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!)
Add lots of water to it and it will become diluted
Add some of the solute to a large(r) amount of solvent.
Dilute it.
poure water on the concentrated acid
to prepare 1N we have to dilute 40gms of NaOH in 1 litre of water as for NaOH normality =molarity so to prepare 0.1N NaOH we have to dilute 4gms of NaOH in 1 litre of water..
You prepare a primary solution then dilute portion of your solution down to the required concentration. For example, you want a 10 ppm salt solution (10 mg/L), you dilute 1 g of salt in 1 L of water you get 1000 ppm salt solution. You take 10 ml of your salt solution (0.01 g salt in 10 g) and add in additional 980 ml of water then you get a 10 ppm weight solution.
To prepare a 0.9% solution take 0.9grams NaCl and dilute with 100mls of water.
How to prepare 0,28% ammonia
To prepare a dilute solution.
Dilute it.
poure water on the concentrated acid
to prepare 1N we have to dilute 40gms of NaOH in 1 litre of water as for NaOH normality =molarity so to prepare 0.1N NaOH we have to dilute 4gms of NaOH in 1 litre of water..
You prepare a primary solution then dilute portion of your solution down to the required concentration. For example, you want a 10 ppm salt solution (10 mg/L), you dilute 1 g of salt in 1 L of water you get 1000 ppm salt solution. You take 10 ml of your salt solution (0.01 g salt in 10 g) and add in additional 980 ml of water then you get a 10 ppm weight solution.
The dilute solution become a concentrated solution.
A solution that only contains a small amount of solute, is a dilute or very dilute solution.
dilute it 1 in 5000. likely best done with a serial or step dilution
To prepare a 0.9% solution take 0.9grams NaCl and dilute with 100mls of water.
To dilute a solution, add water to it. To concentrate a solution, take water out of it.
The quantity of the solvent is increased to dilute a solution.