Second New DIY Two Part Recipe with Higher pH Boost

[Chrisanthellae]

That might be calcium carbonate precipitation.

One would not normally expect substantial precipitation if these are accurate, but perhaps the local pH is getting too high. Where are you measuring that pH?

Do you really mean +/- 0.4? It gets up to 8.55 and down to 7.75?

• pH: 8.15 (+/- 0.4, Pinpoint monitor)
• Alk: 7.4 (Salifert), 7 (API)
• Calcium: 400 (API)
• Mag: 1540 (Salifert)
• Temperature: 76-77

Oops! No, I meant +/- 0.04, so always between 8.1 and 8.2. It is very stable at all times of day (fuge on inverse cycle). The pH probe is in my skimmer chamber, so any additions are mixed thoroughly in the tank before coming back around through the sump. My sump layout is MBBR -> Skimmer/Heater/Carbon -> Fuge -> Return Pump/ATO/Doser.


Yesterday, I raised the water level in the return chamber and added an old aqueon powerhead. Hoping the increased local water volume + really fast mixing will help. I still see the gel-like globs from the NaOH solution but they are small and instantly spread throughout the chamber. For reference, when I dose the soda ash solution it now dissolves so fast I don't even see the typical white cloud. Fingers crossed!

 

[Randy Holmes-Farley]

Yesterday, I raised the water level in the return chamber and added an old aqueon powerhead. Hoping the increased local water volume + really fast mixing will help. I still see the gel-like globs from the NaOH solution but they are small and instantly spread throughout the chamber. For reference, when I dose the soda ash solution it now dissolves so fast I don't even see the typical white cloud. Fingers crossed!

Sounds good. Let us know what happens.

 

[Justin Swinney]

What is the recycling code on the bottom of the jug?

RO tubing is often polyethylene, which is fine.

It says hdpe

 

[Randy Holmes-Farley]

It says hdpe

High Density Polyethylene. It’s perfect.

 

[dadarara]

Hi all
little confused

I bought the Magnesium Sulphate MgSO4 as a powder.
so what's the difference with magnesium sulfate heptahydrate, which is MgSO4 - 7H2O .
It includes 7 parts of water ? am I correct?
So if I don't have this , how does that affect the measurements ?

Aslo, really confused about the CUP measurements.
"magnesium sulfate heptahydrate (3 cups) and magnesium chloride hexahydrate (5 cups) in enough purified freshwater to make 1 gallon total volume."

how much is the CUP. some said its 236gr. so whats the correct number?

Generally speaking, I understand that its kind of trial and error thing. I need to dose and measure. to get over time, the right dosage for the particular conditions of my tank.
But would really like to have the correct ratio to limit the number of "ERRORs" , I think.

 

[Randy Holmes-Farley]

Hi all
little confused

I bought the Magnesium Sulphate MgSO4 as a powder.
so what's the difference with magnesium sulfate heptahydrate, which is MgSO4 - 7H2O .
It includes 7 parts of water ? am I correct?
So if I don't have this , how does that affect the measurements ?

Aslo, really confused about the CUP measurements.
"magnesium sulfate heptahydrate (3 cups) and magnesium chloride hexahydrate (5 cups) in enough purified freshwater to make 1 gallon total volume."

how much is the CUP. some said its 236gr. so whats the correct number?

Generally speaking, I understand that its kind of trial and error thing. I need to dose and measure. to get over time, the right dosage for the particular conditions of my tank.
But would really like to have the correct ratio to limit the number of "ERRORs" , I think.

Do you have a link to the description of the mag powder you have? magnesium sulfate heptahydrate is a powder/granular material, despite all the water.

A "cup" is exactly 236.6 mL. In the case of this recipe, it is also 8 ounces (by coincidence). Here's where that came from when the recipe was only magnesium sulfate (it's improved now with magnesium chloride)

Part 3: The Magnesium Sulfate​

Dissolve a 64 ounce container of Epsom salts (about 8 cups) in enough purified fresh water to make 1 gallon total volume.

 

[dadarara]

unfortunately I don't have the description, cause I bought it at a local store that sells lots of chemicals etc..
I am confidant its ok cause he said many people buy from him particularly for aquariums
He just gave me "magnesium sulfate" and MgSO4 is written on the bottle.
So should I assume its "clean" and without the 7H2O ?
Let's assume it is for a moment. how does that may affect my calculations ?
Not being a chemist , I assume it's the same chemical stuff , just without water. Hope I am right.

