What is in supersoil? If it contains alot of bark, like alot of these mixes have as filler, then it is considered soilless. Other additives like peatmoss are also considered soilless. A higher ph is used typically in mineral soils outdoors with a range of maybe 5.8 to 6.5 A ph of of 6 will work in soil, soilless, and hydroponics. It is kind of an all purpose number.Nape said:I have 10 WW started and I have a Q on PH.
Is this mix considered soilless mix for PH purposes?
60% SuperSoil Potting mix.
20% Vermiculite
20% Perlite
Should PH be 5.8-6.2 or 6.2-7.0?
Thanks,
Sounds like the ph is high. Maybe lack of iron. Don't go applying iron though cause you will throw the balance of all your other micros out of whack. Too much iron = manganese deficiency possibly. Better to tinker with the ph. Don't forget to include some sulfur in your ferts. This could also give an overall yellowish color. It is also immobile and will affect your top leaves. Check out the thread in my signature on sulfur and ways to make sure you can include some.inc0gnit0 said:Maybe that's why my newest growth is always a lighter green, It looks much worse in the pics but it evens out as the plan grows. I'll try to get the pH down and see what happens.
Once the buffers are gone from the nutrient solution and its sitting at a certain ph, you might find that just a drop of ph down drastically will change the ph.the cult said:i got a question for someone with good knowledge of ph and buffers, so i figured id take my shot here in this thread.
when i mix nutes and add ph down i take a reading with my metre, says eg 5.5 (approx where i want to be), im happy, i leave water for 30 mins, its risen to lets say 6.2, the effect of buffers in the nute solutions. i then add a drop of ph down, and take a new reading, its all of a sudden down at 4 something. how can this be? i dont understand the process. the buffering doesnt really change the ph of the water? it appears the ph was still at 5.5 as just a drop into the solution deals a total coupe de grace to the mix and i have to add fresh water in steps to get back up to the level i want to achieve.
can anybody explain how this works and what the buffers actually do?
and yeah, i calibrate my metre every week hehe
Titration
From Wikipedia, the free encyclopedia
Titration setup: the titrant drops from the burette into the analyte solution in the flask. An indicator present then changes color at the endpoint.Titration is a standard laboratory method of quantitative/chemical analysis which can be used to determine the concentration of a known reactant. Because volume measurements play a key role in titration, it is also known as volumetric analysis. A reagent, called the titrant, of known concentration (a standard solution) and volume is used to react with a measured quantity of reactant (Analyte). Using a calibrated burette to add the titrant, it is possible to determine the exact amount that has been consumed when the endpoint is reached. The endpoint is the point at which the titration is stopped. This is classically a point at which the number of moles of titrant is equal to the number of moles of analyte, or some multiple thereof (as in di- or tri- protic acids). In the classic strong acid-strong base titration the endpoint of a titration is when the pH of the reactant is just about equal to 7, and often when the solution permanently changes color due to an indicator. There are however many different types of titrations (see below).
Many methods can be used to indicate the endpoint of a reaction; titrations often use visual indicators (the reactant mixture changes colour). In simple acid-base titrations a pH indicator may be used, such as phenolphthalein, which turns (and stays) pink when a certain pH is reached or exceeded. Methyl orange can also be used, which is red in acids and yellow in alkalis.
Not every titration requires an indicator. In some cases, either the reactants or the products are strongly coloured and can serve as the "indicator". For example, an oxidation-reduction titration using potassium permanganate (pink/purple) as the titrant does not require an indicator. When the titrant is reduced, it turns colourless. After the equivalence point, there is excess titrant present. The equivalence point is identified from the first faint pink colour that persists in the solution being titrated.
Due to the logarithmic nature of the pH curve, the transitions are generally extremely sharp, and thus a single drop of titrant just before the endpoint can change the pH significantly — leading to an immediate colour change in the indicator. That said, there is a slight difference between the change in indicator color and the actual equivalence point of the titration. This error is referred to as an indicator error, and it is indeterminate.
the cult said:i got a question for someone with good knowledge of ph and buffers, so i figured id take my shot here in this thread.
when i mix nutes and add ph down i take a reading with my metre, says eg 5.5 (approx where i want to be), im happy, i leave water for 30 mins, its risen to lets say 6.2, the effect of buffers in the nute solutions. i then add a drop of ph down, and take a new reading, its all of a sudden down at 4 something. how can this be? i dont understand the process. the buffering doesnt really change the ph of the water? it appears the ph was still at 5.5 as just a drop into the solution deals a total coupe de grace to the mix and i have to add fresh water in steps to get back up to the level i want to achieve.
can anybody explain how this works and what the buffers actually do?
and yeah, i calibrate my metre every week hehe