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Post subject: Bleach Freezing Point & Consequences
Posted: December 7th, 2007, 6:00 pm
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Joined: October 8th, 2007, 2:34 pm
Posts: 4
What happens if Regular 6% Bleach freezes? I have about 20 gallons in 182 oz bottles out in the garage. Bringing them in is possible but I'd rather not but if it will lose it's CL I'll do it.

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Post subject:
Posted: December 7th, 2007, 6:19 pm

Joined: May 30th, 2007, 8:57 pm
Posts: 9117
Location: South Carolina
Hi jakebear and welcome to TFP!

....not to hijack your thread, but perhaps the responders could also include info on the freezing point of muriatic acid! I know there is a thread out here somewhere , just can't seem to find it!

Again, welcome.

Joyce

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Post subject:
Posted: December 7th, 2007, 7:59 pm
 TFP Expert

Joined: March 28th, 2007, 2:40 pm
Posts: 8087
Location: San Rafael, CA USA
Taking the info from posts I made on The Pool Forum:

The freezing point depression of a 12% Sodium Hypochlorite solution (which also has 9.4% salt due to the manufacturing process of chlorine) is 15.3C or 27F so the freezing point is -15.3C or 5F. So unless you are expecting sustained temperatures well below freezing (i.e. closer to 5 degrees Fahrenheit or below), then it should be safe.

The full calculation was determined from the following. 12% solution is (approximately; ignoring Trade % vs. weight % distinctions) 12 grams of sodium hypochlorite in 100 grams total. There is also 12*58.443/74.4422 = 9.42 grams of salt (from the way chlorine is produced) so that's 100-12-9.42 = 78.58 grams water. There is 12/74.4422 = 0.1612 moles times 4 for dissociation and salt (there is sodium, hypochlorite, sodium, chloride) so 0.6448 moles solute in 78.58 grams water so in 1000 grams (1 kilogram) that is 8.2 so that times 1.86 is 15.3C = 27F.

The full calculation for bleach is determined from the following. 6% solution is (assuming weight %) is 6 grams of sodium hypochlorite in 100 grams total. There is also 6*58.443/74.4422 = 4.71 grams of salt (from the way chlorine is produced) so that's 100-6-4.71 = 89.29 grams water. There is 6/74.4422 = 0.0806 moles times 4 for dissociation and salt (there is sodium, hypochlorite, sodium, chloride) so 0.3224 moles solute in 82.29 grams water so in 1000 grams (1 kilogram) that is 3.92 so that times 1.86 is 7.3C = 13.1F.

The freezing point depression for 6% Sodium Hypochlorite as found in Clorox Regular and most Ultra brands of bleach is 7.3C or 13.1F so the freezing point is -7.3C or 19F.

The freezing point of full-strength Muriatic Acid (31.45% Hydrochloric Acid) is -46C (-50.8F) (for Hasa; other brands quote even lower freezing points) so unless you live in the Artic, I think you are safe to leave your Muriatic Acid outside.

[EDIT] The freezing point of half-strength Muriatic Acid (say, 15% Hydrochloric Acid) is -18C (-0.4F). [END-EDIT]

Richard

Last edited by chem geek on September 11th, 2012, 2:59 pm, edited 2 times in total.

Post subject:
Posted: December 7th, 2007, 8:44 pm
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Joined: March 29th, 2007, 11:56 am
Posts: 4160
Location: Coastalish 'down easter'
Thank you Richard Most of us may not be able to follow the full "freezing point depression" causes, but with solid numbers, ie, 5F, it doesn't take an advanced degree to understand

Thanks again for all the info you provide

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Post subject:
Posted: December 13th, 2007, 7:18 pm
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Joined: October 8th, 2007, 2:34 pm
Posts: 4
Thanks to all -- Guess I'll move it in when the temp drops

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