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Author Topic: NaHCO3 in water?  (Read 13603 times)

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CABAL

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NaHCO3 in water?
« on: September 21, 2007, 05:44:01 AM »


Hey all!

If I put NaHCO3 in water, does make Na+ and HCO3- ions right away?

I'm asking because I read that plants uses the carbondioxide from the compound,
but how do they do this?

Thanks,

Nicholas
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DevaDevil

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Re: NaHCO3 in water?
« Reply #1 on: September 21, 2007, 06:29:28 AM »

sodium bicarbonate (baking soda) is soluble in water, so it will be present in ionic form. (solubility ~7.8 g/100 ml water)

(Bi)Carbonate in acidic solution will be in equilibrium with carbon dioxide and water. HCO3- + H+ <--> H2O + CO2

As far as plants go, I'll let a biologist do the talking.
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CABAL

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Re: NaHCO3 in water?
« Reply #2 on: September 21, 2007, 08:23:31 AM »


Edit: Oh, if I dissolve 10g of NaHCO3 in 1 Liter of water, what would the pH be?
(an estimate would be enough)..sorry to be so pushy!

Thanks!!

Just what I needed!

Nicholas
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enahs

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Re: NaHCO3 in water?
« Reply #3 on: September 21, 2007, 10:13:56 AM »

An estimate would be:
A little less then 7.0, assuming pure water.

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CABAL

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Re: NaHCO3 in water?
« Reply #4 on: September 21, 2007, 11:18:58 AM »


Thanks!! :)

Very nice!!

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Borek

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Re: NaHCO3 in water?
« Reply #5 on: September 21, 2007, 11:22:50 AM »

An estimate would be:
A little less then 7.0, assuming pure water.

Nope. Between 8.0 and 8.1. That's without taking

H2CO3 = CO2 + H2O

equilibrium into account, which could remove some CO2 from the solution, making it even more basic.
« Last Edit: September 21, 2007, 11:55:49 AM by Borek »
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