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250 M means contains 250 moles per liter, which is probably impossible 1) . However, taking the question as stated, the answer is (2.0 mole)/(250 moles/liter) = 0.0080 liter or 8.0 milliliters, to the justified number of significant digits.
1) Commented: It is impossible!
The solution in this question is really impossible in every way:
- The highest solubility of KCl in boiling water that is: 567 g/L (100 °C), the molar mass being 74.551 g/mol, this is 7.6 mol/L ( = 7.6 M)
- Even one Litre pure (molten) KCl can not contain 250 moles!
The density if pure KCl is (less than) 1.984 g/cm3 , being equal to 0.027 mol/mL =
27 mol/L with NO solvent added. ( = 27 M)
What else can I help you with?
What is the grams in 250 ml of a 5 percent solution?
To find the grams in 250 ml of a 5% solution, you can use the formula: (volume in ml * percentage concentration / 100). So for this case: (250 ml * 5%/100) = 12.5 grams.
What volume would be needed to dilute a 5.7 M solution to a final concentration of 0.35 M and a volume of 250 mL?
By using the formula V1 x N1 = V2 x N2 Taking V1= 250 ml; N1= 0.35M; N2= 5.7M. V2 = volume of 5.7M needed to dilute V2 = V1 x N1 N2 = 250 x 0.35 = 15.35ml 5.7
What is the number of moles of solute in 250 mL of a 0.4M solutionon centration?
1 mole in 250 ml and 4 moles in 1 liter or 1000 mls
What is made by adding 4.5 moles of NH3 to 250ml of water.what is the molarity?
Adding 4.5 moles of NH3 to 250 mL of water will result in a solution with a volume slightly greater than 250 mL. To calculate the molarity, you need to know the final volume of the solution. Once you have the final volume, you can use the formula: Molarity = moles of solute / liters of solution.
How do you prepare 100 ppm stock solution of nickel nitrate in 250 ml?
To prepare a 100 ppm stock solution of nickel nitrate in 250 ml, first calculate the mass of nickel nitrate needed. Nickel nitrate (Ni(NO3)2·6H2O) has a molar mass of approximately 290.79 g/mol. For a 100 ppm solution, you need 100 mg of nickel nitrate in 1 liter, so for 250 ml, you would require 25 mg of nickel nitrate. Weigh out 25 mg of nickel nitrate, dissolve it in a small volume of distilled water, and then dilute the solution to a final volume of 250 ml with distilled water in a volumetric flask.
How much 2M Nacl solution would you need to make 250ml of 0.15M Nacl solution?
By the definition of molarity, which is mass of solute in moles divided by solution volume in liters, 250 ml of 0.15 M NaCl* solution requires (250/1000)(0.15) or 0.0375 moles of NaCl. Each liter of 2M NaCl solution contains 2 moles of NaCl. Therefore, an amount of 0.0375 moles of NaCl is contained in (0.0375/2) liters, or about 18.75 ml of the 2M NaCl, and if this volume of the more concentrated solution is diluted to a total volume of 250 ml, a 0.15 M solution will be obtained. _________________ *Note correct capitalization of the formula.
What volume of 5.19M sodium chloride contains 250 moles of sodium chloride?
The answer is 48,17 L.
What is the grams in 250 ml of a 5 percent solution?
To find the grams in 250 ml of a 5% solution, you can use the formula: (volume in ml * percentage concentration / 100). So for this case: (250 ml * 5%/100) = 12.5 grams.
What volume of 12M HCl solution is needed to prepare 250 mL of 0.100M solution?
To find the volume needed, you can use the formula: M1V1 = M2V2. Here, M1 = 12M (initial concentration), V1 = volume of 12M HCl solution needed, M2 = 0.100M (final concentration), and V2 = 250 mL. Rearranging the formula, V1 = (M2 * V2) / M1 = (0.100M * 250mL) / 12M = 2.08 mL. Therefore, you will need 2.08 mL of the 12M HCl solution to prepare 250 mL of 0.100M solution.
How many mL of water are present in 250 mL of a 15 percent by volume aqueous hydrochloric acid solution?
The water volume is 212,5 mL.
How many g of KCl do you need to make 2.5 L of a 10 weight volume solution?
For a 10 % solution you need 250 g KCl.
If you have 250 milliliters of a solution and you need to have the solution in cubic centimeters How do you convert this?
1cc (cubic centimeter) and 1mL (milliliter) are the same volume. So, 250mL is the same as 250cc
What volume would be needed to dilute a 5.7 M solution to a final concentration of 0.35 M and a volume of 250 mL?
By using the formula V1 x N1 = V2 x N2 Taking V1= 250 ml; N1= 0.35M; N2= 5.7M. V2 = volume of 5.7M needed to dilute V2 = V1 x N1 N2 = 250 x 0.35 = 15.35ml 5.7
What is the number of moles of solute in 250 mL of a 0.4M solutionon centration?
1 mole in 250 ml and 4 moles in 1 liter or 1000 mls
Homogenized whole milk contains 4 butterfat by volume. How many milliliters of fat are there in a glass (250 mL) of milk?
10 mL
A solution contains 30 g of calcium chloride in 250 g of water express the mass percent?
The solution has a total mass of 30 + 250 = 380 g. The mass percent of calcium chloride in this solution is 100(30/380) = 7.9 %, to the justified number of significant digits.
How many milliliters of a stock solution of 2.00 m kno3 would you need to prepare 250 ml of 0.150 m kno3 please show work?
To prepare 250 ml of 0.150 M KNO3 solution, you would need to dilute the stock solution (2.00 M KNO3) with a certain volume of water. You can use the formula for dilution: M1V1 = M2V2, where M1 is the initial concentration (2.00 M), V1 is the initial volume (unknown), M2 is the final concentration (0.150 M), and V2 is the final volume (250 ml). Rearrange the formula to solve for V1: V1 = (M2 * V2) / M1. Substitute the values: V1 = (0.150 M * 250 ml) / 2.00 M = 18.75 ml. You would need 18.75 ml of the stock solution to prepare 250 ml of 0.150 M KNO3 solution.
