Milliliters in a titration?
953411
30.2 mL\n\n(4.93g Al(OH)3 / 78 g/mol)x3 = .1896 moles OH\n\n.250 L x 2.00 M HCl = .2500 moles H\n\ntherefore this is .2500 - .1896 = .0604 mole H extra.\n\n2.00 M / .0604 mole = 0.0302 L = 30.2 mL
946830
Just remember M1*V1=M2*V2 where M is molarity and V is volume. A little Algebraic manipulation gives you:\n\nV1 = (M2*V2)/M1\n     = (0.195*15.5)/18.0\n     = 0.168 L = 168 mL
683322
Well, I suppose 1.25 g is 1250 mg, so seeing there's 1250 mg in each ml of solution, taking out 0.2 ml of the solution will net you 250 mg of the substance.
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.
435050
Well... A titration is a method to know an unknown concentration of a given solution.\nIf you need to know a NaOH solution concentration, you should do the following:\n1. Measure 20 ml of NaOH.\n2. Drop some drops of phenolphtalein (10 should do, no more)\n3. The solution will go pink with this drops of phenolphtalein...\n4. Using a burette (it's a graduated tube to know how much of a given substance you are pouring), drop some HCl (you should have this in your laboratory) measuring it till the solution of NaOH is clear again.\n5. Solve this equation: V(HCl) x N(HCl) = V(NaOH) x N(NaOH)... V(HCl) it's the volume you used to turn the solution clear again. The N(HCl) it's the concentration of that HCl (Chloridric Acid) given in equivalents/litre. V(NaOH) is 20 ml, the one you used at the begining... You have to calculate N(NaOH), and that's it =)\nHope you find it useful! ^^
773889
Suspected trick question.  The volumes included are irrelevant.  You know the molecular weight (66000 Da) and you know how many micromoles you need total in each solution.  What does it matter if the one micromole is in 1 ml or 10K gallons?  You know it only contains one micromole.  Divide the molecular weight by 10^6 and you're done.  (or you have not stated the problem correctly)
241919
It kind of depends on what you are starting with but lets say that you have a solution of drug containing a concentration of 20 milligrams per milliliter and you are running it at 2 milliliters per hour.  You need to multiply it out to convert the units.  If you are starting with 20 mg/mL at 2 mL/hour, first you convert hours to minutes and then you convert mg to micrograms.  The mL cancel, the mg cancel, the hours cancel, and the units you are left with are micrograms per minute!\n\n__20 mg___  x   __2 mL___  x  ___1 hour___ x _1000 mcg__ =\n1 mL             1 hour         60 minutes    1 mg\n\nThere are other ways to do it, but I find this the easiest.  If you need to figure out mcg/kg/minute, you just divide the last number by the patient's weight.
784999
.15 M solution of NaCl means .15 moles of NaCl (solute) in 1000g of water (solvent).\ntherefore, to make 250 ml (or g) solution [ as density of H2O is 1]\nmoles of NaCl required = .15/4 = .0375 moles \n& moles = given wt * molecular wt \nso, given wt (or required wt in this case)= moles/ molecular wt. = .0375/58.1 = 645.4388 * 10^-6 g
748321
You're kidding right? \n\n1L (1000ml/ 1L) x (0.5g/1ml) = 500g
93233
any time you see the prefix mili, it means 1/1000.  So there are 1000 mililiters in a liter.
646163
Presuming that the base is monobasic.\n\na) with 25 ml added, you are at the equivalence point.  The pH is 7.\nb) after adding 25.01 ml, you will have 0.01 ml of base that did not get reacted.  The molarity of the base in solution will then be 0.1 * (0.01/50.01) = 2.0 x 10^-5.  Your pOH is 4.70, pH would be 9.30\nc) Now, it's 0.1 ml of unreacted base.  Molarity is 0.1 * (0.1/50.1) = 2.0 x 10^-4.  Your pOH is 3.70, pH is 10.30.\nd) Now 1 ml of unreacted base.  Molarity is 0.1 * (1/51) = 2.0 x 10^-3.  pOH is 2.70, pH is 11.30.\ne) Now 25 ml of unreacted base.  Molarity is 0.1 * (25/75) = 3.33 x 10^-2.  pOH is 1.48, pH is 12.52.\n\nIn each case, you have to figure out the amount of unreacted titrant and recalculate the molarity as if you were simply diluting it, using McVc = MdVd, where the volume is now the total volume of the solution (the unreacted amount plus the 25 ml of acid and the 25 ml of base that have neutralized each other).
163778
If you're talking about water, 1 liter water= 1 kg so 1 milligram=1 milliliter . But if you're talking in general, you can't compare them, because milliliter measures volume, and milligram meausures weight. Good luck :)
644701
Summary: convert your concentration to a mole, mass, or volume fraction and multiply by 1 million.\n\nDiscussion:\nParts per million must be measured in consistent units:\n\nmass per 1 million mass units\nvolume per 1 million volume units\nmoles per 1 million mole units\n\nFor example, if you add 1 milligram of substance to 1 kilogram of solution, the concentration is:\n\n1 mg/1 kg = 0.001 g / 1000g = 1e-6\nMultiply the resulting mass ratio by 1 million and you convert this to ppm\n1e-6*1million = 1 ppm\n\nI don't think it is correct to directly use molarity or molality times 1 million, since both of these are ammount/volume: the units are not consistent.  You have to convert the "volume" in the concentration to a "mass" or "molar" amount consistent with the concentration measurement.\n\nIf you have a concentration in terms of a mole fraction, it is just the mole fraction times 1 million.  A mole fraction of unity (one) is the same as 1 part per part (pure!).\n\nIf you have a concentration in terms of a volume fraction or mass fraction, you just multiply by a million.  It is important to note that whether you do parts by mole, volume, or mass you will get different numbers for a given system.  It is important to be clear which one you are talking about.  You can read more on wikipedia, look up ppm.
862256
Going from 10^12 cells/mL to 10^10 is a 1:100 dilution.\nIf you want a final of 2mL, you need to add 20uL of your stock solution.\nSo do 20uL of stock (10^12)+ 1980uL of salt solution = 2000uL (10^10), which is the same as 2mL.
837288
Use the formula M1V1=M2V2\n\nThat is the first Molarity times the first volume are equal to the second Molarity times the second Voume.\n\n.2098M x70mL = .662M x V2\n\nSolve for V2.\n\n(.2098 X 70)/.622 = V2\n\nV2 = 23.61mL NaOH to titrate the solution to neutrality.
559540
the formula M=moles/L\n first convert mL into L\n(500)(10^-3) = .5L\nM= .50moles/.5L =  1M
973272
ok, first go to moles.\n\n24.0g LiOH (1mol/23.948g) = 1.0022mol\n\nnow get liters using molarity\n\n1.0022mol (1L/0.153mol) = 6.55L or 6,550mL \n\nRight, there ya go, remember that you have 3 sig.figs. so you may want to represent significance by using scientific notation. So...\n6.55x10^3mL\n\nIf you're ever stuck, just simply go to moles and that will get you started (and usually gets you some points on tests).