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Before reading this answer, I recommend that you look at the question under the Related Questions links to the left of this answer "How do you prepare a solution of a specific concentration by dissolving a solid in a liquid?"
You must know two things to make a solution: the number of moles of the solute, and the number of liters of solution. Then you will add the correct volume of the concentrated solution so that you have the right number of moles, and then add water until the total volume is correct.
To make a solution from another solution by diluting it, you first need to know how many moles of solute you need in the final solution. That's very easy! You need to know the concentration of the final solution and its volume. Then just multiply those two together to get the number of moles of solute you need:
Equation 1) Moles of solute = Molarity * liters of solution
Now you know how many moles you need, you just have to figure out how to them them! To do that, we'll use the same equation, but now rearranged in a different order. We want to know how many liters of the original (concentrated) solution we need to get the correct number of moles. So just dividing both side by "Molarity" we get:
Equation 2) Liters of Solution = Moles of solution ÷ Molarity
So that will tell us how much concentrated solution to use. Then just add that much of the concentrated solution to enough water so that the total volume is correct.
-- Step #1: Determine the concentration and total volume of the new solution you want to make (probably given to you in the question you are solving!)
-- Step #2: Determine how many moles of solute must be present in that solution, using Equation 1
-- Step #3: Determine what volume you need (how many liters) of the concentrated solution you need to get the number of moles you got in Step #2, now using Equation 2
-- Step #4: Add the volume of concentrated solution you determined in Step #3 to the correct amount of water so that the total volume is what you need (from Step #1). HOWEVER, WHEN DILUTING A STRONG ACID, ALWAYS ADD ACID TO WATER! SAME FOR A STRONG BASE! To do this, just estimate how much water you will need to add (the total volume minus the volume from Step #3), and add a little less than this. Then add the concentrated acid to that, and then add a bit more water to get the exact volume correct.
-- Let me do a couple of examples now:
--Example 1: How do you make 200 mL of a 0.1 M solution of hydrochloric acid (HCl) from a solution of 1.0 M HCl?
--Answer: First let's find how many moles of HCl we need in our diluted solution. Using Equation 1, we have:
Moles of HCl = 0.2 L * 0.1 M = 0.02 moles
(remember that 200 mL = 0.2 L)
Now how many liters of the 1.0 M solution do we need to get 0.02 moles? Now using Equation 2:
Volume of 1.0 M solution = 0.02 moles ÷ 1.0 M = 0.02 L
And again, 0.02 L is equal to 20 mL
So to make our solution, we are going to ADD ACID TO WATER. So, first add about 150 mL of water to a flask. Then add 20.0 mL of 1.0 M HCl. Then add as much water as necessary to that the total volume is exactly 200 mL. This is usually done in what is called a volumetric flask -- and you'd want to use a 200 mL volumetric flask in this case.
--- Example 2: How do you make 2.0 liters of a 0.231 M solution of potassium nitrate (KNO3) from a 3.0 M solution of KNO3?
--- Answer: Same as before, how many moles of KNO3 do we need in the diluted solution?
Moles of KNO3 = 0.231 M * 2.0 L = 0.462 moles.
Now how many liters of 3.0 M solution do we need to get that many moles?
Liters of 3.0 M solution = 0.462 moles ÷ 3.0 M = .154 L
And again, that 154 mL.
To make our solution, we will add 154 mL of the 3.0 M KNO3 solution to a volumetric flask, and then add as much water as we need so that the total volume is exactly 2.0 liters (use a 2 liter volumetric flask for this!)
What else can I help you with?
How do you prepare 05M glutaraldehyde?
To prepare a 0.5M glutaraldehyde solution, you would need to dilute a concentrated glutaraldehyde stock solution with the appropriate volume of water or buffer solution. Calculate the volume of stock solution needed based on the desired final volume and concentration, then dilute with the solvent. Finally, mix the solution thoroughly to ensure uniform distribution. Remember to follow safety protocols when working with glutaraldehyde, as it is a hazardous chemical.
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 0.25N sulphuric acid from 2N sulphuric acid?
