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pH in Hydroponics
 

 

pH Affects Plant

pH affects plant growth and nutrient availability.

bulletpH can affect the availability of nutrients.
bulletpH can affect the absorption of nutrients by plant roots
bulletpH values above 7.5 cause iron, manganese, copper, zinc and boron ions to be less available to plants.
bulletpH values below 6 cause the solubility of phosphoric acid, calcium and magnesium to drop.
bulletpH values between 3 and 5 and temperatures above 26OC encourage the development of fungal diseases.

Why pH Varies

The ratio in uptake of anions (negatively charged nutrients) and cations (positively charged nutrients) by plants may cause substantial shifts in pH. In general, an excess of cation over anion leads to a decrease in pH, whereas an excess of anion over cation uptake leads to an increase in pH. As nitrogen (an element required in large quantities for healthy plant growth) may be supplied either as a cation (ammonium - NH4+) or an anion (nitrate - NO3-), the ratio of these two forms of nitrogen in the nutrient solution can have large effects on both the rate and direction of pH changes with time. This shift in pH can be surprisingly fast.

Daylight photosynthesis produces hydrogen ions which can cause the nutrient acidity to increase (lowering the pH). At dusk photosynthesis stops and the plants increase their rate of respiration and this coupled with the respiration of micro organisms and the decomposition of organic matter uses up the hydrogen ions so the acidity of the solution tends to decrease (pH rises).

Most varieties of vegetables grow at their best in a nutrient solution having a pH between 6.0 and 7.5 and a nutrient temperature between 20 and 22OC.

In low light (overcast days or indoor growing environments) plants take up more potassium and phosphorous from the nutrient solution so the acidity increases (pH drops). In strong intense light (clear sunny days) plants take up more nitrogen from the nutrient solution so the acidity decreases (pH rises).

Extremes in pH can result in precipitation of certain nutrients.

For plant roots to be able to absorb nutrients, the nutrients must be dissolved in solution. The process of precipitation (the reverse of dissolving) results in the formation of solids in the nutrient solution, making nutrients unavailable to plants. Not all precipitation settles to the bottom of the tanks, some precipitates occur as very fine suspension invisible to the naked eye.

Plants can tell us their problems through leaf symptoms (e.g. Iron deficiency) when it's too late. Iron is one essential plant nutrient whose solubility is affected by pH which is why it is added in a chelated form (or daily). Iron deficiency symptoms occur readily. At pH values over 7, less than 50% of the Iron is available to plants. At pH 8.0, no Fe is left in solution due to iron hydroxide precipitation (Fe(OH)3 - which eventually converts to rust). As long as the pH is kept below 6.5, over 90% of the Iron is available to plants.

Varying pH of summer lettuce nutrient solutions also affects the solubility of calcium (Ca) and phosphorus (P). Due to calcium phosphate precipitation (Ca3(PO4)2) the availability of calcium and phosphorus decreases at pH values above 6.0. All other nutrients stay in solution and do not precipitate over a wide pH range. Poor water quality could exacerbate any precipitation reactions that may occur.

Generally in the pH range 4.0 to 6.0, all nutrients are available to plants. Precipitation reduces Iron, Calcium and Phosphorus availability at pH 6.0 and over .

Adjusting pH

The addition of acids or alkalis to nutrient solutions is the most common and practical means to adjust pH, and can be easily automated. See our hydroponics controller . There are ways to minimize pH variations and they are worth some consideration.

Nitrogen is the essential inorganic nutrient required in the largest quantity by plants. Most plants are able to absorb either nitrate (NO3-) or ammonium (NH4+) or both. NH4+ as the sole source of nitrogen or in excess is deleterious to the growth of many plant species. Some plants yield better when supplied with a mixture of NH4+ (ammonium) and NO3- (nitrate) compared to NO3- alone. A combination of NH4+ and NO3- can be used to buffer against changes in pH.

