What is the best pH for lime coagulant?
409381
i suppose it's around 10-11, as it is used to neutralise the acidity in water.
963001
First of all you should give us more info, like what exactly is the elimination test, concentrations, conditions and if you know the pH of the final solution or the final concentration of acetic acid.\n\nA very rough explanation based on the limited info, would be that HF is a much stronger acid than HPO4-2, so in an acidic environment it manages to dissociate much better, giving the conjugate base or if you prefer the conjugate base F- is much weaker than PO4-3 so PO4-3 will steal away the H+ from the acetic acid. Thus it is possible that in the acidified medium you have most of the phosphate in the form of HPO4-2, and the concentration of PO4-3 is too low to lead to precipitation.\nOn the other hand, although CaF2 is much more soluble, most of F- will remain as such and thus its concentration might be high enough to promote precipitation.
642853
The pH can vary widly depending on the type of electroplating.  The nitrates will be the species associated with the metals used and of course sodium.\nCan you be more specific on which proceses you are looking at  See \n\nhttp://es.epa.gov/techinfo/facts/metalmfg.html\n\nhttp://es.epa.gov/cooperative/topics/metfactsheets.html\n\nhttp://www.epa.gov/ttn/chief/ap42/ch12/final/c12s20.pdf
857742
Any acid.  Vinegar is the best probably.
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.
780228
HCL and NaOH are 'strong' acid and base. When they react, the product is neutral. NaOH + HCL --> NaCl + H2O\n\nWhat you need to find is which is the limiting reactant, the other one (what is left over) will effect the pH by its concentration in the otherwise neutral solution.\n\nFor your first problem:\n\n0.0557M HCL = 0.0557mols/liter*0.00542L = 3.02*10^(-4)mol HCL\n\n0.0377M NaOH = 0.0377mols/liter*0.00337L = 1.27*10^(-4)mol NaOH\n\n3.02*10^(-4)mol HCL - 1.27*10^(-4)mol NaOH = 1.75*10^(-4)mols HCL\n\n0.00542L + 0.00337L = .00879L\n\n[(1.75*10^(-4)mols HCL) * (1 L) ] / (.00879L) = .020M HCL\n\npH = -log(.02) = 1.70
625417
pH= -log(6.0 x10^-3)\npH is about 2.22
944314
The pH scale goes from 1-14, with 1 being the most acidic, 14 being the most basic, and 7 being neutral. \n\nSince a pH of 9 is closer to neutral than extremely basic (pH = 14), I would call the window cleaner weakly basic.
282642
actually, pure water does not have a pH of 7.0, it is slightly acidic, around 5.6-5.8 from what i have seen at work.
382713
The best method is pH meter (other than color indicator). \nTo measur the exact end point, what you have to is:\n\nStart the titration\nInsert a pH probe inside the solution\nNow start adding base to the acid and swirl the solution properly\nKeep track of your pH readings..\nYou will see a sudden jump (some thing like from 5.6 to 9.0 even with one drop addition)\nthats end point.
702231
Vinegar's pH is between 2-3.
131291
To maintain the pH of the pool between 7.2 and 7.8, sodium carbonate (soda ash) is used to raise pH and sodium bisulfate or hydrochloric acid (muriatic acid) can be used to lower it.
836016
Here is a good guide\n\nhttp://dbhs.wvusd.k12.ca.us/webdocs/Stoichiometry/Limiting-Reagent.html
682738
There is a product made by HTH called pH Minus. (I'm sure there are other company's that make it as well), it's fairly inexpensive, around $14.00 for 1/2 gal. Just follow the directions and your water will be back to normal in no time at all. It works quickly! GOOD LUCK!
875212
Since HCl and NaOH are both strong solutions (acid and base, respectively), you know the pH is going to be 7.0.
1093978
Take a look at your sludge under a microscope. If the bacteria create too long fibres, the sludge will capture gas bubbles and refuse to sink even with strong coagulating agents. \n\nYou might have to restart the biological stage of your treatment plant with a new culture. Check with your service specialists first, though.
600985
According to the Henderson-Hasselbalch equation,\n\npH = pKa + log [A-]/[HA]\n\nSo, when pH = pKa, then [A-] = [HA]\n\nA buffer has is a mixture of undissociated acid and the products of dissocation.  With the concentrations equal, there is the maximum number of ions to react with to changes in pH.