what does OH stand for in chemistry terms?
440388
Hydroxide Ion \nor if attached to another compound an alchohol group
925482
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.
169778
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)
265538
well, the [H+] (which is the same as [H3O+]) concentration and the [OH-] concentration always add up to 1.0x10^=14. so an equation for that would look like\n\n[H+] x [OH-] = 1.0x10^-14\n\nso just divide 1.0x10^-14 by your concentration of H30+. its as easy as taht!
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OH- is an alkali (pH is more than 7) and H+ is an acid (pH is less than 7).\n\nAcid + Alkali -> Neutrality\n\nSince it's neutral, water (pH 7) is produced.\n\nHope my explanation helped c",)
309221
The OH group comes from the acid in esterification, but when you're writing out the reaction, it doesn't really matter where it comes from; you'll end up with the correct formulas regardless.
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Methoxy-. For example, if you have a toluene molecule with a -O-CH3 next to the methyl group, it would be 2-methoxytoluene.
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1 mol of Mg + 2 mol of OH = 1 mol of Mg(OH)2 because there is only one Mg used and 2 OH molecules
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Here is a great site that explains it for pretty much all chemical nomenclature.\nhttp://dbhs.wvusd.k12.ca.us/webdocs/Nomenclature/Nomenclature.html
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The only other way I know of is to know the formula of a compound or ion/radical containing that element, and use the following rules:\n1. Total for all elements in a compound must be 0. Total for an ion is the charge on the ion.\n2. First element in a compound is always (+); last element in a compound is always (-). (Not necessarily true for ions: Hydroxide ion OH- has O -2 and H +1; I believe it's true for all other ions/radicals but not certain.)\n3. H is always +1 or -1.\n4. O is almost always -2, unless it's -1 or +2 because of one or more of the above rules. (Example 1: Oxygen molecule O2 has one +2 and one -2; Example 2: Hydrogen peroxide H2O2 has two H +1 and two O -1.)\nIn fact, oxidation number doesn't mean much unless it's in the context of a compound. As above, oxygen atom can be either -2, -1 or +2 depending on the compound it's in. In fact, a molecule with two or more oxygen atoms can even have its oxygen atoms in different oxidation states!
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a) neutral\nb) basic\nc) basic\nd) acidic\ne) acidic if in solution\nf) basic.\n\npH is a scale ranging from 0-14.  7 is the intermediate and a pH of 7 means that the solution is neutral.  If the pH is below 7, then there are more H+ than OH- in the solution.  Hence the solution becomes acidic.  If the pH however is greater than 7, then there is less H+ than OH- in the solution and the solution is basic.\n\nFor the acid H2SO4, when in solution, it will dissociate to form H+ and SO4-.  The H+ gives the acid its acidic property.  Similarly when Ca(OH)2 is dissolved, it dissociates into Ca2+ and OH-.  The OH- gives the compound its basic property.
859846
That is all a matter of how you look at it. pH is the negative log of the hydrogen ion concentration. We say if something has a pH of less than 7, it is acidic. Soda contains carbonic acid and phosphoric acid, and thus has a pH less than 7. On the other hand, the sum of the pH and the pOH should equal 14. pOH is defined as the negative log of the hydroxide concentration. So, if the pH is 5, the pOH is 9, thus showing OH- to be present.\n\nPotato, potato....glass half empty, half full kinda thing...
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SOH stands for Sine equals Opposite over Hypotenuse.\n\nCAH stands for Cosine equals Adjacent over Hypotenuse.\n\nTOA stands for Tangent equals Opposite over Adjacent.
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The abbreviation for Oxygen is O2 (O subscript 2) because it is diatomic, which means that you find 2 oxygen molecules together naturally.
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H2CO2 is better written as HCO(OH).\n\nThe dissociation equation is:\n\nHCO(OH) ---> HCOO(-) + H(+)\n\nYou can see from the reaction that it can give only one proton (The other H, bound to the C is not acidic).\n\nSo monoacid.
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p stands for "potenz" which means potential, H stands for Hydrogen. Thus, pH stands for "Hydrogen potential" and it's a measure of acidity.
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d) Reducing agent. Oxidation is the loss of electrons. The substance getting oxidized donates the electrons to the subnstance getting reduced. For that reason, a) Electron donor is also correct.\n\nI don't know if you're allowed more than one answer to this question. It may be that the teacher did not see that the reducing agent was an electron donor, and thought of electron donation in the Lewis base sense, which does not come up in this question.