SPECiFIC GRAVITY OF 60% SULFURIC ACID?
26943
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786996
This is a tricky question. Perhaps reading: http://www.newton.dep.anl.gov/askasci/chem03/chem03067.htm will help.
611049
pervious answer is incorrent.\n\nThere are 0.1 moles of H30+ ions in the solution as once sulphuric acid has dissociated once it creates the rather stable conjugate base HSO4+ which is what makes sulphuric acid "strong".  This ion has a very small pK value, and is to all purposes not dissociated.  Reaction of the solution with a base will encourage it to dissociate tho.
864563
In part, specific gravity can be measured with a hydrometer.  You establish a range that the liquid displaces and let it bob until it comes to equalibrium.  This test can be measured at any temperature.  \n\nHowever, mass density is done in a container that is kept at a constant temprature.  The math is easy once the measurments are taken, but there is more time involved in setting up the test and bringing the whole thing to equalibrum
1072394
The listed percentage of vinegar is almost always "by weight" and not volume.\n10% vinegar means that 10% of the weight of the vinegar is acetic acid, the other 90% is water.\n\nTo calculate the molality, we need to figure out how many moles of a solute (acetic acid) is dissolved in the solvent (water).\nWe need also calculate the volume of the solution (in liters).\n\nTo solve this, take (for example) a 100 gram sample of 10% acetic acid, this would mean that 10 grams out of 100 are acetic acid.  Knowing the molar mass of acetic acid (60.05 g/mol) we can calculate the number of moles of acetic acid present.\n10 g / 60.05 g/mol = .1665 moles\n\nA 10% acetic acid solution has a density very close to that of water, so it is not unreasonable to just assume a density of 1 g/cm^3 (if you want a more accurate answer, look up the density your self).  If we assume the density is 1 g/cc, then 100 grams of 10% vinegar would have a volume of 100 mL, or .1 Liters.\n\nWe now know the number of moles of solute and number of Liters of solution, we can calculate molarity.\nM = moles / Liter\nM = .1665 moles / .1 Liter\nM = 1.665 Molar
457644
It does indeed have a higher specific gravity than fresh water.\n\nPure water has a specific gravity of 1000 kilograms per cubic meter\n\nSea water (in general) has a higher specific gravity, on average it is around 1026 kilograms per cubic meter
861217
molarity = moles/L\nso just plug in what you have!  6.3M= mol/0.216 L   just multiple 6.3 by 0.216 and you will get the moles of the acid (i dnt have a calculator on me right now, but just do the calc out and theres ur answer! ) :)
933864
to what?  Are you looking for the molecular weight of the monoprotic acid?  If so, remember M (molarity) is in moles/lter) and your colume of NaOH is in mL so you'ww want to convert that to liters.\n\n\n.01524 liters x .1578 moles/liter = 0.002405 moles\n\nso therefore you have 3.567  g / 0.002405 moles = 1483 gram/mole\n\nuse dimensional analysis and keep track pf the units to find the answer
976396
1 G, I dont see how it can be zero otherwise it would float off!\n\nOK call me an idiot...I have just read the other answers lol
911230
http://www.neis.com/chemnames/s/Sulfuric_Acid.html
127716
based on the given balances equation.\n\nthe volumes could be:\n  \nSTP = 22.4L per mole\n\n 14.2L SO2 ( 1 mol H2S / 2 mol SO2) = 7.01 L of H2S\n\n and\n \n14.2L SO2 (3 mol O2 / 2 mol SO2 )  =  21.3 L of O2
377356
Surface gravity of sun: 273.95 m s-2 (27.9 g)
455269
H2SO4 + Mg(OH)2 -> 2H2O + MgSO4
529624
its dilute h2so4 (38%) sulphuric acid.
781338
The density is 0.357 g/mL. This is because specific gravity is the ratio of the density of the unknown liquid to the density of water, 1.0 g/mL.\n\nIf, say, you wanted to know the density of the liquid in pounds per gallon, you would multiply 0.357 by the density of water, which is 8.320 lb/gal
939750
W=mg ... where g is the gravitational acceleration
251863
At 20 degrees C, it's 0.6g/100mL. You can convert that to a Ksp.