define acid and base.?
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In general science terms, an acid is a molecule or ion that, when placed in water, will give up a hydrogen ion (H+) to a base, or accept an unshared pair of electrons from a base. \n\nA base is a substance which dissociates (separates) in aqueous solution to yield hydroxyl ions (OH-) which react with an acid to form a salt.\n\nAcids and bases react with one another in a neutralization reaction to form a salt. This is also the basis of buffers.\n\nIf you want to get down the simplest definitions: \n\nAn acid is a solution that has more free hydrogen ions (H + ) than hydroxyl ions (OH - ) and a pH less than 7.\n\nA base is a solution that has less free hydrogen ions (H + ) than hydroxyl ions (OH - ) and a pH of more than 7.
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Any acid, for example:\n\nHCl + H2O  --> Cl- + H3O+
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Technically with molar amounts being equal, an acid and a base react in what is called a "neutralization reaction"...\n\nie:\n\nHCl + NaOH ---> NaCl and water\n\nBasically you get a salt and a water.
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A base - any phosphate is a base
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pH from 0 to 7: Acid solution.\nPH from 7 to 14: Basic solution.
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B/L acids HBr, NH4, H3O, HSO3, H20 respectively. the other reactant is a B/L base.
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2 M HCl\n\nHCl is a strong acid and acids have pH less than 7\n\nH3PO4 is a weak acid\n\nNH3 is a base\n\nNaOH is a base
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acid\ngas naphtha\noxygen  and hydrogen\nacid\nacid
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What I think you're talking about are how acidic and how basic something is according to the pH scale.  Maybe?  \n\nWe us the pH scale to describe how acidic or how basic a solution is. pH stands for potential of hydrogen. It's numbered from 1 to 14--increasing in basicity.\n\nHydrogen and hydroxide ions are very reactive, and the proper balance of these ions is critical for the proper functioning of chemical processes within an organism.\n\nA compound that donates hydrogen ions to solutions is called an acid.  Examples of an acid would be something like lemon juice and tomato juice.  Even the gastric juice inside of your stomach.\n\nA base is a compound that accepts hydrogen ions and removes them from solutions.  Examples of a base would be something like bleach or oven cleaner.\n\nThe increasing acidity means there's a higher concentration of H+.  The decreasing basicity means there's a lower concentration of H+.  \n\nPURE WATER is neutral----or 7 on the pH scale.\n\nHope this helps. :o)
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Ph is A measure of the acidity or alkalinity of a solution, numerically equal to 7 for neutral solutions, increasing with increasing alkalinity and decreasing with increasing acidity. The pH scale commonly in use ranges from 0 to 14.
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Acidic \n\nbelow 6 acidic above 7 basic
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N=aM where a in the case of acids is the number of H+ the molecule can give (regardless if it is a strong or weak acid)\n\nso N=aM=3*0.20=0.60\n\na for a base would be the number of OH- it gives (or number of H+ that it receives), whereas for redox reactions the number of electrons gained/lost during the reaction or if you prefer the change in the oxidation number
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HNO3 and NH4NO3. A buffer is a solution of a weak acid with the corresponding weak base. It is set up to maintain a specific range os Ph, determined by the proportions of acidvs base and by the POh of the acid/base. The amoutnt of H+ that a buffer syatem can absorb before the buffer breaks is determined by the streangth, ie molarity, of the solution. a
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Sulfuric Acid- just learned that today... check the link for more info...\nit is a VERY strong acid!
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an organic base is an organic compound(contains carbon) that will act as a base in a reaction.ie it will either donate an OH- ion or it will accept a H+ ion..ie a proton
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acid has a ph value below 7\nand alkali has a value above 7\n\nAn acid (often represented by the generic formula HA) is traditionally considered any chemical compound that when dissolved in water, gives a solution with a pH of less than 7. That approximates the modern definition of Brønsted and Lowry, who defined an acid as a compound which donates a hydrogen ion (H+) to another compound (called a base). Common examples include acetic acid (in vinegar) and sulfuric acid (used in car batteries). Acids generally taste sour;\n\nIn chemistry, an alkali (from Arabic: al-qaly القالي) is a specific type of base, formed as a carbonate, hydroxide or other basic (pH greater than 7) ionic salt of an alkali metal or alkali earth metal element. The word alkali or the adjective alkaline are frequently used to refer to all bases, since most common bases are alkalis, although strictly speaking this is inaccurate.
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1 is c.  Buffer is a mixture of a weak acid and its conjugate base.\n2 is a.  pH is the dependent variable in the experiment, volume of titrant (either acid or base) is the independent variable.