 

[Randy Holmes-Farley]

unfortunately I don't have the description, cause I bought it at a local store that sells lots of chemicals etc..
I am confidant its ok cause he said many people buy from him particularly for aquariums
He just gave me "magnesium sulfate" and MgSO4 is written on the bottle.
So should I assume its "clean" and without the 7H2O ?
Let's assume it is for a moment. how does that may affect my calculations ?
Not being a chemist , I assume it's the same chemical stuff , just without water. Hope I am right.

It's more likely the hydrate. The anhydrous material is more expensive and has to be heated to drive off the water.

Magnesium sulfate - Wikipedia

en.wikipedia.org

"Magnesium sulfate is usually encountered in the form of a hydrate MgSO4·nH2O, for various values of n between 1 and 11. The most common is the heptahydrate MgSO4·7H2O, known as Epsom salt, which is a household chemical with many traditional uses, including bath salts."

Anyway, dissolve some in water and see if it gets warm. If so, it is not the hydrate.

Here's someone testing both:

Enthalpy of Hydration Between MgSO4 and MgSO4 ∙ 7 H2O — Adam Cap

Introduction Enthalpy of hydration is the energy change for converting 1 mol of an anhydrous substance to 1 mol of the hydrated substance. In order to find this number, it is necessary to first calculate the enthalpy of dissolution for each substance separately, and then find the different...

adamcap.com

 

[dadarara]

thank you so much Randy amazing how detailed your answers are.
What I have omitted from my description above was that I bought several chemicals.

Calcium Hydroxide

Calcium CHLORIDE CaCl2

Magnezium SULFATE - Epsom salt - MgSO4

Magnezium CHLORIDE MgCl2

Sodium BICARBONAT NaHCOO3

So as you can see, I got both the Mag Sulfate and Chloride. I will be calling the store to ask them of course.
probably it is some sort of form of hydrate. And as a most common is 7H2O. most probably this is what I have.

But just to be sure about my next steps.
Please confirm that it does not make a huge difference, in terms of the final result. Though of course maybe the concentration in water might be different. Is this assumption correct ?

 

[Randy Holmes-Farley]

The mag sulfate is the hydrate. Epsom salt is the hydrate. Not sure on the mag chloride, and calcium chloride, but I would guess those are as well.

The mag compounds are half water by weight, so it does make a difference. The water heat test works for all of them.

 

[Justin Swinney]

Also, I am currently doing the brs/tropic marin hybrid with the k trace in the calcium and a trace in soda ash. If I put the a elements in the sodium hydroxide will they precipitate put in the extreme high ph?

 

[e34stx]

sorry do i still require dosing mag with the part c? thanks

 

[thatmanMIKEson]

sorry do i still require dosing mag with the part c? thanks

Yes, its not a magnesium substitute

 

[Randy Holmes-Farley]

sorry do i still require dosing mag with the part c? thanks

If you use part C at the directed dose, you do not use my part 3 at it’s directed dose, although my Part 3 is fine to use for a mag boost if it drops below your target despite Part C.

 

[Randy Holmes-Farley]

Yes, its not a magnesium substitute

That's technically true, but Part C is mostly magnesium sulfate (plus other stuff).

 

[e34stx]

Thanks chap

 

[Dan I]

Hey @Randy Holmes-Farley just finished mixing up your recipe. I'm pretty sure you answered this I couldn't find it if you did. My calcium mix came out brown tint, and it should be fine to dose right. I used the calcium chloride I linked earlier. Also, I just found that you recommended to mix 20% less than your recipe after I mixed this because this is anhydrous calcium chloride. Should I dump this batch and do a new one following that instruction?

 

[Randy Holmes-Farley]

Yes, calcium sometimes has some brown. Possible from traces of iron oxide.

 

[Dan I]

Yes, calcium sometimes has some brown. Possible from traces of iron oxide.

I just edited my post. Don't know if you saw the second part. I mixed this using with the anhydrous calcium chloride and used 500grams. I noticed you recommended to use 20% less when using this product. Should I dump this mix and make a new one?

 

[Randy Holmes-Farley]

I just edited my post. Don't know if you saw the second part. I mixed this using with the anhydrous calcium chloride and used 500grams. I noticed you recommended to use 20% less when using this product. Should I dump this mix and make a new one?

No. Just use a little less or add more water.