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Ch9 ppt notes example #2 1 :At soft drink factories, carbon dioxide can be made from chalk and acid. If each 16 ounce bottle of Pepsi needs 1.1 liter of CO2 in it, how many grams of chalk were used for one bottle of Pepsi? The balanced equation is: CaCO3 + 2HCl CaCl2 + CO2 + H2O