0
How many grams of nacl would you dissolve in water to make a 50mM nacl solution with a 500mL of final volume?
Wiki User
∙ 10y ago
Solubility increases with temperature, but the solubility of sodium chloride in water is 316 grams per litre at 0 degrees Celsius, and 330 grams per litre at 70 degrees Celsius. Since room temperature is somewhere between these two, this gives upper and lower limits of the solubility at room temperature.
50 grams of water has a volume of 50 cubic centimetres, or 0.05 litres. In one litre you could dissolve between 316 grams and 330 grams, so in 0.05 litres you could dissolve between 15.8 and 16.5 grams, where 15.8 = 316 x 0.05 and 16.5 = 330 x 0.05.
So we can say it's around 16 grams of NaCl in 50 grams of water at room temperature.
Wiki User
∙ 15y ago
Wiki User
∙ 10y agoTo make a .5 molar solution in 750 g of water you need .5 * 1000 / 750 = 2/3 mol of sodium chloride.
The molar mass of sodium chloride is 58.44 g/mol, so that's 58.44 * 2/3 = 38.96 g of sodium chloride.
Wiki User
∙ 8y agoThe concentration is 50 % but this solution is supesaturated.
Wiki User
∙ 8y agoThis mass is 270,225 g.
Wiki User
∙ 7y agoThe mass is 202 g.
Wiki User
∙ 15y ago14.625
Wiki User
∙ 14y ago1.4625
Wiki User
∙ 10y ago1.461 g
Add your answer:
Earn +20 pts
How many grams of sodium chloride molecular weight 58.5 g mole would you dissolve in water to make a 5 solution with 500 final volume?
5.85gms/500cc
How many grams of NaCl would be required to make 6M solution?
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.
How many grams of NaCl molecular weight 58.5 g mole -1 would you dissolve in water to make a 0.5M NaCl solution with 500 ml final volume?
14.625
What is the concentration in mv percent of a solution prepared from 50 g NaCl and 2.5 L of water?
Chemists often express the concentration of an unsaturated solution as the mass of solute dissolved per volume of the solution. This type of concentration is expressed as percent relationship. The mass/volume percent is also referred to as the percent (m/v)The solubility of NaCl at room temperature is 36g/100mL. Clearly in the problem stated above, the NaCl-H2O solution is quite dilute and much below the saturation point.The following formula is useful in determining the mass/volume percent:m/v% = [ mass solute(g) / volume of solution (mL) ] x 100%2.5 L can be expressed in mL.2.5L = 2500mLtherefore the m/v% = (50g NaCl / 2500 mL H2O) * 100%m/v% = 0.02 * 100%m/v% = 2%Therefore the concentration of this solution as a m/v percent is 2%.Note1: The question is a bit misleading since it never states what is the desired final volume of the NaCl-H2O solution. The required number of grams of solute should never be added directly to the desired final volume of solvent, because volume generally changes when solutions are made.When preparing solutions, the correct procedure is to dissolve the solute in a volume of solvent smaller than the final desired volume. The resulting solution is then diluted to the desired final volume by addition of more solvent. See note 2 for preparation.Note2: To actually prepare this solution, it would be ideal to have the appropriate volumetric glassware. Lets say all you had was a 2L volumetric flask, a 500mL volumetric flask and a 3L storage container.What you could do is add the 50g of NaCl to the empty 2L volumetric flask, then fill the flask with water until you reach the 2L calibration mark. You could then transfer that solution to the 3L storage container.You would then fill the 500mL volumetric flask with water to its calibration mark, and then transfer the water to the storage container. The result would be a 2% (m/v) saline solution with a final volume of 2.5L contained in a 3L storage container.
How do you prepare a 500mL of 1M of NaCl solutuion?
