0
What else can I help you with?
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 many grams of zebulose would you have to dissolve in 4 liters of water to make a 250 millimolar solution?
26.8125 g
How much NaCl is required for 100 mM NaCl solution?
To prepare a 100 mM NaCl solution, you would need to calculate the molecular weight of NaCl, which is approximately 58.44 g/mol (sodium's atomic weight is 22.99 g/mol and chlorine's is 35.45 g/mol). To make a 100 mM solution, you would need 0.1 moles of NaCl per liter of solution. This would be equivalent to 5.844 grams of NaCl per liter of solution.
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.
How to prepare a solution of 250 mM of sucrose?
A 5% sucrose solution has 5 grams of sucrose in every 100 grams of solution. As 1mL of water has a mass of 1 gram, you should dissolve 5 grams of sucrose in 95 mL of water.
How do you prepare saline water for nasal drops?
simply dissolve 5 ml of salt in 250 ml of warm water
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 many grams of zebulose would you have to dissolve in 4 liters of water to make a 250 millimolar solution?
26.8125 g
How I will make 3 Molar solution of potassium chloride in 250 milliliter?
To make a 3 Molar solution of potassium chloride in 250 milliliters: Calculate the mass of potassium chloride needed using its molar mass. Dissolve this mass of potassium chloride in a small amount of water, then add water to bring the total volume to 250 ml. Stir to ensure complete mixing and dissolve the potassium chloride completely.
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 can you make a hydrating solution containing 150mg of salt per 8 oz?
Weight 150 mg sodium chloride and dissolve in 250 mL water.
How do you prepare 0.02 n iodine solution?
2.538g in 1000ml. If you are making this for a titration, like for SO2 or thiosulfate, you need also to add iodide: 1. dissolve 8 g potassium iodide in about 250 mL water. 2. add 2.538 g iodine to the water solution. Stir until dissolved. 3. transfer to a 1000 mL volumetric flask and Q.S. to 1000 mL You should standardize vs. thiosulfate or arsenious oxide.
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.
How many grams of the compound trinitrotoluene are needed to prepare 250 ml of a 0.100 M solution of the compound?
C7H5N3O6 Molarity = moles of solute/Liters of solution (250 ml = 0.25 Liters ) 0.100 M C7H5N3O6 = X moles/0.25 L = 0.025 moles -------------------------now, 0.025 moles C7H5N3O6 (227.14 grams/1 mole C7H5N3O6) = 5.68 grams TNT ====================a good firecracker!
How do you prepare 100 ml of 1millimoles of CuSO4.5H2O Sol.?
If you mean 100 ml of 1 mM CuSO5.H2O, then dissolve 0.1 mmole CuSO4.H2O in sufficient water to make a final volume of 100 ml.molar mass CuSO4.5H2O = 250 g/mole 250 mg = 1 mmole 25 mg = 0.1 mmol Dissolve 25 mg in final volume of 100 mls
How do prepare 0.1M citric acid?
To prepare a 0.1M citric acid solution, measure out the appropriate amount of citric acid powder using a balance, dissolve it in the desired volume of water (usually in a volumetric flask), and mix well until fully dissolved. Finally, adjust the volume to the desired final volume with water, as needed.
How do you prepare a 0.5 M solution of chlorosulphonic acid?
Chlorosulfonic acid, or chlorosulfuric acid, has the formula HSO3Cl. That means I mole is 116.5 g. To make a 0.5 M solution, you need to weigh out 29.167 g of the acid and transfer it, with washings to a 250 ml graduated flask. Make it up to the mark with de-ionized water, ensuring that there is thorough mixing.
