To prepare a 6N ammonium hydroxide solution from a 30% solution, you would first calculate the molarity of the 30% solution. Then, you would dilute the 30% solution with water to reach the desired concentration. Calculate the volume of the 30% solution needed and dilute it with water to reach the final volume for a 6N concentration.
To calculate the mass of magnesium needed, use the formula: mass of solute = volume of solution (ml) x percentage concentration / 100. In this case, it would be 60 ml x 20% = 12 g or 12,000 mg of magnesium will be required to prepare 60 ml of a 20% solution.
To make a 5% solution of calcium chloride with a total volume of 500 ml, you would need to add 25 grams of calcium chloride. This is calculated by multiplying the volume of the solution (500 ml) by the desired concentration (5%) and converting to grams.
To create a 400 L solution that is 62% acid, you would need 200 L of the 80% acid solution and 200 L of the 30% acid solution. This would result in a final solution with the desired concentration.
To make a 1.0 M solution of sodium cation using sodium chloride, you need to consider the molar mass of sodium chloride (58.44 g/mol). Since 1 mole of sodium chloride provides 1 mole of sodium cation, you would need 58.44 g of sodium chloride to make a 1.0 M solution in 100 ml.
To prepare 4N potassium chloride solution, dissolve 149.5 g of potassium chloride in 1 liter of water. This will give you a solution with a concentration of 4N. Make sure to use a balance to accurately measure the amount of potassium chloride needed.
25
To prepare 250ml of a 2M potassium chloride solution, measure out 17.8g of potassium chloride and dissolve it in water to make a total volume of 250ml. Make sure to stir the solution well to ensure the potassium chloride is completely dissolved. Then, adjust the final volume to exactly 250ml by adding more water if needed.
The volume is 0,3 mL.
125 ml 500(ml) * 0.05 = 25 25 / 0.20 = 125
To prepare a 10mM ferric chloride solution, first calculate the molecular weight of FeCl3 to determine the amount needed to achieve a concentration of 10mM. Dissolve this amount in a known volume of water or solvent to make up the final volume of the solution, ensuring thorough mixing to achieve homogeneity.
To prepare a 1000 ppm chloride solution from sodium chloride, first calculate the mass of sodium chloride needed using the formula: (ppm concentration * volume of solution in liters) / 1000. Then dissolve this calculated mass of sodium chloride in the desired volume of water to make the solution. Finally, ensure the solution is thoroughly mixed before testing the concentration with appropriate methods.
500ml = 500cm3 = 0.5dm3 0.250M = 0.250mol/dm3 number of moles = molarity x volume number of moles = 0.250mol/dm3 x 0.5dm3 = 0.125mol 0.125mol of NaCl is needed to prepare the required solution.
Sodium chloride may be used as standard (for example to prepare sodium solutions with known concentration) because is a stable compound.
90 ml of dextrose and 4.41 litres of water.
To prepare a neutral ferric chloride solution from solid ferric chloride, first dissolve the solid ferric chloride in distilled water to form a concentrated solution. Then, slowly add a base such as sodium hydroxide solution while monitoring the pH using a pH meter until the desired neutral pH is reached. Finally, dilute the solution to the desired concentration with more distilled water if needed.
To prepare a 6N ammonium hydroxide solution from a 30% solution, you would first calculate the molarity of the 30% solution. Then, you would dilute the 30% solution with water to reach the desired concentration. Calculate the volume of the 30% solution needed and dilute it with water to reach the final volume for a 6N concentration.