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What volume of the 0.91 percent with NaCl is needed to prepare 100 ml of 0.45 percent with NaCl?
Wiki User
∙ 11y ago
Your stock is a bit more than twice as concentrated as your target concentration. Take 49.45 ml of the stock and mix with enough water to bring it up to 100 ml.
Now, the foregoing, notwithstanding, you want to prepare 100 ml...The precision of that measurement is going to drive your final results. It has only one significant digit so, your adding a quantity of stock with 4 significant digits (49.48 ml) is way too precise to be relevant. This is where you say, "I need to cut the concentration by about half so, I'll take 50 ml of the stock and add 50 ml of water. Sort of like how Justin Wilson measured ingredients for cooking.
Wiki User
∙ 11y ago
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How do you prepare a 30 percent NaCl solution?
Dissolve 30g of sodium chloride in 100 mL of water.
How many grams of sodium chloride are needed to prepare 600 ml of a 0.9 percent saline solution?
600 mL of 0,9 % sodium chloride: 6 x 0,9 = 5,4 grams NaCl
How would you prepare 400ml of a 0.24M NaCl solution?
We first calculate the amount, in moles, of NaCl that we will need.Amount of NaCl needed = 0.24 x 400/100 = 0.096mol. Mass of NaCl needed = (23.0 + 35.5) x 0.096 = 5.616g So to produce 400ml of 0.24M NaCl solution, accurately add 5.616 grams of NaCl to 400ml of deionised water.
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.
What volume of a 2.10 M NaCl solution is needed for a reaction that requires 200 g of NaCl answer in units of L?
To find the volume of the 2.10 M NaCl solution needed, first calculate the molar mass of NaCl (58.44 g/mol). Then, convert 200 g to moles (200 g / 58.44 g/mol). Use the molarity formula (Molarity = moles / volume) to find the volume required: volume = moles / Molarity. Plugging in the values gives volume = (200 g / 58.44 g/mol) / 2.10 mol/L, resulting in approximately 4.43 L.
What final volume would be needed in order to prepare a 0.50 M NaCl solution from 10.0 g of NaCl?
To determine the final volume needed to prepare a 0.50 M NaCl solution from 10.0 g of NaCl, you first need to calculate the number of moles in 10.0 g of NaCl using its molar mass. Then, use the formula C = n/V (concentration = moles/volume) to find the final volume, where n is the number of moles you calculated and C is the desired concentration.
How do you calculate 100 ml of 0.9 percent NaCL?
To calculate 100 ml of 0.9% NaCl solution, you would need to multiply the volume by the concentration as a decimal. 0.9% = 0.9/100 = 0.009. 100 ml * 0.009 = 0.9 grams of NaCl would be needed.
What volume of water should be added to 23.4 g of NaCl to make 100.0 mL of 4.00 M solution?
To prepare a 4.00 M NaCl solution, first calculate the moles of NaCl in 23.4 g. Then, determine the volume of water needed to make a total volume of 100.0 mL minus the volume of NaCl solution. Add the water to the NaCl to make a 100.0 mL solution.
How would you prepare 260 mL of 0.340M NaCl solution using an available 2.50M solution?
You would need to dilute the 2.50M NaCl solution with water. To prepare 260 mL of 0.340M NaCl solution, you would need to use the formula C1V1 = C2V2, where C1 is the initial concentration (2.50M) and V1 is the volume of the initial solution needed. Using this formula, you would calculate the volume of the 2.50M solution needed, then add water to dilute it to a total volume of 260 mL.
How do you prepare a solution 2 percent NaCl wv?
To prepare a 2% NaCl (w/v) solution, you would dissolve 2 grams of NaCl in enough water to make 100 mL of solution. This means you would add 2 grams of NaCl to a flask and then add water until the total volume reaches 100 mL.
How many moles of sodium chloride are needed to prepare 500 mL of a 0.250 M solution?
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.
How do you prepare a 30 percent NaCl solution?
Dissolve 30g of sodium chloride in 100 mL of water.
How many grams of sodium chloride are needed to prepare 600 ml of a 0.9 percent saline solution?
600 mL of 0,9 % sodium chloride: 6 x 0,9 = 5,4 grams NaCl
How would you prepare 30mL of a 5M NaCl solution from a 2M NaCl stock solution?
You have to evaporate (by open boiling) 45 mL of the 75 mL 2M NaCl solution thus reducing the volume to 30 mL 5M NaCl.
How would you prepare 400ml of a 0.24M NaCl solution?
We first calculate the amount, in moles, of NaCl that we will need.Amount of NaCl needed = 0.24 x 400/100 = 0.096mol. Mass of NaCl needed = (23.0 + 35.5) x 0.096 = 5.616g So to produce 400ml of 0.24M NaCl solution, accurately add 5.616 grams of NaCl to 400ml of deionised water.
How do you prepare approximately 100 ml of 1.0 m NaCl?
To prepare 100 ml of 1.0 M NaCl solution, you would need to dissolve 5.84 g of NaCl in enough water to reach a final volume of 100 ml. Measure out the required amount of NaCl, add it to a beaker, and then add water while stirring until the final volume reaches 100 ml.
How much 7 percent NaCl soln and 45 percent Nacl sol req'd to make 800ml 15 percent NaCl soln?
Let x be the volume of 7% NaCl soln needed, and y be the volume of 45% NaCl soln needed. We have the following equations: x + y = 800 (total volume of final soln) and 0.07x + 0.45y = 0.15*800 (amount of NaCl in final soln). Solve these equations to find x and y.
