how does the ph of a solution affect the dissolving time of acetominophen??/?
109262
From looking at the structure, it appears that if anything, it would be very slightly acidic, which means that a low pH (more acid) would slow down the dissolving time.  So, to increase dissolving time, add a base.
304287
This is called Base line correction.\nYour solvent may be having some absorption, or the impurities in it may be having some absorption..so to measure your compunds absorption exactly, you need to take the solvent (n whcih you are going to dissolve your compound later) and do this base line correction.\nIn a way you are telling instruments "NOT TO WORRY ABOUT THESE ABSORPTIONS"\n\nThats it\nYou got it?
62986
Molecular compounds do not dissolve in aqueous solution. Ionic compounds do. Sugar does not dissolve readily into water because it is an organic substance. Organic substances do not dissolve easily.
951269
For all practical purposes, if a solution is saturated (can not dissolve any more) it is full and all others will fall to the bottom, undissolved. \n\nRealistically a small (very small) amount of the other powder could dissolve if it had different enough properties.
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
397908
The different acids have a different pH so turn a differetn colour.\nThe concentrations are different. The HCl is more concentrated as it will fully dissociate.
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.
750075
Ask a pharmacist...it would depend on what was in the formula
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.
627599
Ksp is a value dependant on the solute and solvent, (and temperature and pressure), and it determines the molar solubility. It is NOT affected by the amount of solid in the area.  And the solubility formula doesn't have the concentration of solids in it, does it, so that shouldn't be a factor in the amount dissolved.  So, it stays the same.  Does that make sense?  If not modify the question and I'll explain more.
929853
To answer this question I would need to what material you're using (wood, metal or what)  and what are the dissolving tablets (Alka-seltzer or hydrocloric acid). Sorry.
845596
The pH buffers used in a lab experiment can go "bad" at different rates depending on the way they're stored. If your buffer is always stored in a closed container, then the contamination is usually pretty low and the buffer can last for a long time. However if your buffer is constantly exposed to open air and moisture, the pH of your solution can vary quite a bit. I'm not sure if you are familiar with the effect of boiling "tap" water, but boiling the water gets rid of carbonic acid in the solution, similar to the acidity found in a soft drink. So over time, if a buffer is exposed to air, the buffer will tend to become more acidic if no other factors (contamination by other careless people in the lab for example :P) are present. Hope this helps!
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
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.
179057
It's not C.  An increase in pH makes a solution more alkaline, meaning less H+ in the fluids.\n\nI'm going to say A here because a rise in pH is associated with increased O2 binding to hemoglobin.
462489
put one of the acids in the titer, the other in the flask underneath.  Use a magnetic stirrer in the flask to ensure good mixing and ensure that you take required precautions (like goggles gloves lab coat ...possibly in a fume cupboard).\n\nThe two acids don't react with each other but is this 4:1 mix not acqua regia?
766207
The pH of the buffered aspirin is between 8-10.  What is really important is not the pH itself but the pH at which the coating will disoolve.  You do not want the coating to dissolve at low pH in the stomach, but to do that in the relatively higher pH of the intestin where it can be absorbed.