If you need to make just 100mL, then you need 1 tenth of a liter that is 5M. If you were to make 1L of 5 molar NaCl, you would need 5 times the molar mass of NaCl (58.44g/mol) dissolved in 1L of water. Thus for 1L of a 5M solution you need 5 * 58.44g, or 292.2 grams of NaCl. However, since we only want 100mL, which is 1/10 of a Liter, we also only need 1/10 the amount of NaCl, or 292.2 / 10, which is 29.22g. So, measure out 29.22g NaCl, and dissolve completly in a volume less than 100mL, say 80mL, then bring the final volume up to 100mL. You now have 100mL of a 5M NaCl solution.
How do you prepare 0.1 percent mercuric chloride solution?
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.
How could one make a 2 M solution of a compound?
Dissolve 2 moles of the compound in enough water to make a final volume of 1 liter.
How do you prepare 1 molar iodoacetamide solution?
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.
How many grams of sodium chloride molecular weight 58.5 g mole would you dissolve in water to make a 5 solution with 500 final volume?
5.85gms/500cc
How you would make a 0.5 molar solution of urea with a final solution volume of 0.5 liter.?
Dissolve 15,015 g urea in 0,5 L demineralzed water; work with a thermostat at 20 oC and a volumetric flak.
What is the molarity of a solution that is made using 1.2 moles of a substance in 500mL?
Molarity (M) is defined as moles of solute/liters of solution. Assuming the final volume is 500 ml (0.5 liters), then M = 1.2 moles/0.5 liters = 2.4 M
How many grams of NaCl would be required to make 6M solution?
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.
How many grams of NaCl molecular weight 58.5 g mole -1 would you dissolve in water to make a 0.5M NaCl solution with 500 ml final volume?
14.625
What is the effect on the molarity of a solution of adding more solvent to a solution?
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.
What is the concentration in mv percent of a solution prepared from 50 g NaCl and 2.5 L of water?
Chemists often express the concentration of an unsaturated solution as the mass of solute dissolved per volume of the solution. This type of concentration is expressed as percent relationship. The mass/volume percent is also referred to as the percent (m/v)The solubility of NaCl at room temperature is 36g/100mL. Clearly in the problem stated above, the NaCl-H2O solution is quite dilute and much below the saturation point.The following formula is useful in determining the mass/volume percent:m/v% = [ mass solute(g) / volume of solution (mL) ] x 100%2.5 L can be expressed in mL.2.5L = 2500mLtherefore the m/v% = (50g NaCl / 2500 mL H2O) * 100%m/v% = 0.02 * 100%m/v% = 2%Therefore the concentration of this solution as a m/v percent is 2%.Note1: The question is a bit misleading since it never states what is the desired final volume of the NaCl-H2O solution. The required number of grams of solute should never be added directly to the desired final volume of solvent, because volume generally changes when solutions are made.When preparing solutions, the correct procedure is to dissolve the solute in a volume of solvent smaller than the final desired volume. The resulting solution is then diluted to the desired final volume by addition of more solvent. See note 2 for preparation.Note2: To actually prepare this solution, it would be ideal to have the appropriate volumetric glassware. Lets say all you had was a 2L volumetric flask, a 500mL volumetric flask and a 3L storage container.What you could do is add the 50g of NaCl to the empty 2L volumetric flask, then fill the flask with water until you reach the 2L calibration mark. You could then transfer that solution to the 3L storage container.You would then fill the 500mL volumetric flask with water to its calibration mark, and then transfer the water to the storage container. The result would be a 2% (m/v) saline solution with a final volume of 2.5L contained in a 3L storage container.
If 20.00mL of a 1.50M solution of KBr is diluted to a final volume of 150.0mL what is the new molar concentration?
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
How do you prepare 1000 ppm chloride solution from NaCl?
What volume of this solution do you desire? Let's say you want to make 1 liter of such a solution. You would weigh out 1 gram (1000 mg) of NaCl and dissolve it in enough water to make a final volume of 1 liter (1000 ml). Since 1000 ppm means 1000 mg/liter, this is how you make 1 liter of that solution. For larger or smaller volumes, adjust appropriately.
