Want this question answered?
The molarity is 2 mol/L.
20.2 g of CuCl2 = .1502 mol CuCl2 M=mol/L M=.1502 mol/L
The formula mass of (anhydrous) CaCl2 is: 110,99 g/mol;as dihydrate CaCl2.2H2O it is: 147,01 g/mol
Manganese dioxide is insoluble in water.
3mol/0.5L
2 m is the molarity of a solution that has 6 mol of CaCl2 in 3 km of water.
2m
The molarity is 2 mol/L.
2 m
You'll need: 0.450 (L) * 25 (mol/L) = 11.25 mol CaCl2 and add water to it up to 450 mL.To be weighted:11.25 (mol CaCl2) * [40.08 + 2*35.45](g/mol CaCl2) = 1491.736 g = 1500 g =1.5 kg CaCl2 (CaCl2 as dry substance!, not hydrated)
20.2 g of CuCl2 = .1502 mol CuCl2 M=mol/L M=.1502 mol/L
2.0 mol of CaCl2 releases 2.0 mol of Ca+2 ions & 4.0 mol of Cl- ions = 6 moles of ions find molality: 6 moles / 0.800 kg water = 7.5 molal solution dT = kf (molality) dT = 1.86 C (7.5m) dT = 14 Celsius drop in freezing temp the new freezing point is - 14 C
Ca-1(40.08)g=40.8g/mol of Ca Cl-2(35.45)g=70.9g/mol of Cl2 40.08g+70.9g=110.98g/mol CaCl2 110.98g CaCl2/1mol * 1.9mol =210.86 g of CaCl2
0.89 moles of CaCl2 is equal to 98.8g.
Ok, lets begin by writing out the reaction : 2AgNO3 +CaCl2 --> 2AgCl(s) + Ca(NO3)2 Precipitate = AgCl Now find the mol of compound in each solution: 14g AgNO3 x (mol/170g) = .082mol 4.83g CaCl2 x (mol/111g) = .044mol Determine limiting reactant: Notice in reaction that 2 CaCl2 molecules react with 1 AgNO3. Because 2(.044mol) > 1(.082mol), AgNO3 is your limiting reactant. Now that you know this you can find the mass of the precipitate .082molAgNO3x (2molAgCl/2molAgNO3)x(143.3g/molAgCl) = 11.75g b) Assuming all the AgNO3 is exhausted, there will be 2(.044)-(.082) = .006mol CaCl2 left .006mol x (111g/mol) = 0.67g CaCl2
The formula mass of (anhydrous) CaCl2 is: 110,99 g/mol;as dihydrate CaCl2.2H2O it is: 147,01 g/mol
Molarity is probably the most commonly used unit of concentration. It is the number of moles of solute per liter of solution (not necessarily the same as the volume of solvent!). Example: What is the molarity of a solution made when water is added to 11 g CaCl2 to make 100 mL of solution? Solution: 11 g CaCl2 / (110 g CaCl2 / mol CaCl2) = 0.10 mol CaCl2 100 mL x 1 L / 1000 mL = 0.10 L molarity = 0.10 mol / 0.10 L molarity = 1.0 M http://chemistry.about.com/od/lecturenotesl3/a/concentration.htm http://www.tpub.com/content/MIL-SPEC/MIL-P/MIL-P-71158/MIL-P-7115800013.htm http://www.tpub.com/content/armymedical/md0837/md08370139.htm