what is stronger acid. Monoprotic or diprotic?
83361
It's not really a valid question. The only diprotic strong acid is sulfuric acid (H2SO4) with the loss of its second proton being weak. Otherwise, diprotic acids are weak.\n\nIf you're asking for a comparison between something like HCl or HNO3 and H2SO4, you'd have to consult chemical literature.
137739
hydrochloric acid or sulfuric acid are two of the most commonly known acids\n\nthe strongest known acid is fluoroantimonic acid\n\ni would think soaking a human body in any acid would eventually give you a nice human stew, though
759411
Acidic.  Citric acid.
376499
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.
839133
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.
974122
White vinegar - mild acid.
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
131282
The vinegar in salad dressing has a lot of water in it, which is more polar than both the oil and acetic acid.  As mentioned above, oil is nonpolar, water and acetic acid are polar, nonpolar and polar do not typically mix.  "Like dissolves like."
433633
Date: Mon Nov 15 22:43:44 1999\nPosted By: Tye Morancy, MadSci Admin\nArea of science: Chemistry\nID: 942629613.Ch Message:\n\n\nHi Nathan,\n\n   That's a cool question to ask...\n\n   The strongest acid on earth is a 80% solution of Antimony Pentaflouride in \nHyrdoflouric Acid.  This acid solution is so strong that they could only \nmeasure a 50% solution.  Just to give you an idea of how strong a 50% solution \nis, it would be equivalent to an acid 1018 times stronger than concentrated \nsulfuric acid!!  Pretty strong huh?\n\n   By the way, this acid is listed in the Guiness Book of World Records as the \nstrongest acid known.\n\n   Thanks for the question Nathan...\n\nTye
948423
You are going the wrong way.\nThe dissociation constant of a weak monoprotic acid is Ka. If you have a polyprotic acid then you have Ka1,Ka2,etc and more than one equivalence points.\n\nDo the plot, find the equivalence point, and then pKa=pH for 1/2 volume of base of that needed to reach the equivalence point.\nSince you have a weak acid you don't have the equivalence point at pH=7 but at higher pH (The equivalence point will be at the middle of the rising curve). \nThen Ka=10^-pKa\n\nYou can have a look at \n\nhttp://www.shodor.org/unchem/basic/ab/\n\nhttp://www.chemguide.co.uk/physical/acidbaseeqia/phcurves.html
687922
Actually, if you mean strength as in acidity, a solution with a pH of 5 would be 10 times stronger than one with a pH of 6.\n\nHowever, both would be very weak acids, since neutral is about pH 7.
265381
The answer to your question is 1) Val to Leu.  They are both hydrophobic amino acids and Leu has just one more carbon.\n\nFor 2) Asp has an acid and Pro is hydrophobic and cyclic.\nFor 3) Lys is basic and Leu is hydrophobic.\nFor 4) Trp is large (the largest) and Ala is small (2nd smallest) even though they are both hydrophobic.\n\nThe main categories for amino acids are acidic, basic, hydrophobic and hydrophilic.  Any change within a category is fairly conservative as long as the size doesn't change too much.\n\nFor structures and categories, see:  http://en.wikipedia.org/wiki/Amino_acids
1118024
Acidic \n\nbelow 6 acidic above 7 basic
901233
MSDS for Monosodium glutamate (not glutimate)\n\nC5H8NO4Na
984099
I'm very surprised your book doesn't have information on VSEPR.  The acronym "VSEPR" stands for "valence shell electron pair repulsion".  Please double-check the list of topics in the back of your text.  \n\nA dipole moment in the context that you're considering is an incomplete sharing of electrons. In a covalent bond, one of the atoms involved is better at attracting & holding electrons than the other (more electronegative), so that instead of the covalent bond being perfectly shared it gets distorted to one side.  If a molecule has a dipole moment, it has more electrons (higher electron density) in one direction than in others.  One example of this is the covalently bonded acid, H-Cl.  Hydrogen is not very electronegative, but chlorine is very electronegative, so the chlorine atom does a better job holding onto the two shared electrons in the H-Cl bond.  \n\nI hope this gets you started in the right direction.  If you really can't find the info in your text, please go to a library and look at another chemistry book.
877634
Any acid, for example:\n\nHCl + H2O  --> Cl- + H3O+
829401
Basically, water in pure water the water molecules will undergo autoionisation which will produce to types of ions namely H+ and OH- ions. Anyway it is a reversible reaction where H2O exist in equilibrium with H+ and OH- ions. \n\nWhen a strong acid is dissolved in water, it will disscociate completely to produce H+ ions and the anions. This is a forward and non-reversible reaction. Whereas when a weak acid is dissolve in water only part of it will dissociate and the degree of dissociation depends on is solubility constant. This is a reversible reaction.\n\nWhen an acid is mix with water both the acid and the water will contribute its proton. ( acid dissociate completely and water partially.) But the proton from water is so little and can be neglected so normally the concentration of the H+ ions of the acid is used for calculation.\n\nHope this helps.... Good luck..