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Q: What is the molarity of a solution that has 6 mol of CaCl2 in 3 kg of water?

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2 m is the molarity of a solution that has 6 mol of CaCl2 in 3 km of water.

molarity is #moles divide by # liters, so 3.0 divided by 0.500 is 6.0 molarity (2 siginficant figures is all you are allowed)

The molarity is 0,75 mol/L.

2m

Molarity of a solution is equal to mol/L.

4 mol/0.800 kg

molarity = moles/litre [solution] = 12 mol/6 L [solution] = 2 mol/L = 2 M

The molarity is 6 mol/l.

2 m

The molarity is 0,041

3mol/0.5L

1 m

This solution is 2 molar (2 mol/L).

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

The molarity is 7 mol/L.

Molarity=no. of moles of solute/vol of solution in(L) molarity=0.4/9.79=0.04086 mol L-1=0.04086 M.

Molarity = moles of solute/Liters of solution Molarity = 6 Moles NaCl/2 Liters = 3 M NaCl ========

Molarity of water is 55.5 mol/L

0.6 mol/dm3

1m

Molarity = Moles/Unit VolumeSo here Molarity = (0.0255) / (10-2) = 2.55 M

The molarity of the given solution is 2.5 mol/L.

The moLaRity of this solution ie 2 mol/L or 2M KI (it is a 'two molair potassium iodide' solution)

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)

.036

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