the ph of a 1.00M of a monoprotic acid solution is 2.21.what can be said about the  strength of thisacid?
539720
it's a pretty strong acid\n\nGastric Juice has a pH of 1-3\nLemons have a pH of 2.2-2.4\n\ni'd say it's pretty strong\n\nthe closer to 0 the more acidic it is, the closer to 14 the more basic it is\n\n0=VERY strong acid, 14= VERY strong base
592167
We assume NaOH is a strong base and therefore dissociates completely at 60 degrees C. a concentration of .002M solution of NaOH dissociating completely contributes .002 mols/liter of OH ions to the solution. Since pOH = -log[concentration of OH-], pOH = -log.002 = 2.699 (with correct logarithmic sig figs). pH is 14 - pOH, so the pH of the solution will be 14-2.699 = 11.301.
168314
Ionic strength of isolated protein depends on the pH of the medium. At pI i.e. isoelectric pH ionic strenght would be 0.\n\nHope this helps.
530188
"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.
1014284
2.70\n\nregard what ppl saying below, I can make this a little bit more clear.\n\nFirst of all, since the concentration of HCl is 0.00200M and HCl is a strong acid, so we can safely assume 100% dissociation. So, we have 0.02M hydronium ions [one to one ratio]; even if we consider the dissociation of water, it will not make any difference. the dissocation of water is depressed by the presence of "high" concentration of hydronium ions. \n\nyou can even calculate how much water actually dissociates into hydroxide and hydronium ions using the disociation constant of water, 10^-14. But I can guarantee you this will not make ANY difference in pH, say less than 1% for sure.\n\ndissociation of water need to be put into consideration ONLY IF the concentration of hydronium ions is VERY low, say 10^-6 -10^-7, or pH around 7, then it will make a difference. \n\nSo, pH = -log[H3O+]= -log[0.002]= 2.70
62342
Acidity is when an excess of H+ binds H2O as H3O+.  Strong acids are ones like HCl, which in solution will ionize completely--Cl-, being very soluble, will let go of H+ to make the solution acidic.  Other "weak" bases are ones that do not necessarily ionize completely.  Excess H+ will bind to sites in the weak acid molecule rather than binding to H20, meaning that the pH will not be as low (low pH < 7 = acidic).  In this way, a weak acid can act as a buffer--in pure water, it will ionize to a certain extent, but with excess H+, it will bind more H+, but the free H+ in solution will only change very little, and the pH remains rather stable.
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
491609
The weaker the acid, the stronger the conjugate base.  The stronger the acid, the weaker the conjugate base.\n\nBy "strong", we are refering to its ability to dissassociate in water and break into ions.\n\nIt might help if you convert all your pKa values to Ka, or all your Ka values to pKa to make it easier to compare.\nWhat does a high Ka value mean?  What does a low Ka value mean?  How does this compare to your definition of a "Strong" acid/base or a "strong" conjugate acid/conjugate base?
706503
find the heat evolved, assuming heat cap of water is 4.2J/g/K\n\n(31.43-25.32) x 4.2 x 100g = 2566.2J\n\nnow according to definition, molar heat of neutralisation is calculated upon the mols of water formed. this number of mols is equivalent to the no. of mols of the limiting reagent (in this case, the HCl).\n\nmol of HCl= 0.050 x 1 = 0.05mol\n\nenthalpy of neutralisation= 2566.2/0.05= 51324J/mol\n\nthis answer is pretty close to real-life experimental values for strong acid-strong base.
810972
Cool stuff, I used to get confused by ugly chemistry calculations, too :D\n\nYou have 3.88 g acid in 250cm3, so in the 25 cm3 you titrated there are 0.388 g of the acid. You need to know how many moles that is, so that you can calculate molar mass.\n\nThe amount of NaOH used up is 46.5 cm3 × 0.095 mol/dm3, that is 0.0465 dm3 × 0.095 M, which equals 0.00442 mol (It's not exactly that much, but I'll stick with three significant figures).\n\nSince NaOH reacts with monoprotic acids in a 1:1 ratio, that means that there was exactly the same amount of acid in the solution.\n\nNow we know that 0.388 g of the acid is 0.00442 mol, so we can divide the mass by the number of moles to get molar mass. That is 0.388g/0.00442 mol = 87.8 g/mol.\n\nRelative molecular mass is simply molar mass in grams, but without the unit, so Mr of the acid is 87.8.
