How to Dilute an Acid

Purchasing the most dilute acid that will meet you needs is recommended for safety and ease of use, but sometimes you will need to dilute it further at home. Do not skimp on safety equipment, since concentrated acids can cause serious chemical burns. When calculating the amount of acid and water you need to mix, you'll need to know the molar concentration (M) of your acid and the molar concentration you'd like to end up with after dilution.

How to Safely Dilute Acids

Add distilled water to a large flask and add a tiny quantity of acid. Allow the solution to cool off, then add the remaining acid in small doses. If you’re using an extremely concentrated acid, cool the water in an ice bath beforehand.

Part 1

Part 1 of 3:

Calculating the Dilution Formula

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1
Check what you already have. Find the concentration of the acid solution on the label, or in the word problem you are working on. This number is often written in units of molarity, or molar concentration, abbreviated as M. For example, a "6M" acid contains six moles of acid molecules per liter. ^{[1]
X
Research source} We'll call this starting concentration C ₁ .
- The formula below will also use the term V ₁ . This is the volume of the acid we will be adding to water. We probably won't use the entire bottle of acid, though, so we don't know what this number is yet.
2
Decide on an end result. The desired concentration and volume of acid is typically determined by a school assignment or by the requirements of the laboratory you are working in. ^{[2]
X
Research source} For example, we might want to dilute our acid to a concentration of 2M, and need 0.5 liters (0.1 US gal). We'll call this desired concentration C ₂ and the desired volume V ₂ .
- If you are using unusual units, convert them all to units of molar concentration (moles per liter) and liters before you continue.
- If you are not certain what concentration or volume of acid is required, consult your teacher, a chemist, or an expert in the task you plan to use acid in.
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3
Write the formula for calculating dilution. Whenever you prepare to dilute a solution, you can use the formula C ₁ V ₁ = C ₂ V ₂ . ^{[3]
X
Research source} words, this means "the initial solution's concentration x its volume = the diluted solutions' concentration x its volume." We know this is true because concentration x volume = the total amount of acid, and the total amount of acid will remain the same as it is added to the water.
- In our example, we can write this formula (6M)(V ₁ )=(2M)(0.5L) .
4
. This term, V ₁ , will tell us how much of the initial acid solution we need to add to water in order to end up with the desired concentration and volume. ^{[4]
X
Research source} Rearrange the formula as V ₁ =(C ₂ V ₂ )/(C ₁ ) , then plug in the numbers you know.
- In our example, we would end up with V ₁ =((2M)(0.5L))/(6M)= ¹ ⁄ ₆ liter (0.0 US gal). This approximately equals 0.167 liters (0.0 US gal), or 167 milliliters.
5
Calculate how much water you'll need. Now that you now V ₁ , the amount of acid you'll be using, and V ₂ , the amount of solution you'll end up with, you can easily calculate how much water you need to make up the difference. V ₂ - V ₁ = the volume of water required.
- In our case, we want to end up 0.5 liters (0.1 US gal) and will be using 0.167 liters (0.0 US gal) of acid. The amount of water we need = 0.5L - 0.167L = 0.333L, or 333 milliliters.
- Always double-check your calculations to make sure that they're accurate. ^{[5]
  X
  Expert Source
  
  Chris Hasegawa, PhD
  Retired Science Professor & Dean
  
  Expert Interview. 29 July 2021.}

Part 2

Part 2 of 3:

Preparing a Safe Workspace

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1
Read the relevant Chemical Safety Cards online. International Chemical Safety Cards provide succinct, detailed safety information. Search for the exact name of the acid you will be using, such as "hydrochloric acid," in the online database . Some acids may require additional safety precautions, besides those described below.
- Sometimes several cards are issued, depending on the concentration and additions to the acid. Pick the one that most closely matches your initial acid solution.
2
Wear splash goggles, gloves, and a lab coat. Splash safety goggles that cover all sides of the eyes are required when handling acid. Protect your skin and clothing by wearing gloves and a lab coat or apron.
- Tie up long hair before handling the acid.
- Acid can take several hours to burn holes through clothing. Even if you do not notice a spill, a few drops can damage your clothing if it is not underneath a lab coat.
Whenever possible, keep the acid solution in a functioning fume hood while you are working. This limits exposure to gaseous vapors produced by the acid, which can be corrosive or poisonous. ^{[6]
X
Research source} If a fume hood is not available, open all windows and doors, or turn on a fan to ventilate the area.
4
Know where running water is located. If acid gets on your eyes or skin, you'll need to flush it with cool, running water for 15–20 minutes. Don't start the dilution until you know where to find the nearest functioning eye wash station or sink.
- When washing your eyes, keep your eyelids wide open. Rotate your eyes by looking up, right, down, and left to make sure all sides of your eyeball are rinsed.
5
Have a spill plan ready, specific to your acid. You can purchase an acid spill kit that contains all the necessary materials, or acquire neutralizers and absorbers separately. The process described here can be used for hydrochloric, sulfuric, nitric, or phosphoric acid, but other acids may require further research to dispose of properly:
- Ventilate the area by opening windows and doors, and turning on fume hoods and fans.
- Apply a weak base such as sodium carbonate (soda ash), sodium bicarbonate, or calcium carbonate to the outer edges of the spill, avoiding the resulting spatter.
- Continue to apply slowly, working inward, until the spill is covered.
- Mix well with a plastic tool. Check the pH of the spill with litmus paper. Add more base if necessary to get the pH between 6 and 8, then flush the spill down a drain with plenty of water.

