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Old 04-18-2012, 06:00 PM
LawnsharkMB LawnsharkMB is offline
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Lowering PH,

What is the fastest and safest way to lower the ph of a lawn? I have 7 lawns that the ph is 7.0 to 7.4. All are centipede. I have never applied sulfur to a lawn before. I have read that aluminum sulfate is the quickest but it will burn the lawn. I know SCU and ammonium sulfate will lower the ph but doesn't this take a while? Thanks for any advice in advance.
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Old 04-18-2012, 07:49 PM
RAlmaroad RAlmaroad is online now
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Landshark:
I'm in the region also. Sulfur with 10%dolemite (clay) does a great job on our sandy soil. I buy the flakes and spread it at 10lb/K. It needs warm soil to activate it. It brakes down rather quickly. Your centipede will do great if you use ammonium sulfate (21-0-0)@ 1/2lb/K which is a sulfur based Nitrogen. I bet you are a granular guy! Luckily, it can be had in the granular form. I use 14-0-46 liquid and boost it with the ammonium + iron and micros.
Lesco has the sulfur but it is way too high. I get mine from the co-op at about half of their price. I put it down in November and then again in April and just waited on the heat.
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Old 04-18-2012, 10:35 PM
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10 pound per thousand sq ft of 0-0-0-90 Sulfur with 10% Bentonite not dolomite will lower pH one point in 30 days. pH is the inverse logarithm of the hydrogen Ion in a solution. Therefore as a Inverse, the More hydrogen atoms the lower the pH number. Small p in math stands to an inverse and the capital H stands for Hydrogen.



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Old 04-29-2012, 10:39 AM
Kiril Kiril is offline
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This is the equation for pH, it is NOT an inverse log, it is a negative log.

pH = -log [H+]

The inverse log (or better known as the exponent) of the negative of the pH is the hydrogen ion concentration.

[H+] = 10^(-pH)


Example:

If I have a [H+] = 0.0002, what is the pH?
pH = -log(0.0002) = 3.70
If I have a pH = 3.70 what is the [H+]?
[H+] = 10^(-3.70) = 0.0002

Last edited by Kiril; 04-29-2012 at 10:45 AM.
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Old 04-29-2012, 12:13 PM
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Quote:
Originally Posted by Kiril View Post
This is the equation for pH, it is NOT an inverse log, it is a negative log.

pH = -log [H+]

The inverse log (or better known as the exponent) of the negative of the pH is the hydrogen ion concentration.

[H+] = 10^(-pH)


Example:

If I have a [H+] = 0.0002, what is the pH?
pH = -log(0.0002) = 3.70
If I have a pH = 3.70 what is the [H+]?
[H+] = 10^(-3.70) = 0.0002

My Bad, I am getting old and have CRS. The negative log is a Inverse of the positive log. In the case of pH, the measurement of Hydrogen ions in a solution is a reverse of numbers. The higher the pH, the lower amount of Hydrogen ions. The lower the pH the higher the Hydrogen ion count.


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Old 04-29-2012, 01:05 PM
Kiril Kiril is offline
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logarithmic functions are inversely related to the exponential function is the easiest way to remember it, at least for me.

logbx is the inverse of b^x where b = base

I think the most important relation to remember here for most people is for every unit change in pH, there is a 10 fold change in [H+]

Using the example above, increasing pH to 4.7 reduces [H+] by a factor of 10.

[H+] = 10^(-4.70) = 0.00002

Last edited by Kiril; 04-29-2012 at 01:11 PM.
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