is a base from by hydroxide ions?
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There are two ways to define bases.\n\n1\nThey are inorganic compounds which give negatively charged OH- anions (hydroxyl anions) which can react with cations in a solution. If nothing to react with, they just rise the concentration of hydroxyl anions [OH-] in the water solution. This leads to the rise of pH: if there is 10 times more hydroxyl anions than protons (causing acidity), pH = 8; if 100 times, pH is 9 e.t.c. An example: NaOH.\n\n2\nOrganic compounds can also act like bases: they can take protons (H+) from other compounds. We can say that they decrease the amount of acidic groups in other compounds in this way. Examples of this group of compounds are nitrogen-containing alkaloids (nicotine e.t.c.) which can react like bases with organic acids, forming salts. No effect on pH in the environment, just a reaction between organic base and organic acid.
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NaOH is a strong base that forms hydronium ions (H3O) when introduced to oxacilic acids.  If you know the equation that relates pH to hydronium ion concentration you should be able to calculate the exact change.
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The strong base NaOH will be fully dissociated in water, and you're adding quite a bit (looks like 5 grams/10 mLs).  The water actually consists mostly of hydroxide anions at this point, and hypochlorite ions (your oxidiser) from the bleach.  The pH is 14 or so.  These are the only conditions you'll find Fe(OH)3 at.\n\nIt Ferric hydoxide is  instable due to its loose bonding (easy dissociation) with the hydroxide ions.
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In strongly acidic solutions, anions which are strong bases cannot be present to a great extent. These would include OH- or CH3COO-.\n\nIf the solution also contains silver ions, the halide ions (Cl-, Br- and I-) could not be there as well, because they would precipitate out with the silver.
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bases are proton aceptors.
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Most acids form ions in solutions by _protolysis_ (transferring a hydrogen ion to the solvent), and most bases form ions in solution by disassociation (if they contain OH-ions) or by accepting a hydrogen ion from the solvent.\n\nExample: Na3PO4 + H2O --> 3 Na+ +HPO4(2-) + OH-
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This deals with Bronsted-Lowry (B-L) acids and bases, and conjugate-base pairs \n\nB-L acids: donate H+ ions: STRONG ACIDS dissociate into ions\nH20 + HCl --> Cl- + H+  (H+ is the same as hydronium [H3O+])\nso it can be written as H20 + HCl --> Cl- + H3O+ \nThis looks like it donates a H+ ion, but it dissociates because it is a STRONG acid.  \n\nwk acid: HA= wk acid; A- = conjugate base\nHA + H2O ---> H3O+ + A-\n\nB-L bases: accept H+ ions: STRONG bases dissociate\nNaOH + H2O --> H2O + Na+ + OH-\n\nwk base: B = wk base; HB = conjugate acid\nB- + H2O --> HB + OH-\n\nThat's all you need to know to write all eqns.
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They form basic oxides and hydroxides.  The elements themselves are not basic under any definition of "basic".
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Think of the net ionic equation which is occuring.\nSince both the HCl and Ca(OH)3 are dissolved in aqueous solution, broken into ions, just focus on the H+ and OH- part of it first.\n\nH+(aq) + OH-(aq) --> H2O(l)\nThe Hydronium ion and the Hydroxide ion react to form water.\nWhat is left over are the Ca+2 and Cl- ion which drop out of the net ionic eqaution since they form the very soluble compound, Calcium Chloride (CaCl2).\n\n2 HCl (aq) + Ca(OH)2 (aq) --> 2 H2O (l) + CaCl2 (aq)
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Hydrochloric acid produces H plus and Cl - :2 ions per molecule\n\nWater self ionizes to produce H plus and OH minus : 2 ions\n\nCarbonic acid H2C03 can produce 2 H plus and one C03 two minus ions: 3 ions\n\nSodium hydroxide dissociates to give Na plus and OH minus: 2 ions\n\nCarbonic acid potentially forms the greatest number of ions per molecule\n\n\nCarbonic acid is formed of the greatest number of ions per molecule?
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Hydronium ions, in an aqueous solution.  H30+
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An acid and its conjugate base differs by a hydrogen cation (or proton) H+, so:\n\na. H2SO4 and HSO4-\nd. HCl and Cl-\ne. HF and F-\n\nare conjugate acid-base pairs
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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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Confusion between base and alkali\nThe terms "base" and "alkali" are often used interchangeably, since most common bases are alkalis. It is common to speak of "measuring the alkalinity of soil" when what is actually meant is the measurement of the pH (base property). Similarly, bases which are not alkalis, such as ammonia, are sometimes erroneously referred to as alkaline.\n\nNote that not all or even most salts formed by alkali metals are alkaline; this designation applies only to those salts which are basic.\n\nWhile most electropositive metal oxides are basic, only the soluble alkali metal and alkali earth metal oxides can be correctly called alkalis.\n\nThis definition of an alkali as a basic salt of an alkali metal or alkali earth metal does appear to be the most common, based on dictionary definitions
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A salt is formed between the reaction of an acid and a base. Usually, a neutral salt is formed when a strong acid and a strong base is neutralized in the reaction: \n           H+ + OH- = H2O \nThe bystander ions in an acid-base reaction form a salt solution. Most neutral salts consist of\ncations: Na+,K+,Rb+,Cs+,Mg2+,Ca2+,Sr2+,Ba2+ \nanions:  Cl-,Br- ,I-,ClO4-,BrO4-,ClO3-,NO3-\nThese ions have little tendency to react with water. Thus, salts consisting of these ions are neutral salts. For example: NaCl, KNO3, CaBr2, CsClO4 are neutral salts.\n \nWhen weak acids and bases react, the relative strength of the conjugated acid-base pair in the salt determines the pH of its solutions. The salt, or its solution, so formed can be acidic, neutral or basic. A salt formed between a strong acid and a weak base is an acid salt, for example NH4Cl. A salt formed between a weak acid and a strong base is a basic salt, for example NaCH3COO. These salts are acidic or basic due to their acidic or basic ions.\nAcidic ions: NH4+,Al3+,Pb2+,Sn2+.\nTransition metal ions: HSO4-, H2PO4- \nBasic Ions: F-,C2H3O2-,NO2-,HCO3-,CN-,CO32-,S2-                 SO42-,HPO42-,PO43-
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calcium hydroxide is a base, and is often added to acidic soils to raise the pH. this is very helpful, because some plants cannot absorb needed nutrients in acidic soil. acidic soil is commonly found in the northeast area of the US.
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If your aim is to obtain just plasmid DNA (for example, recombinant cloning vectors) from bacterial cells Then a way would be adding Sodium Hydroxide until the pH of the cell extract reaches 12.012.5, which causes the base pairs in non-supercoiled DNA to break.