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Old 04-02-2014, 05:12 AM   #151
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pH is appx neutral and kH currently around 2, but it changes. A couple months ago kH was 0. I haven't done the 24 hour tap test in a long time.

Why has no one studied what dkh levels typical hold what ph levels? That would have been useful right now
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Old 04-02-2014, 05:14 AM   #152
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Why has no one studied what dkh levels typical hold what ph levels? That would have been useful right now
It would be quite instrumental

Do you have the numbers for how much bicarbonate of soda increases pH? Have you seen that somewhere?
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Old 04-02-2014, 05:15 AM   #153
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It would be quite instrumental

Do you have the numbers for how much bicarbonate of soda increases pH? Have you seen that somewhere?

No I'm looking as we speak. I've tried dkh to ph chart in google so far
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Old 04-02-2014, 05:17 AM   #154
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No I'm looking as we speak. I've tried dkh to ph chart in google so far

I think reef system keepers may have a closer idea as their ph and alkalinity is fairly critical.
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Old 04-02-2014, 05:23 AM   #155
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I suppose you could calculate how much bicarb is required to raise dkh by 1 then see how much ph has increased. Keep doing that to see if it's a linear rise
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Old 04-02-2014, 05:41 AM   #156
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"Sodium bicarbonate drives the pH towards an equilibrium value of 8.2."

Does that mean that is as high as it will go?
To the kitchen to dump baking soda in water! :P

OK except not right now too busy
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Old 04-02-2014, 05:50 AM   #157
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"Baking soda rests around 8.4 on the pH scale, slightly above the neutral mark of 7. The effect of baking soda will be influenced by the current pH of your water--you will not be able to raise the pH above 8.4
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Old 04-02-2014, 05:52 AM   #158
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I mean this is saying to me that we can't raise it above 8.4
And adding baking soda raises the kH.

7.14 parts of alkalinity are required for each part of ammonia to be removed. What is a "part" of alkalinity expressed as a dkH? (you figure this out somewhere right, I swear you have posted it)

we should be able to figure this out since the pH will not go above 8.4 and that is fine.
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Old 04-02-2014, 05:54 AM   #159
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OK. CaCO3 is what they use to determine alkalinity. But baking soda doesn't have any Ca. So I'm confused. How is it raising the kH?

Do I only count the CO3? I have a calculator for this. If we need 7.14ppm CO3 for each 1ppm ammonia, I can calculate that.
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Old 04-02-2014, 06:01 AM   #160
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I have an idea about cycle stalls. We always ask people like, oh did your pH crash etc. But it's not the pH that gets "eaten" it's the alkalinity. It's the CARBONATE. In hard water this is usually CaCO3. With baking soda it's NaHCO3. What if people's cycles tend to stall when their carbonates are 0 even if they haven't seen a pH crash? The pH goes down because the nitrifying bacteria produce acid. It's not because they eat the pH itself. They eat the kH. What if all of the kH is gone, so the pH hasn't crashed, but they are stalled.
I have never once asked someone to check their kH. Not once.

Am I... crazy? Am I right? is this a potential breakthrough?
We never advise adding baking soda if pH isn't a problem...
but what if they have ZERO KH LEFT
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