Part 3

Part 3 of 3:

Diluting the Acid

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1
Cool water in an ice bath when using concentrated acids. This step is only necessary when you'll be handling extremely concentrated acid solutions, such as 18M sulfuric acid, or 12M hydrochloric acid. ^{[7]
X
Research source} Cool the water you'll be using by keeping it in a container surrounded by ice for at least 20 minutes before the dilution begins.
- For most dilutions, the water can be at room temperature.
2
Add distilled water to a large flask. For projects involving careful measurement, such as titration, use a volumetric flask. For most practical purposes, an Erlenmeyer flask can be used instead. In either case, choose a container that can easily contain your total desired volume, with plenty of space remaining, to minimize splashes over the rim.
- You don't need to carefully measure this water, as long as it came from a container that was carefully measured to contain the total required amount of water.
3
Add a tiny quantity of acid. If using a small volume of acid, use a graduated (Mohr) pipette or volumetric pipette with a rubber bulb on top. For larger volumes, place a funnel in the neck of the flask, and slowly pour in a small quantity of the acid using a graduated cylinder.
- Never use a mouth pipette in a chemistry lab.
Strong acids may generate lots of heat when added to water. If the acid was highly concentrated, the solution may splatter or produce corrosive fumes. If this happens, you will need to perform the entire dilution in very small doses, or cool the water in an ice bath before you continue.
5
Add the remaining acid in small doses. Allow the solution time to cool off between each dose, especially if you notice heat, fumes, or spatter. Continue until the required amount of acid has been added.
- This amount was calculated as V ₁ above.
For best results, you can stir the solution with a glass stirring rod after each addition of acid. If the size of the flask makes this impractical, stir the solution after the dilution is complete and the funnel is removed.
Pour the acid solution you created into a clearly labeled container, preferably a PVC coated glass bottle, and store in a safe location. Rinse the flask, funnel, stirring rod, pipette, and/or graduated cylinder in water to remove all traces of acid.

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How do you dilute acids safely?

Chris Hasegawa, PhD
Retired Science Professor & Dean
Dr. Chris Hasegawa was a Science Professor and the Dean at California State University Monterey Bay. Dr. Hasegawa specializes in teaching complex scientific concepts to students. He holds a BS in Biochemistry, a Master’s in Education, and his teaching credential from The University of California, Davis. He earned his PhD in Curriculum and Instruction from The University of Oregon. Before becoming a professor, Dr. Hasegawa conducted biochemical research in Neuropharmacology at the National Institute of Health. He also taught physical and life sciences and served as a teacher and administrator at public schools in California, Oregon, and Arizona.

Chris Hasegawa, PhD

Retired Science Professor & Dean

Expert Answer

Double-check your calculations and measurements before you dilute anything.

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When I dilute acid should I add acid to water or water to acid?

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You should always add acid to water, otherwise you will end up with an extremely exothermic reaction that can even boil the water and cause violent bumping that can result in acid splashing all over the place.

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Is it possible to measure acid in ppm?

Jomari Cabato

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To convert from molarity to ppm, first determine the molar mass of a substance. For instance, chloride has a molar mass of 35.5. A solution with 1 M concentration would have 35.5 g of chloride per 1 L of solution.

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It is possible to add half the required amount of water, diluting it fully, then slowly mixing in the remaining water. ^{[8]
X
Research source} This is not recommended for concentrated solutions.

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When mixing two acids, always add the stronger acid to the weaker, for the reason described above.

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Always add acid to the water, not the other way around. When the substances meet, they will produce a large amount of heat. The more water is involved, the more of a heat sink you have to absorb this heat, preventing boiling and splattering.

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Warnings

Even when the acidic effects are not profound the acid may still be poisonous. An example is hydrocyanic acid (not very strong, very poisonous).

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Never counter the effects of spilled acid with strong lye, such as KOH or NaOH. Use water or a weak base such as diluted sodium hydrogen carbonate (NaHCO3) instead.

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Do not dissolve materials for fun or whatever other reason, unless you know exactly what you are doing. In this way you may create extremely dangerous products such as poisonous or explosive gasses or explosives that ignite spontaneously.

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So called 'weak' acids may also produce lots of heat and be very dangerous. The distinction between weak and strong acids is purely a chemical one.

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Things You'll Need

Splash goggles
Gloves
Lab coat or apron
Eyewash station (access to cool, clear running water you can easily place your eye under)
Volumetric flask (for best accuracy) , or Erlenmeyer flask
Pipette (for small quantities) , or graduated cylinder ( for larger )
Water
Acid
Acid spill kit, or sodium bicarbonate and a plastic tool
Glass stirring rod

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Retired Science Professor & Dean

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How to Dilute an Acid

How to Safely Dilute Acids

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Calculating the Dilution Formula

Preparing a Safe Workspace

Diluting the Acid

Expert Q&A

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Tips

Warnings

Things You'll Need

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