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Topic: NaHCO3 in water?  (Read 24588 times)

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Offline CABAL

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NaHCO3 in water?
« on: September 21, 2007, 11:44:01 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

Offline DevaDevil

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Re: NaHCO3 in water?
« Reply #1 on: September 21, 2007, 12:29:28 PM »
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.

Offline CABAL

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Re: NaHCO3 in water?
« Reply #2 on: September 21, 2007, 02:23:31 PM »

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

Offline enahs

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Re: NaHCO3 in water?
« Reply #3 on: September 21, 2007, 04:13:56 PM »
An estimate would be:
A little less then 7.0, assuming pure water.


Offline CABAL

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Re: NaHCO3 in water?
« Reply #4 on: September 21, 2007, 05:18:58 PM »

Thanks!! :)

Very nice!!


Offline Borek

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Re: NaHCO3 in water?
« Reply #5 on: September 21, 2007, 05:22:50 PM »
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, 05:55:49 PM by Borek »
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