To prepare 0.25N sulphuric acid from 2N sulphuric acid, you can dilute the 2N solution by adding 7 parts of water to 1 part of the 2N solution. This will result in a final 0.25N sulphuric acid solution.
How do you prepare 0.05N of HCl?
To prepare 0.05N HCl solution, you would need to calculate the amount of concentrated hydrochloric acid solution (typically 37% concentration) needed to dilute with water to get the desired concentration. Measure the appropriate volume of the concentrated acid and dilute it with the required amount of water to achieve a final volume of 1 liter.
How do you prepare 10mL of a 25M HCl solution?
To prepare 10mL of a 25M HCl solution, you would need to dilute the concentrated HCl solution with the appropriate amount of water. For example, to make a 25M solution, you could start with a 10M HCl solution and dilute it appropriately. To determine the specific volume of each solution needed for dilution, you can use the formula C1V1 = C2V2, where C1 is the initial concentration, V1 is the volume of the initial solution, C2 is the final concentration, and V2 is the final volume.
How do you prepare 05M glutaraldehyde?
To prepare a 0.5M glutaraldehyde solution, you would need to dilute a concentrated glutaraldehyde stock solution with the appropriate volume of water or buffer solution. Calculate the volume of stock solution needed based on the desired final volume and concentration, then dilute with the solvent. Finally, mix the solution thoroughly to ensure uniform distribution. Remember to follow safety protocols when working with glutaraldehyde, as it is a hazardous chemical.
How can one prepare dilute ammonia solution?
To prepare a dilute ammonia solution, mix a small amount of concentrated ammonia solution with a large amount of water in a clean container. Always add the ammonia solution to the water slowly and carefully, as ammonia is caustic and can release fumes. It's important to wear proper protective gear such as gloves and goggles while handling ammonia.
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 0.25N sulphuric acid from 2N sulphuric acid?
To prepare 0.25N sulphuric acid from 2N sulphuric acid, you can dilute the 2N solution by adding 7 parts of water to 1 part of the 2N solution. This will result in a final 0.25N sulphuric acid solution.
How do you prepare 0.1N Na2S2O3 solution?
To prepare a 0.1N Na2S2O3 solution, dissolve 24.98 grams of Na2S2O3·5H2O (sodium thiosulfate pentahydrate) in distilled water and dilute to 1 liter in a volumetric flask. This will give you a 0.1N (normal) solution of Na2S2O3.
If you add solute to a dilute solution the solution becomes more what solution?
The dilute solution become a concentrated solution.
A solution that does not contain enough solute?
A solution that only contains a small amount of solute, is a dilute or very dilute solution.
How do you prepare 0.05N of HCl?
To prepare 0.05N HCl solution, you would need to calculate the amount of concentrated hydrochloric acid solution (typically 37% concentration) needed to dilute with water to get the desired concentration. Measure the appropriate volume of the concentrated acid and dilute it with the required amount of water to achieve a final volume of 1 liter.
How do you prepare 10mL of a 25M HCl solution?
To prepare 10mL of a 25M HCl solution, you would need to dilute the concentrated HCl solution with the appropriate amount of water. For example, to make a 25M solution, you could start with a 10M HCl solution and dilute it appropriately. To determine the specific volume of each solution needed for dilution, you can use the formula C1V1 = C2V2, where C1 is the initial concentration, V1 is the volume of the initial solution, C2 is the final concentration, and V2 is the final volume.
How can you prepare solution 0.2 ppm from 1000 ppm?
To prepare a 0.2 ppm solution from a 1000 ppm solution, you would need to dilute the 1000 ppm solution by adding 5000 parts of solvent for every 1 part of the 1000 ppm solution. This means mixing 1 part of the 1000 ppm solution with 5000 parts of solvent to achieve a 0.2 ppm concentration.
What is typically done to a solution to dilute it?
The quantity of the solvent is increased to dilute a solution.
How do you prepare 1 N ferrous ammonium sulphate?
To prepare 1 N ferrous ammonium sulfate solution, dissolve 392.15 g of the compound in distilled water and dilute to 1 L. This will yield a solution with a concentration of 1 N.
