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initial molarity*initial volume= final molarity*final volume Initial molarity= 1.50M Initial volume= 20.00ml Final Volume=150.0ml Thus final molarity =1.50M*20ml/150ml=0.200M. New molar concentration= final molarity
What volume do you want to make. To make 1 liter, you take the 185 g (the molar mass) and dissolve in enough solvent to make the final volume 1 liter.
The concentration is 1 mol/L or 5,611 g KOH/100 mL solution.
You need to add the 50ul stock solution to 1200ul of distilled water to produce 1250ul of solution with a concentration of 2ul per ml.
13.6% methanol solution.
initial molarity*initial volume= final molarity*final volume Initial molarity= 1.50M Initial volume= 20.00ml Final Volume=150.0ml Thus final molarity =1.50M*20ml/150ml=0.200M. New molar concentration= final molarity
.48 = [OH-]
Assuming you want 0.1% weigh/volume, you dissolve 0.1 g mercuric chloride in 100 ml of solution. So, you would weigh out 0.1 g (100 mg) of solid and dissolve in enough solvent to make a final volume of 100 ml.
Dissolve 2 moles of the compound in enough water to make a final volume of 1 liter.
For all dilution/ concentration problems you use the simple equation: M1V1 = M2V2 2.40*V2 = 8.25*25 V2 = (8.25*25)/2.40 V2 = 85.9mL Final volume will be 86mL.
What volume do you want to make. To make 1 liter, you take the 185 g (the molar mass) and dissolve in enough solvent to make the final volume 1 liter.
4.8214
5.85gms/500cc
Dissolve 15,015 g urea in 0,5 L demineralzed water; work with a thermostat at 20 oC and a volumetric flak.
It depends on the final solution Volume you want to prepare. For 100ml of a 6M NaCL solution, you add 35.1g of NaCl to water until you reach 100ml. Dissolve and autoclave for 15 mins.
14.625
Adding more solvent to a solution decreases the molarity of the solution. This is based on the principle that initial volume times initial molarity must be equivalent to final volume times final molarity.