95=t of ml. WAHT DOSE IT MEAN???
154995
95 tons of mililiters
265173
You are correct using the formula:\n\nC1*V1 = C2 * V2\n\nwhere C is the concentration and V is the volume.\n\n\nNow, you know that you want a concentration of 0.39M solution of NaCl in a 100 ml sample.\n\nSo, the equation should read:\n\n0.82 * V1 = 0.39 * .1 L\n\n0.82*V1 = 0.039\n\nV1 = .047L\n\nso, take 47 ml of the .82M NaCl and dilute it up to 100 mL.  That will give you the 0.39 M NaCl.
74467
The solution has a density of 1.0 g per millilter, and it is a 0.1% concentration of Thimerosal.  So, the thimerosal has a concentration of 0.1% x 1.0g/mL, which is 1 mg/mL.\n\na) 0.5g of solution / 1.0 g/mL = 0.5 mL of solution\n0.5mL x 1.0mg/mL = 0.5 mg of thimerosal\n\nb) 50g of solution / 1.0 g/mL = 50 mL of solution\n50mL x 1.0mg/mL = 50 mg of thimerosal\n\nc) 25g of water / 1.0 g/mL = 25 mL of solution\n25mL x 1.0mg/mL = 25 mg of thimerosal\n\nd) 75mL x 1.0mg/mL = 75 mg of thimerosal\n\ne) 0.75g / 1.0mg/mL = 750 mg of solution\n750 mg / 1.0 mg/mL = 750 mL of solution
741771
0.5M = 500mM\nv x c=v'xc'\nv x 500 = 50 x 1\n0.1mL of the 0.5M solution diluted to 50mL will be 1mM
713107
range/amount\n\nrange = 120 mV (90mv - (-30mV))\namount = 2^16 = 64*1024\n\nplug-n-chug
214560
It has to do with the type of liquid you are using. For water it is 1000 Milligrams=1 C.C.\n\nC.C. is a way to measure volume. For example: the C.C.'s of 1 mg of cotton is more than that of 1 mg of gold.
711363
The volume will be 549.5 mL.  Let me know if you want to see the work.   Use this equation PV/T=P*V*/T*.    P,V, and T are just the pressure, volume, and temperature for the initial system (they are usually represented as P1,V1, and T1 but I left out the numbers which should be subscripts for simpliofication because yahoo does not have many text options.)  P*,V*, AND T* are the pressure, volume, and temperature after the system has been changed.  You could use any units pretty much for the pressure and volume as long as you keep the units consistent.  However always use Kelvin for the temperature.  Kelvin = 273 + Celcius Temp.
532149
I don't know if this is right ... but check it and tell me\n\nV*C KOH = V*C HBr\n\nV KOH = 18.6ml C KOH = 0.752M\nV HBr = 22.1ml C HBr = ?\n\n18.6*0.752 = 22.1*C HBr\n\nC HBr = 0.6329M\nIts seems reasonable cause the difference between concentrations isn't significant
976160
the number of moles in the 1 L  bulb is using pV=nRT\n\nn1 = pV /nR  = 649 *1 /RT = 649/RT\n\nfor the 0.5 L  we obtain n2 = 445 * 0.5/RT= 222.5/RT \n\nn1+n2 = 871/RT  which is put in a total volume of 1.5 l\n\nSo, the pression is  871/1.5 = 581.2 mm Hg\n\nNote that with my answer, you need not to know neiter the temperature nor to convert the pression in mmHg in pascals or atmospheres
564420
.1ml of 100:1 dilution had 280\n1.0 ml of dilution has 2800\n1.0 ml of undiluted has 280,000
726441
4.74 / 300 = 0.0158 g/ml\nin 35 ml\n0.0158 * 35 = 0.553 g\nDividing by 40 g/mol (MW) we get\n0.553 / 40 = 0.0138 mol in 100 ml\nSo in 1000 ml the number of moles will be 0.138\nThe molarity is then 0.138 M.
328014
1 ml = 1 cc\n1 ml = 15-16 gtts (drops)
748321
You're kidding right? \n\n1L (1000ml/ 1L) x (0.5g/1ml) = 500g
939108
Given:\nPV = nRT, 862 torr x (1 bar/750torr) = 1.15 bar, 117 C +273 = 390 K, CH4 = 16 g/mol\n\nn/V = P/(RT)\n\nn/V = (1.15bar)/[(0.08315 L bar/K mol)x(390K)\nn/V = 0.035 mol/L x (16 g/mol) x (1L/1000mL)x(1mL/1cm^3)\ng/cm^3 = 5.67 x 10^-4 g/cm^3
703531
FW of NaCl is 58.44  then\n\n   58.44 gm in 1000 mL = 1 Molar\n\n   4.78  gm in 200 mL = ?\n\ndo cross multiplication\n\n(4.78 gm x 1000 mL x 1 M) / (58.44 gm x 200 mL) = 0.4089 M\n\n(gm/gm and mL/mL cacels out so you get answer in M)\n\n\nNow you are taking 28 mL of 0.4089 M solution and diluting it to make final volume of 100.  Use M1V1 = M2V2\n\n0.4089 M x 28 mL = ? x 100 mL\n\n\nThen  ? = (0.4089 M x 28 mL) / 100 mL    { mL/mL cancels out and you get answer in Molarity)\n\n\n? = 0.1145 Molar is your answer
1187434
I think that's dalton's law.  Whoever came up with it, the pressure is additive.  So convert so everything is in the same units, multiply by the percent, add, and then compare to the answers.  I bet it's more fun than you predict.  Whooo!  Conversion factors!  I don't want to take that kind of enjoyment away, so get cracking!
808549
M=molesof solute/Liter of solution\n\nM= molarity