what (with universal indicator) Ph is Ethanoic acid?
350659
Why do people answer complete and total bullcrap answers?\n\n\nThe only thing they were right about was it is a weak acid, and even that bears no relavance to its P.H only you use a diferent formula in calculating it\n\n\nthe question is incomplete, you need to know the molarity of the acid and then you get the square root of it disociation constant (Ka) multiplied by its molarity\n\nand then you -log(base10)the answer you got from the first part and that is the P.H\n\nin short  Sq root(Ka*molarity acid)= H+ concentration\n\nP.H= -logH+
920228
CuSO4•5H20\nThe dot notation denotes the hydrate.
445522
Acetic acid (HC2H3O2, or CH3COOH). Vinegar.
192513
A strong acid, like HCl, might cleave your ethanoic annhydride. That's the only thing I can think of. Phosphoric acid gives you a weak source of protons.
921604
theoretically yes 10m acid has a pH of -1, and 10 moles of base pH 15.\n\nBut , in fact, for very high concentrations, you must not take in account the concentration of ions H+ but the activity . The actvity takes in account the high concentration and is \n\nactivity = gamma * pH where gamma is lower than one for high concentrations
814491
formic\n\nFormic acid (systematically called methanoic acid) is the simplest carboxylic acid. Its formula is CH2O2 or HCOOH.
1057594
I think this is how you do it:\nacid and base is measured in terms of pH and pOH. as you know, the H makes it acidic and the OH makes it basic, and if you mix an H and OH, you get water, which is to say it was neutralized.\nSo, let's say you have HBr with a pH of 4. You that pH is a measure of the concentration of H present in the mixture. So, to get the actual number you do -10ph, and you'll get a number like 10^-5 or something. So, to neutralize that many Hs, that's how many OH's you need. so, you'll need a pOH 4, which is the same thing is a pH of 10 (pOH = 14 - pH). \nhope that helps, good luck. and read the book, and do some of hte exercised in the book.
513863
Since it is a strong monoprotic acid:\n\npH=-log[Acid]= -log[0.105] = 0.98\n\npOH= 14- pH = 14- 0.98 = 13.02
114804
No need to break it down to "molecular" other wise, try this: Sodium thiosulphate. Dont just use it coz they all vary in their Ph U know the basisity or acidity they concentrate.
1125360
H2O2 can exist in many forms at pH = 7, \n\nH3O2+, H3O3- are among the possibilities.
224213
well, pH = -log[H+]. so if you just undo the log you will have the concentration of H+ (which is the same as H30+). then .. [H+} + [OH-] = 14 good luck!
713316
HNO3\n\nIf you couldn't answer this question, you must be a real noob in chemistry!!  Well, for other times, here's the way to differentiate betwee acids and bases.\n\nAcids:   acids can be easily identified by the hydrogens they contain.  Most acids have their hydrogen in the beginning of their formula.  HNO3 can be easily identified as an acid: it is commonly called nitric acid.\n\nBases:  most bases can be identified by the (OH) group at the end of their formula... therefore, we can immediately label b) and d) as bases.   \n\nNow here, NH3 is kind of tough to define with the definitions given above.   I believe that the proper explanation is out of your scope for know (from what I can deduce).   So, you'll learn that later on.  But for your info, NH3 is ammonia, the stuff they use in cleaning fluids, and it is basic.\n\nHope this helps.
455471
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
99880
Glacial Acetic Acid freezes/melts at slightly under room temperature (62.1F,16.7C).
222097
OH-(aq) + HC2H3O2(aq)---> H2O(l) + C2H3O2-(aq)
570617
KMnO4 is an oxidizing agent.\n\nit will turn ethanol into ethanal (or acetylaldehyde).  if there is a great excess of potassium permanganate, it will turn ethanal into ethanoic acid (or acetic acid).\n\nbasically, both steps involve decreasing the number of bonds from carbon to hydrogen and increasing the number of bonds from carbon to oxygen.
851253
hydrochloric acid, acetic acid (vinegar), boric acid, sulphuric acid, ascorbic acid(vitamin c) etc.