Water Molecules in one drop?
929435
a drop of water weights  about  0.05 g \n\nThe molecular weight of water is 18 (H2 o = 2*1+16)\n\nso the number of moles of water in a drop is  0.05/18 =1.67 10^21 molecules
1141302
The molecular mass of water is 18.0153 g/mol, and the density of water is\n997.07 g/L at 25 C.  That makes\n\n(997.07 g/L)(mol/18.0153 g) =  55.346 mol/L.
761477
Actually you have an electrolyte, so the drop in the freezing point  is\n\nΔT=i*Kf*m\n\nwhere i is the van't Hoff coefficient and (for simplicity) for strong electrolytes it is equal to the number of ions that are produced by its dissociation, according to the molecular formula.\nNaCl dissociates completely to two ions (Na+ and Cl-) thus i=2\n\nfor water Kf=1.86\n\nm is the molaLity and not molaRity. \nYour solution is 2 M = 2mole solute/L of solution \nmolality is mole solute/kg of solvent. You need additional info in order to convert molarity to molality\n\nIf you had 2 molaL and not molaR solution then m=2, or if we assume due to lack of more info that in this case molaRity=molaLity...\n\nΔT=i*Kf*m =2*1.86*2 = 7.44\n For pure water Tfwater=0 C, so for the solution \nTf= Twater-ΔT= 0-7.44= -7.44 C
1036867
Of course ice and water are chemically identical consisting of H2O.  The two hydrogen atoms attach to the oxygen atom other than in a straight line (not like beads on a string).  The electron field surrounding the water molecule is uneven providing it with a "polarity" that makes it much easier to pack many molecules together in a given (rather than arbitrary) arrangement.  When water is a vapor (or steam) there is so much vibrational energy that the molecules bounce off each other maintaining a "pressure" depending on their energy (temperature).  When the molecules are a liquid, they are very closely packed and are nearly incompressible (even seven miles below the surface of the ocean!).  The bulk water expands and contracts only a little with temperature changes.  When heat is removed from the water (in a freezer?) the molecules are attracted to each other in a preferred array due to polarity and form long chains of molecules that use up space far less efficiently.  The "ice" is less dense and floats on water because the space between chains is filled with a vacuum or gases that weigh very little.  When the water is allowed to freeze in open space (a cloud?) the polarity is free to align water molecules in the most preferred orientation; a six sided snow flake.  When hoar frost forms on a cold window pane the ice forms in dendrites, like growing Christmas trees.  Hope that helps a little.
1014427
A liter is the quantity of liquid that will fit in a 10 cm x 10 cm x 10 cm cube.  A milliliter would be the size of a 1 cm x 1 cm x 1 cm cube.\n\nAccording to this source, one drop of water is .0251 ml.  So it would take 40 drops to make a milliliter.
328014
1 ml = 1 cc\n1 ml = 15-16 gtts (drops)
325448
for one molecule of H2O, there will be one molecule of H2 and one molecule of O.\n\nfor one molecule of H2O, there will be two atoms of H and one atom of O.
432258
Since it is at thermal equilibrium, the energy (q) of the water must equal the energy (q) of the metal.\n\nTherefore: mcAT = mcAT\n\n(90)(4.18)(0.9) = (11)(87.2)(c)\n\nSolving for c, the specific heat of the metal would be 0.353 J/g*oC
291231
H2O...two parts hydrogen and 1 part oxygen in each of the water molecules.
537207
The vapour density and molecular weight relations is given by \n\n2 x VD = Mol. Wt\n\nThe normal vapour density of Air is taken as 14.4. That is 28.8 is the average molecular weight. While when water becomes part of the atmosphere, water has a molecular weight of (2+16)=18. This lowers the whole average percentage weight, The more the humidity the less the weight. There the density decreases as it is the weight per unit volume.\n\n\nPlease make it the best answer
741504
Vapor Pressure of Solutions\n\nA. \n\nAmount of the sugar present = 10.0g/ (342) = 0.0292397661 mol\nAmount of water present = 200g/ (18) = 11.11111111 mol\nThus, X(H2O), which signifies the fraction of water present,\n= 11.11111111/ (11.11111111 + 0.0292397661)\n= 0.9973753281\nAt 25 deg Celsius,\nVapor Pressure of Water is then = 0.9973753281 x 23.8\n                                                      = 23.73753281 Torr.\n\n\nB.\n\nAmount of Calcium Chloride = 49.4g/ (40.1) = 1.2319202 mol\nAmount of water = 150g/ (18) = 8.333333333 mol\nThus, X(H2O), which signifies the fraction of water present,\n= 8.333333333/ (8.333333333 + 1.2319202 )\n= 0.8712088294\nVapor Pressure of Water is then = 0.8712088294 x 23.8\n                                                      = 20.73477014 Torr.\n\n\nFREEZING POINT DEPRESSION/BOILING POINT ELEVATION OF SOLUTIONS\n\nA - NOTE: T(f) signifies T with the small f at its bottom right. Similarly, b(f) is an 'f' with a small f at its bottom right.\n\ndT(f) = change in freezing point\n\nChange in dT(f) = 5.48 - 3.77 = 1.71\nTherefore, from {c}\nb(f), which signifies the molality,\n= 1.71/ 5.12 = 0.333984375\n\nSince molality = (Amount of solute added)/ (mass of solvent/ kg),\n\nAmount of solute added = [500 x 10^(-3)]x(0.333984375)\n                                        = 0.1669921875mol\n\nThus, Mr of the unknown compound is 20.0/ (0.1669921875)\n= 119.7660819\n\nB\n\nChange in T(b) = (0.51) x {54.6/ [0.997x400x10^(-3)]}\n                         = 69.82447342\nsince  dT(f) = K x b(f) and\nmolality = (Amount of solute added)/ (mass of solvent/ kg).\n\nI am afraid I do not know how to proceed from here for I am not sure of the method to find the normal boiling point of a solution.
849763
Water vapor.\n2 H2 + O2 = 2 H2O
1080141
"what element(s) and what bond(s) make water a universal solvent?"
866201
water itself, of course.\nThe following ions.....\niron ions, calcium ions, sodium ions, chloride ions, fluoride ions...\n\noxygen molecules, carbon dioxide molecules, sometimes around here hydrogen sulfide molecules.\n\nALMOST EVERYTHING is in water in minute concentrations.
153248
The molecules of water do not actually "change."  They vibrate faster as they get warmer.  If they are vibrating slowly enough, the molecules are packed closely together into the solid form of water we call ice.  As they move faster they become the liquid state we commonly call water.  When they are vibrating fast enough they "evaporate" into the gaseous state.  \nIn any of these 3 states they are still molecules of water, they are just moving around at different speeds.
271556
In addition to the fact that at 4 degrees celcius, water has an absolute density of EXACTLY 1 g/cc, at 0 degrees, it is in equilibrium with its solid phase (ice) which has a density of LESS than 1 g/cc due to its open cage like crystal structure. So, its exact density at 0 degrees is impossible to standardise.
955333
an easy example you can remember is H2O(water).\nif u want a more difficult one, u can use CH3COOH(acetic acid)!\n\nALL DE BEST!