what are the essential factors affecting the buffering capacity of a buffer solution?
493490
Buffer capacity is defined as the moles of acid or base necessary to change the pH of one liter of solution by one unit.\n\nBuffer Capacity = (number of moles of OH- or H3O+ added)     divided by ( pH change) x (volume of buffer in L)\n\n-Buffering capacity increases as the molar concentration (molarity)of the buffer salt/acid solution increases.\nThat's only partially true.The pH of a buffer solution is independent of buffer concentration only if there is a sufficient quantity present. A buffer consists of a solution of a weak acid (base) and the salt of weak acid (base). The addition of either acid or base converts acid(base) to the acid (base) salt, or the salt back to acid (base) when another acid or base is added to the solution.If there is not enough buffer present compared to the added acid or base, the buffer can be swamped, and the pH will change significantly. So it is only partially true that the buffer is independent of the buffer concentration.If the amount of acid or base added, is small compared to the buffer concentration then the pH is not sensitive to the amount of buffer present\n\n-the closer the bufferd pH is to the pKa,the greater the buffering capacity\n\nThe solution is at a maximum buffer capacity (the minimum dpH/dn) when pH = pKa, as can be seen algebraically: \nKa = [H3O+][A-]/[HA]; [H3O+] = Ka[HA]/[A-] \n\nlog [H3O+] = log Ka + log ([HA]/[A-]) \n\npH = pKa - log([HA]/[A-]) \n\nThis rearranged form of the ionization constant of an acid is sometimes called the Henderson-Hasselbalch equation. \n\nSince pH = pKa if and only if [HA] = [A-], maximum buffer capacity of a conjugate acid-base pair is always found at pH = pKa. Reasonable buffer capacity is still obtained if the ratio of [HA] to [A-] is somewhere between 0.1 and 10, but outside this range it decreases rapidly. A chemical buffer can be effective about pH = pKa +/- 1. To make up a buffer solution one would first choose a reasonable acid-base conjugate pair on the basis of its pKa value and any other chemical constraints (one would not use the HCN/CN- pair, for example, in biological systems because cyanide is toxic). One would then adjust the concentrations such that both are reasonable (say 10-3 molar or above) while the desired pH is still obtained. The conjugate acid-base pairs glycinium ion/glycine, hydrogen citrate/citrate, dihydrogen phosphate/monohydrogen phosphate, and boric acid/hydrogen borate are often used for the preparation of aqueous buffers.
1088951
Carbonic Acid is an example of a buffer. It keeps the equilibrium in your blood stream, so that the pH remains around 7.2-7.4. If there are too much acid, it acts as a base to reduce the amounts of acid, and vice versa. \n\nSuppose you injected yourself with sodium hydroxide (why, I don't know), then:\nNaOH + H2CO3 = NaHCO3 + H2O \nBut if you drank HCl instead of H2O:\nHCl + NaHCO3 = NaCl + H2CO3 \n\nObviously, the pH in your mouth is different from that of your stomach, seeing as how stomach acid is HCl. but naturally, without additional acids and bases, they are all roughly the same.
485893
Check on the internet for the ratios used by comercial factories, then prepare a solution from glycol and water in the given proportion. That's all!!!
163386
The time necessary to diffuse H+ ions in the base. Thats it, when u add the necessary amount of acid at once.\n\nUsually when neutralization is carried out the conical flask (or whatever where the base is kept) is kept shaking to increase individual molecular motion. The more motion, the greater chance of H+ ion meeting OH- ion and neutralize each other in a given time interval\n\nH+(aq) + OH-(aq) --> H2O(l)
577726
a BASE is a proton acceptor; an ACID is a proton donator\n\nweak base - has low tendency to accept protons\nweak acid - has low tendency to donate protons - doesn't fully dissociate (reaction stays incomplete, in equilibrium)\n\n\nBuffer solutions are made up of weak acids, so an equilbrium is set up:\n\nHA  <==> H+ + A-\n(HA - acid; H+ - protons; A- - base)\n\nThe pH stays constant because, if an acid (donating H+ ions) is added, the extra A- ions will react with them to form HA. If more base is added, there are plenty of HA molecules to give up the H+ and react with them.  Therefore the amount of H+ ions in solution is constant.  Since pH is a measure of H+ ions in solution, pH stays constant too.
674116
It will depend on the specific resin.  Look up the resin, the capacity is usually given in the technical information.
409824
When what is mixed is not fully disolved into the liquid medium.  It usually settles.  A cenrifuge will not separate out the components that are not part of the solution.
712534
used to change colligative properties of solutions
940690
that would depend on the molarity of the substance. there could be any number of moles in that much solution.
235402
See comment above.\n\nYou do need to do several trials at various concentrations though. You can then determine it through a linear regression.\n\nI also suggest that you consult a book on Analytical chemistry, because Beer's law has limitations. For example, it loses linearity at higher concentrations.
271476
pH = 4.75\n\ntechnically, the pH can be anything.  But, for the most effective acetic acid buffer, the pH would be 4.75 because the pKa of acetic acid is 4.75.  When the pH = pKa, the amount of acid and base are equal, thus its resistant to pH changes is greatest.
707264
Methylamine (CH3NH2) and methylammonium chloride (CH3NH3Cl) would be a good buffer in both are in solution together in appreciable concentrations.\n\nNitrates, chlorides, and sulfates (either as acids or salts) will not act as buffers as those anions have no tendency to act as bases (they are the anions from strong acids, which are "strong" because they dissociate completely in solution).  The same with alkali metal hydroxides, which are strong bases.
768732
pH at pKa +- 1 unit. from henderson hasselbalch\npH = pKa + log [base]/[acid] \ngiving +- 1 when the ratios are 1/10 or 10/1 in concentration\nthe capacity of a buffer is achieved when the ratio of weak acid to conjugate base exceeds 10:1 or vice versa. \nDoes that help?
516770
Depends on conductivity of water which in turn depends on factors such as -- impurities present in water, temperature of water.
56873
The first answer is right on. But remember this as well: enzymes also have some ability to "buffer" the solution they are in as well! Because proteins (enzymes) have many chemical groups that can bind multiple hydrogen groups, its able to buffer to some extent. Generally speaking though, you'd need  a LOT of enzyme to really buffer a solution...so usually we don't worry about it!!
544916
Heat the solvent, then it can take more solute into solution than when it's cool.  Then when you cool it, it is supersaturated.
725588
1. concentration and pressure\n2. see sources