What does pH stand for in pH balance?
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Potential of Hydrogen.
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An acid has a higher concerntration of H+ ions in the solution. The PH scale is based on a logorithimic equation where a PH of 7 is neutral, andything below 7 is acidic and anything above 7 is basic. The conjugate acid is the H part of HX where the X- is the conjugate base. \n\nWikipedia has a great explination: http://en.wikipedia.org/wiki/Conjugate_acid
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pH = -log[H+]\n\nand\n\n[H+][OH-] = 1*10^-14\n\nwhere [ ] means concentration of.\n\n\nSo, to work out [H+], you divide 1*10^-14 by 3*10^-10 to get  3.33333*10^-5\n\nTake the -log of this, and you get 4.477.\n\nThe pH is 4.477.\n\nAll logs are in base 10.
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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",)
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pH (pch) n.\n A measure of the acidity or alkalinity of a solution \n\ntrans·par·en·cy  (trns-pârn-s, -pr-)\nn. pl. trans·par·en·cies \n1. A transparent object, especially a photographic slide that is viewed by light shining through it from behind or by projection. \n\n\nOptical density is the absorbance of an optical element for a given wavelength λ per unit distance:
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pH is the measure of acidity or basicity(alkalinity) of a solution. When pH increases, the solution is more alkaline and when pH decreases the solution is more acidic. A pH of 7 implies that the solution is neither basic(alkaline) nor acidic but neutral. Check the answer to one of the similar questions on Yahoo answers at the following page.
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The concentration of H+ is 3.0 x 10^-4, so you know that the pH will be around 4.  What you need is a calculator that has a LOG button to convert the 0.0003 to an integer value.\n\nSo on your calculator you press the LOG button and then type in 0.0003 and then a ")" and press ENTER.  \n\nYou should get a result that says: -3.522878745 or so.  You need to round off to -3.5 and since pH is the NEGATIVE log of the hydrogen ion concentration you get rid of the minus.\n\nThe answer is 3.5.\n\n1x10^-3.5 is approximately equal to 0.0003.
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basically, we call it an acid if the compound can be resolved into existing H+ and OH- ions. if this can be resolved then it is called acid and base. \n\nThis is pH. amount of H+ ions and amound of OH- ions. more the amount of free H+ ions in the compund more the acidic nature.\nmore the OH more the basic nature and less is the acidic nature.\n\nIt also depends on the medium in which the compound is present. some act as acids in aqueous medium. and so on....\n hope it was helpful. \nAny doubts u can ask further.
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NH4ClO4 --> NH4^+ + ClO4^-\n\nNow in a water solution,\nClO4^- + H2O --> HClO4 + OH- --> This doesn't happen because HClO4 is a strong acid.  Therefore the only contribution to the pH is from the NH4^+\n\nNH4^+ <=> NH3 + H^+\nYou start with [NH4^+] = 0.40 M, and [NH3]=[H^+] = 0 M; after undergoing equilibrium [NH4^+] = 0.40 - x, while [NH3]=[H^+] = x; Ka = [NH3][H^+]/[NH4^+] = (x)(x)/(0.40-x) = Kw/Kb = (1 x 10^-14)/(1.8 x 10^5)\nAssume x << 0.40, so x^2/0.40 = 5.56 x 10^-10\nx = 1.49 x 10^-5 M = [H^+]\npH = -log(1.40 x 10^-5) = 4.827
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pH (potential hydrogen) is a measure of the activity of hydrogen ions (H+) in a solution and, therefore, its acidity or alkalinity. In aqueous systems, the hydrogen ion activity is dictated by the dissociation constant of water (Kw = 1.011 × 10−14 at 25 °C) and interactions with other ions in solution. Due to this dissociation constant a neutral solution (hydrogen ion activity equals hydroxide ion activity) has a pH of approximately 7. Aqueous solutions with pH values lower than 7 are considered acidic, while pH values higher than 7 are considered alkaline..\n\npH = -log(concentration of H+)\njust use the equation to figure it out.\nhttp://en.wikipedia.org/wiki/PH
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7.35-7.40 is the normal blood ph. Lower or higher than this may result in acidosis and alkalosis.
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When doing pool chemistry, you want to stay within a particular pH range. To do so, you add various chemicals (Muriatic Acid, for example) to raise or lower the pH. Muriatic Acid is just a weak weak solution of water and HCl, so you are adding H+ to the water to balance it with the OH-.
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The pH of a solution tells you the concentration of the H+ ions in solution.  However, if we know the pH, we can calculate the pOH and from that, the concentration of the OH- ions in solution.\n\npH + pOH = 14\nif pH = 8.25, pOH = 14-8.25 = 5.75\n\nJust like pH = -log([H+]),\npOH = -log([OH-])\n\nIf pOH = 5.75, that means that -log([OH-]) = 5.75, which mean that 10^-5.75 much give us the concentration of OH- ions.\n\n10^-5.75 = 1.778 E-6\nSo we know that the concentration of the OH- ions in the solution with a pH of 8.25 is 1.778 E-6 Molar.\n\n[OH-] = 1.778 E-6 M
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Your blood keeps its pH range stable.
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"Acid Concentration" is well defined.\nIt means: how many acid molecules per unit volume in the liquid.\n   Or more particularly, how many H+ ions are donated by the molecules in \n a unit volume.\nThat because some acid molecules have 2 or 3 H+ ion to donate.\n\nAcid Strength can mean a couple of different things.\n   a) Is that species of molecule strongly acidic?\n         When comparing acid A to acid B, which one donates its H+ ion \n more easily.\n         HCl in water becomes H+ and Cl- right away,\n           so the H+ is just wandering around in that water, looking for \n some damage to do.\n         So we say "HCl is a strong acid".\n         We also say the Acetic Acid in vinegar is a weaker acid.\n          Its molecules H(C2O2H3) try to keep their H's until somebody \n wants it more than they do.\n         The H+ concentration is less, so the acid does less "damage" or \n reacting with things.\n\n  b) Is that solution strongly acidic?\n         A solution is a bucket of water with some concentration of \n chemicals dissolved in it.\n         A strongly acidic solution must have a high instantaneous \n concentration of free H+ ions,\n             regardless of the concentration of other chemicals.\n         A concentrated solution of a weak acid molecule is still a weakly \n acidic solution.\n\nThere are two independent measures of acidity:\n   - concentration of the supposedly acidic molecule,\n             even if it's keeping 99.9% of it's H+'s to itself.\n   - concentration of free H+ ions.\n          The "-log(base10)" of this concentration is called "pH".\n          pH 4  means 10^-4 molar [H+], which is a weak acid solution\n          pH 1 means 0.1 molar [H+], which is a fairly strong acid solution.\nYou need to pin down both to understand the solution well.\n\n\nA pH 4 weak acid solution could be\n     -   a concentrated solution of a weak acid,\n     -   or a 10,000 times diluted solution of a strong acid molecule.\nA strong acid solution with pH=0 can only be\n         a concentrated solution of a strongly acidic molecule.
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The pH level. 7 is neutral. Below 7 is acidic and above 7 is basic. 1 being most acidic and 14 being most basic.
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The "p" stands for negative log.\nSo, the negative log of the concentration of H+ ions in solution gives you the pH.  \n-log[H+] = 3.40\nMultiply both sides by negative one:\nlog[H+] = -3.40\nNow raise 10 to the both sides.  This will cancel out the log function. \n10^log[H+] = 10^-3.40\n[H+] = 3.98E-4 M\n\nTo get the [OH-], just divide the [H+] into 1.00E-14:\n1.00E-14 / 3.98E-4 = 2.51E-11 M