Dissolve 111 g anhydrous CaCl2 in 1 L distilled water.
Let me translate the question: I think you are asking how to make a 0.1 molar solution of Na2S2O4. Molarity is moles of solute divided by liters of solution. To make this easy, let's assume you want to make one liter of the solution. That means you need to dissolve in 0.1 moles of Na2S2O4 into one liter of water to make a 0.1 molar solution. The formula weight of Na2S2O4 is 174.1 grams per mole so 0.1 moles of it is 17.41 grams. Therefore you would need to dissolve 17.41 grams of Na2S2O4 into one liter of water to make a 0.1 molar solution.
5.0 molar
Molarity is calculated as moles of solute divided by volume of solution in liters. In this case, you have 2 moles of sodium chloride in a 0.5 liter solution. So the molarity would be 2 moles / 0.5 L = 4 M.
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Ammonium molybdate is (NH4)2MoO4. Its molar mass is 148g/mol. A 0.5M solution will have half a mole per liter of water. Half a mole of ammonium molybdate is 74g, so you would measure out 74g of it, and dissolve it in a liter of water.
CaCl2 has more particles when dissolved
Ten milliliters is a hundredth of a liter. So in a two molar solution, you would have .02 moles in 10 ml.
Let me translate the question: I think you are asking how to make a 0.1 molar solution of Na2S2O4. Molarity is moles of solute divided by liters of solution. To make this easy, let's assume you want to make one liter of the solution. That means you need to dissolve in 0.1 moles of Na2S2O4 into one liter of water to make a 0.1 molar solution. The formula weight of Na2S2O4 is 174.1 grams per mole so 0.1 moles of it is 17.41 grams. Therefore you would need to dissolve 17.41 grams of Na2S2O4 into one liter of water to make a 0.1 molar solution.
By definition, a 10 molar solution contains 10 moles of the solute per liter of solution. Therefore, since 100 ml is 1/10 of a liter, 100 ml of such a solution would contain one mole of the solute. Physically, this would normally be accomplished by adding 10 grams, stated to be one mole of the solute, to a 100 ml volumetric flask, then adding pure water until the mark on the neck of the flask is reached.
Dissolve 15,015 g urea in 0,5 L demineralzed water; work with a thermostat at 20 oC and a volumetric flak.
if you mean a 1 litre, 1 molar solution, then you have 1 mole. you just need to multiply by avagadro's number
290 grams
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A solution concentration maybe expressed as g/liter but it is much more common and scientifically desired to express the concentration as a molarity or normality. So 36.5 g per liter of HCl would be 1 molar or 1 normal.
The formula mass of KCl is 75.5 so when 94.375g of it are dissolved in i litre water the solution prepared is 1.25 molar