# What is the simplest way to create a precipitation reaction at home

Whats the easiest way to create a precipitation reaction at home? (Preferably with easily retrievable chemicals) I need this because I'm making a video for my film education.

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I mean without chemicals that are hard to get – felix Mar 24 at 21:04
If Acid-base counts those are probably the easiest. – Hanry Hu Mar 24 at 21:31

Here's one easy way :

Make a solution of salt ($\ce{NaCl}$) in water, and another solution of Silver Nitrate ($\ce{AgNO_3}$), which you can buy easily) in water.

Upon mixing the two, $\ce{AgCl}$ (Silver chloride, a white compound) will instantly precipitate.

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Silver chloride is white. The grey colour is due to elemental silver (which AgCl is reduced to) – orthocresol Mar 24 at 21:43
@orthocresol Thanks, amended – Chemobot Mar 24 at 21:44
Thank you so much! color doenst matter because i can correct the color in after effects :) – felix Mar 24 at 22:13
@Felix please don't post "thank you" as a comment. Instead, up vote or accept answers that you found useful. Thanks – TIPS Mar 24 at 23:37

For a low-hazard experiment with standard household materials, some variation of the following should work:

Chemicals:

1. $\ce{CaCl2}$ : Available as a type of ice melt (e.g., this)
2. Acetic acid : White distilled vinegar
3. $\ce{NaHCO3}$ : Baking soda

Procedure:

1. Dilute the vinegar in water, at about $1$ part vinegar to $10$ parts water.
2. Add a small handful of the $\ce{CaCl2}$ and stir to dissolve.
3. In a separate container, mix $\sim 1~\mathrm{Tbsp}$ baking soda in $1~ \mathrm{cup}$ lukewarm water
4. If all of the baking soda dissolves, keep adding more until it won't dissolve further.
5. Let the baking soda solids settle to the bottom of the container, then carefully pour the liquid into a clear container, suitable for the demonstration.

For the demonstration, add the $\ce{CaCl2}$/vinegar solution drop-by-drop to the bicarbonate solution. If I've thought this through properly, a white $\ce{CaCO3}\!\left(\mathrm s\right)$ precipitate should hopefully form as each drop is added.

To note, I specified the dilute vinegar solution to try to avoid premature precipitation of $\ce{Ca(OH)2}$. If the demonstration solution fizzes too much when adding the drops of $\ce{CaCl2}$/vinegar solution, or if no precipitate forms at all, you could try eliminating the vinegar (skip step $1$) and just dissolve the $\ce{CaCl2}$ in tap water.

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Prepare a solution of table salt in boiling water until no more salt will dissolve. You can then transfer the solution to a different container and allow for the solution to cool. The salt should precipitate out. You should get about 10% of the total salt to precipitate out on cooling.

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