512828
Most organic acids are not very strong (carboxylic acids).  Some medium strength acids in food include carbonic acid in soda water (pops), Oxalic acid is found in spinach, chocolate and nuts (among other foods) and is another medium strength acid. Phosphoric acid is another medium strength acid used in colas.\n\nWeak acids include: lactic acid in milk/dairy, acetic acid in vinegar, ascorbic acid (vitamin C) in fruits, citric acid in citrus fruits,  etc...
172666
When a salt derived from a strong acid and a weak base dissolves in water, the solution becomes acidic. For example, consider the process\n \nNH4Cl(s) ----H2O ---> NH4+(aq) + Cl-(aq)\n\nThe Cl- ion has no affinity for H+. The ammonium ion NH4+ is  a weak conjugate acid of the base NH4+(aq) and ionizes as follows \n\nNH4+(aq) + H2O(l) <=> NH3(aq) + H3O+(aq)\n\nor simply  \n\nNH4+(aq) <=> NH3(aq)  + H+(aq)\n\nThe equilibrium constant ( or ionization constant) for this process is given by \n\n\n\nKa = Kw / kb  =   1.0*10^-14 / 1.8*10^-5 = 5.6*10^-10\n\n\n      x^2 / .10 =  5.6*10^-10\n\n           x^2  =   5.6*10^-11\n\n             x  =    7.5*10^-6 M  =  [H+]\n\npH  =  -log [H+]\n    \n    =  5.12\n\n     my answer is  C , NH4Cl
986526
Sulfuric acid has a higher dissociation constant than acetic acid.  This means that more of it will dissociate in solution.\nAlso, sulfuric acid has 2 hydrogen atoms  that it can give up to solution vs. 1 from acetic acid.
646163
Presuming that the base is monobasic.\n\na) with 25 ml added, you are at the equivalence point.  The pH is 7.\nb) after adding 25.01 ml, you will have 0.01 ml of base that did not get reacted.  The molarity of the base in solution will then be 0.1 * (0.01/50.01) = 2.0 x 10^-5.  Your pOH is 4.70, pH would be 9.30\nc) Now, it's 0.1 ml of unreacted base.  Molarity is 0.1 * (0.1/50.1) = 2.0 x 10^-4.  Your pOH is 3.70, pH is 10.30.\nd) Now 1 ml of unreacted base.  Molarity is 0.1 * (1/51) = 2.0 x 10^-3.  pOH is 2.70, pH is 11.30.\ne) Now 25 ml of unreacted base.  Molarity is 0.1 * (25/75) = 3.33 x 10^-2.  pOH is 1.48, pH is 12.52.\n\nIn each case, you have to figure out the amount of unreacted titrant and recalculate the molarity as if you were simply diluting it, using McVc = MdVd, where the volume is now the total volume of the solution (the unreacted amount plus the 25 ml of acid and the 25 ml of base that have neutralized each other).
866393
HCOOH is Formic acid.  The pKa = 3.75.\n\nHOOCCOOH is Oxalic acid or Ethanedioic acid.  It has two acidic protons.  The pKa1 is 1.23 and pKa2 is 4.19.  The first of these is very much stronger.
320061
Someone else has asked this same question before, and it really isn't that hard . . .\n\n60 ml of 0.250M HCl plus 60 ml of 0.125M NaOH will result in 120 ml of solution total.  All of the NaOH will have been neutralized by the HCl, leaving an excess of HCl, so the solution will be acidic -- the pH will be much less than 7.\n\n60 ml * (1.0 liter/1000 ml) * (0.250 mole/liter HCl) = .015 mole HCl\n\n60 ml * (1.0 liter/1000 ml) * (0.125 mole/liter NaOH) = .0075 moles NaOH\n\nThat means you will have 0.015 - 0.075 = 0.075 moles of HCl left over after the neutralization.\n\nI leave it for you to calculate the pH of a solution of 0.075 moles of HCl in 120 ml of solution.  Remember that pH = -log(base 10)[H+]
624341
A solution that contains an equivalent amount of an acid and its conjugate base.