Plants grown in nutrient solution containing only NO3- as the sole nitrogen source tend to increase solution pH - hence the need to add acid. But when approximately 10%-20% of the total nitrogen is supplied as NH4+, the nutrient solution pH is stabilized at pH 5.5. NH4+ concentration needs to be monitored as it has been shown recently that micro-organisms growing on plant root surfaces can convert the NH4+ to NO3-. Since hand-held ion-selective electrodes for measuring both NH4+ and NO3- are now available, it should be possible to accurately monitor and maintain a predetermined NO3-/NH4+ ratio throughout the life of the crop.

Phosphorus is required in large amounts by plants. Interestingly, there are two forms of fertilizers containing both K and P - KH2PO4 mono-potassium phosphate (MKP) and K2HPO4 di-potassium phosphate. Equal quantities of both can be used to maintain the pH at 7.0. Using a higher proportion of K2HPO4 increases pH. MKP can be used to lower the solution pH.

Buffers are solutions which resist pH change and are used to calibrate pH electrodes. Buffers can be added to nutrient solutions in an attempt to maintain pH stability. One such buffer is called 2-(N-morpholino) ethanesulfonic acid - abbreviated to MES. Many of the companies who claim better pH control with their 'specially' formulated nutrient solutions add MES to their mixes. It is important to remember when using MES, that after MES addition the pH is low and needs to be adjusted to your required level with an alkali such as potassium hydroxide (KOH).

Another method of pH stabilization is to use ion- exchange and chelating resins. Generally, these resins are small beads which have nutrients absorbed or chelated onto them - the nutrient solution circulates through the beads or the beads can be suspended in the nutrient tank. As plants absorb nutrients, more nutrients are released by the resins. The aim is to achieve controlled release of nutrients into the solution in an attempt to mimic the way the soil releases nutrients. Ideally, such release can adequately supply the growing plants' nutritional requirements and maintain pH stability.

Is pH Adjustment Critical?

pH is not as critical as most hydroponicists believe. The main point is to avoid extremes in pH. Plants grow on soils with a wide range of pH. For most plant species there is an optimum pH in the region of pH 5 to pH 6

References - Nothing beats a good book

Asher, C.J. (1978). Natural and synthetic culture media for spermatophytes. CRC Handbook Series in Nutrition and Food. Ed. Miloslav Rechigl, Jr. CRC Press Inc., Cleveland, Ohio. Vol 3, 575- 609.

Bates, R.G. (1981). The modern meaning of pH. CRC Critical Reviews in Analytical Chemistry 11; 247-278.

Errebhi, M. and Wilcox, C.A. (1990). Plant species response to ammonium - nitrate concentration ratios. Journal of Plant Nutrition. 13 (8): 1017-1029.

Ficks, J. and Mitchell, C.A. (1993). Stabilisation of pH in solid-matrix hydroponic systems. HortScience, 28 (10): 981-984.

Haynes, R.J. and Goh, K.M. (1978). Ammonium and nitrate nutrition of plants. Biology Reviews, 53: 465-510.

Huett, D.O. (1994). Growth, nutrient uptake and tipburn severity of hydroponic lettuce in response to electrical conductivity and K:Ca ratio in solution. Australian Journal of Agricultural Research 45: 251-267.

Padgett, P.E. and Leonard, R.T. (1993). Contamination of ammonium-based nutrient solutions by nitrifying organisms and the conversion of ammonium to nitrate. Plant Physiology 101: 141-146.

Parker, D.R., Norvell, W.A., and Chaney, R.L. (1993). GEOCHEM-PC: a chemical speciation program for IBM and compatible personal computers. In R.H. Leoppert, ed, Chemical Equilibrium and Reaction Models, Soil Science Society of America special publication. Madison, WI (in press).

Sposito, G. and Mattigod, S.V. (1980). GEOCHEM: A computer program for the calculation of chemical equilibria in soil solutions and other natural water systems. The Kearney Foundation of Soil Science, University of California, Riverside, California.

Welch, R.M. (1990). Modern technologies for studying the requirements and functions of plant mineral nutrients. Measurement Techniques in Plant Science, Edited by Y. Hashimoto et al. Academic Press, San Diego. pp 319-342. #

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Last modified: May 27, 2013