why carboxylic acid is stronger then phenol?
408703
By Carboxylic acid, let's assume you mean an aliphatic carboylic acid with no electron withdrawing groups attached.\n\nSo let's compare ... acetic acid to phenol.\n\nAcetic acid's pka is 4.76\n\nphenol's pka is 9.95\n\nClearly acetic acid is more acidic. The answers above are essentially correct. A carboxylic acid is stabilized through resonance through the 2 carbonyl groups. The phenoxide anion is stabilized through delocalization of the electrons in a pi system. At the end of the day, though, phenol is still an alcohol and its proton is not given willingly in solution.
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?
336797
The Phenol Coefficient test compares the potency of a disinfectant with that of phenol. A series of dilutions of phenol and the experimental disinfectant are inoculated with the test bacteria Salmonella typhi and Staphylococcus aureus, then placed in a 20 or 37 degree water bath. The highest dilution that kills the bacteria after 10 minutes exposure, \nbut not after 5 minutes are used to calculate the phenol coefficient.\n\nThe higher the phenol coefficient value, the more effective the disinfectant. A value greater than 1 means that the disinfectant is more effective than phenol.\n\nIts advantage is its ease of use.\n\nHowever, the EPA no longer recognizes a product's phenol coefficient as confirmation of its disinfecting capabilities since some products with high phenol coefficients were ineffective when used in the presence of certain organic matter and products with low phenol coefficients can be effective under \nactual use conditions.
27502
Simplest reason is that acetic acid is more water soluble than isopentyl alcohol. That five carbon chain on the alcohol is nonpolar and reduces water solubility.
520962
Did you really need to post this question twice in one minute?\n\nBoth hydrochloric (HCl) and sulfuric (H2SO4) acids can damage human flesh -- the severity of damage and the speed at which it happens depends on the concentration of the acid.\n\nThe same applies to many metals -- the stronger the acid, the more rapidly the acid corrodes and dissolves it.\n\nPlastics are another thing altogether.  Some plastics are completely impervious to both acids, no matter what the concentration.  Other polymers are slowly attacked by the acids, slowly rendering them brittle.  I can't think of any specific polymers off the top of my head that are incompatible with HCl and H2SO4, but I'm sure there are some.
1044294
In the Cannizzaro's reaction a strong base, say OH- attacks the electron-deficient carbon in the initial stage. This is followed by a hydride shift and ultimate proton exchange to form the final stable species. Of almost all aldehyde's compatible for the Cannizzaro rxn formaldehyde is perhaps most e-deficient. So OH0- always attacks it first. The compound that OH- attacks initially gives the acid ultimately. Hence formaldehyde almost always becomes formic acid [oxidation].
730330
Different chemical composition, one has a reaction the other doesn't..☺
236592
Carboxylic acids are named by dropping the -e ending of the parent name and adding -oic acid
992740
Higher the charge greater the tendency to accept electrons, hence more acidic\n\nLower the radius, higher concentration of charge, hence more acidic.\n\nIn3+ is larger than Al3+ hence a weaker acid.
423094
An example of a compound form when carboxylic acid and alcohol react.\n\nAn equation for such a reacton is\n\n R-COOH + R'-OH = R-COO-R' + H2O \n\nthe -COOH group and the -OH group lose a water and become a -COO- linkage: \n\n\nwhere R and R' represent organic groups.
955333
an easy example you can remember is H2O(water).\nif u want a more difficult one, u can use CH3COOH(acetic acid)!\n\nALL DE BEST!
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.
739831
At first a molecule that donates a proton is an acid, not a base - according to the Broensted-Lowry definition of acids and bases.\n\nAdding an electronegative atom in a molecule of an acid increases the acidity - or, the same decreases the basicity - of the molecule. For example:\n\nCl-CH2COOH is a stronger acid than CH3COOH\n\nCl-NH2 is a weaker base than NH3.
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The benefit is that acetic acid is used as a catalyst for organic reactions, because it won't add a substrate onto a double bond.\n\nThe disadvantage is that glacial acetic acid can cause severe burns and even its mist is a lachrymator (sp).
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For solubility.  Many drugs have carboxylic acid functionalities which are more soluble in water (i.e. blood, etc.) as their sodium salts
993231
Okay, first picture a benzene ring - six carbons, flat topology thanks to its aromaticity.  By definition, the benzene carbon with the carboxylic acid group attached is carbon #1.  So, you have two cases here, both with a ring substituent "para" (or directly opposite) the carboxylic acid.  Everybody on the same page?\n\nNow, acidity is defined, in simple terms, as the willingness of a molecule to give up a proton, aka an H+ ion.  The more easily it will part with that H+, the more acidic a compound is.  So, the question, really, is what makes a proton stay stuck to an acid?\n\nA carboxylic acid anion (COO-) has a large electron density delocalized between its two oxygen atoms.  A hydrogen ion will tend to stay stuck to this negatively charged group to balance out it's negative charge.  In layman's terms, a carboxylic acid is more comfortable with a positively charged bit hanging around to make all those nonbonding electrons on the oxygens less unwieldy.  \n\nWith your two compounds, the difference between them is the substituent in the 4 position.  Remember that an aromatic system like this has a flat electron cloud above and below the ring, and this electron cloud will interact directly with any ring substituents.  \n\nThe methoxy group is an electron donor.  It is not, overall, very electronegative, so it will tend to "push" its electron density into the benzene ring, and that will tend to prevent the  carboxylate group from sharing its negative charge density with the aromatic system.  With the negative charge localized to the carboxylate, it will be difficult for the hydrogen ion to dissociate, and 4-methoxybenzoic acid will be very weak.  \n\nFluorine, on the other hand, is an excellent  electron sink; it is one of the most electronegative substituents you can put on a benzene ring.  It will tend to draw electron density towards itself, allowing the carboxylate to push some of its negative charge into the aromatic ring.  The negative charge, then, will be more delocalized, making it easier for the acidic proton to dissociate from the carboxylate group.  4-fluorobenzoic acid will, therefore, be a stronger acid than 4-methoxybenzoic acid.\n\nDoes that make sense?  I hope this helps.
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Trifluoroacetic acid is a strong acid with a pKa of ~0.2 to 0.3.  Acetic acid is a weak acid with a pKa of 4.75.  \n\nTrifluoroacetic acid is about 10^4.5 (10^(4.75-0.25)) times as dissociated as acetic acid.