Chemistry question about aqueous solutions?
812718
A\n\nThe pOH of a solution is the negative log of the concentration of OH ions.  THis would be 9 in this case.  The pOH is the opposite of pH.  The scale is from 0 - 14.  The lower the pOH, the more basic the solution is.  pOH of 7 is neutral.  Lower than 7 is basic and higher than 7 is acidic.  If the pOH of a solution is 9,  the pH of the solution is 5.  The pOH and the pH should add up to be 14.  I hope this helps.
983710
H2SO4 will dehydrate and remove water.\n\n\n(CH3)2 CH - CH2-CH=CH-(CH3)2
238675
If the reactants are in aqueous solution, in high enough concentrations, then solid silver chloride (AgCl) will precipitate. Sodium nitrate wiill remain in solution as sodium and nitrate ions. No chloride ions should remain - they will all have reacted with the silver ions.\n\ni.e.   AgNO3 + NaCl  + NaNO3   ->    AgCl  +   NaNO3\n\nDon't forget to balance the equation.
211023
wow, well put mrjeffy! I have one thing to add though. Because all acids and bases are electrolytes, you can use pH to determine what is and isn't an electrolyte in a solution. If it come out as acidic or basic, it is and electrolyte(the darker, the more basic or acidic). If it comes out neutral, like Distilled Water, it is not. Also don't forget that non-electrolytes will not completely dissolve into solution in water.
429768
To perform a solution-based separation, you need a solvent in which one or some of the solutes (in the mixture to be separated) is/are highly soluble, and in which the other components are highly insoluble.\n\nA simple example might be separating an ethanol/pentane mixture by using water.  Ethanol, being polar, will readily dissolve in water; but the nonpolar pentane will not.
921966
Br2 is extremely soluble in CCl4 - much more soluble than in water.\nLook up "partition".
516306
Until the concentration of salt is large enough to form a saturated solution, ie. one in which no more solute will dissolve, the volume of the solvent (water) will not change.  20g of salt is not nearly enough to form a saturated solution, so the water level will remain at 500ml.
851560
solution...Bicarbonate and sodium. :)
706351
KCl(aq) + AgNO3(aq)  --> KNO3(aq) + AgCl(s)\n\nNet ionic: Cl-(aq) + Ag+(aq)  --> AgCl(s)\n\nNa2SO4(aq) + Ba(NO3)2  --> 2NaNO3(aq) + BaSO4(s)\n\nnet ionic: SO4(-2)(aq) + Ba(+2)(aq)  --> BaSO4(s)
1186593
Mix with a 0% solution in the relation 33:2\n\nSo use 2 units of your solution (like 2 liters) and 33 units of the 0% solution (like 33 liters).\n\nThat's all.
55041
Fresh water evaporates faster than the solutions will.  Between the solutions it would depend on the number of particles dissolved in the water.
45025
It is a chemical that you keep at all times.  In a typical lab that would include acid, bases, certain organic solvents, etc.  You will also hear stock solutions which are solutions of these chemicals.  Do not confuse these with standard solutions which are solutions where the concentration is exactly known.
897586
X2O\n\nExamples:\nH2O => Water
838309
b a solution, the salt will dissolve
395302
mixture is combining substances, solution is dissolving a substance in another
611075
I'm assuming you are extracting from an aqueous solvent?  Preferably, you want to increase the polarity of the aqueous solution, such that the solute has less affinity for water than it would for the organic solvent.  This can be done by "salting" the water (increasing the ionic strength by adding an inert salt, a la NaCl).  You then extract the solute with your organic solvent of choice, usually using smaller aliqouts more frequently vs. larger aliqouts (deals with partition coefficient, or how much will get extracted vs. how much remains in the water).  After extraction, the organic solution is usually dried (more often than not by MgSO4 or Na2SO4) and then the solvent is distilled off to yield hopefully pure product.
261798
The aqueous solubility of AgNO3 at 20C is 67.8 (solubility is 100*m2/(m1+m2) where m2 = mass of solute and m1 = mass of solvent).\n\nRearraging the equation gives us m2 = (m1*67.8/100)/(1-67.8/100).  or\nm2 = (m1*.678)/(1-.678) = 210.56g of AgNO3 @ 20C\n\nAt 50C the aqueous solubility of AgNO3 is 79.2 so\nm2 = (m1*.792)/(1-.792) = 380.77g of AgNO3 @ 50C\n\nTo find the amount needed to make the second solution saturated we must subtract answer 1 from answer 2.\n\nWe find that 170.21g of AgNO3 must be added to make the solution saturated at 50C.