Water Hardness and pH in the Freshwater Aquarium
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Water Hardness and pH in the Freshwater Aquarium

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Water Hardness and pH in the Freshwater Aquarium
Old 05-26-2013, 08:38 PM   #1
 
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Water Hardness and pH in the Freshwater Aquarium

Water in its pure form does not exist in nature; it is a powerful solvent, meaning a substance that easily dissolves other substances to create a solution. As rain falls, it picks up many gasses and particulate matter, and it continues to do this as it passes through the ground. Natural water values therefore vary with respect to hardness and pH because the water acquires specific properties from the landscape. Water flowing over or through rock will assimilate minerals from the rock, becoming what we term “hard” water. Water flowing through soils that contain organic matter will be “soft” because the organics bind with and thus remove minerals while creating acids that enter the water. The pH is largely the result of the hardness as well as the amount of carbon dioxide dissolved in the water.

As each freshwater fish species has evolved over thousands of years, their physiology has adjusted to the water values that occur in their respective habitat. We refer to these values as water parameters, and they include hardness, pH and temperature; each of these has an impact on fish. As an ecological example of this, it is hypothesized that the distinct Corydoras species that are endemic to specific tributary streams of the Rio Negro in Amazonia but are not found in the main river or in adjoining tributary streams is likely due to differing parameters including pH and temperature that act as a barrier to the fish. [1] While many fish species appear to be somewhat adaptable, their physiology can be negatively affected if the parameters are outside the fish’s natural preference. Providing suitable water parameters in the aquarium is therefore an important aspect of providing an environment that is less stressful—and this directly relates to healthier fish.

Total Dissolved Solids [TDS] is the measure of all inorganic and organic substances in suspecnded form in the water. This includes the minerals salts. "Salts" here refers not to our common salt (sodium) but to various mineral salts, the most prevalent of which are chlorides, bicarbonates, carbonates, and sulphates of calcium, sodium, magnesium and potassium. Fish are directly impacted by TDS. In fact, when we speak of soft water fish, we are actually referring to the very low, sometimes near zero, level of TDS in their water.

Water hardness is the measure of dissolved mineral salts in the water, a portion of the TDS. There are two basic types of hardness of importance to aquarists, termed general hardness (abbreviated GH) and carbonate hardness (abbreviated KH, from the German “karbon” [carbon]). The combined GH and KH is sometimes termed “total hardness,” but this is of less importance because the GH and KH individually impact the water in different ways.

General Hardness is basically determined by the minerals calcium and magnesium; GH is sometimes referred to as “permanent hardness” because it cannot be removed from water by boiling as can KH. GH is measured in several different units, but in the hobby the most common are parts per million (ppm) and degrees (dH or dGH). One dGH equals 10 milligrams of calcium or magnesium oxide per litre [2], and is equivalent to 17.848 ppm. Multiplying dGH by 17.9 gives ppm, and similarly dividing ppm by 17.9 gives dGH [the same formula works for KH]. The following chart equates the degrees and relative ppm to common terms in the hobby.

0 - 4 dGH 0 - 70 ppm very soft
4 - 8 dGH 70 - 140 ppm soft
8 - 12 dGH 140 - 210 ppm medium hard
12 - 18 dGH 210 - 320 ppm fairly hard
18 - 30 dGH 320 - 530 ppm hard
over 30 dGH over 530 ppm very hard

Fish are directly impacted by GH and TDS; their growth, the transfer of nutrients and waste products through cell membranes, spawning (sperm transfer, egg fertility or hatching), and the proper functioning of internal organs such as the kidneys can all be affected.

Carbonate hardness is the measure of carbonate and bicarbonate ions; carbonates and bicarbonates are the salts of carbonic acid. It is sometimes referred to as Alkalinity [not to be confused with alkaline as in pH, something very different]. Carbonate hardness is also measured most often in either degrees (dKH) or parts per million (ppm), and the same formula to convert dGH to ppm and reverse also works for KH. KH is normally tied to the GH, since carbonate minerals include limestone, dolomite, calcium and calcite. Mollusc shells and coral are primarily calcium. Carbonate hardness is sometimes called “temporary hardness” because it can be removed from water by boiling which precipitates out the carbonates.

KH has no direct impact on fish; but it does “buffer” the pH by binding to additions of acids or bases, keeping the pH stable—or more correctly, preventing it from changing—and the higher the KH, the greater the buffering capacity. A simple way is to think of the buffer as a sponge that soaks up the acid being added; however, at some point it will become saturated, and further additions of the acid can then cause a sudden and very large fluctuation which is usually fatal to the fish. This buffering is why attempts to adjust (lower) the pH of hard water are dangerous and will fail unless the KH is first reduced.

pH stands for pondus hydrogeni, Latin for “potential of hydrogen.” Water is made up of positively-charged hydrogen ions and negatively-charged hydroxyl ions, and pH is the measurement of the ratio of hydrogen and hydroxyl ions in a body of water. Acidic water contains more hydrogen ions, and basic (alkaline) water more hydroxyl ions; neutral water has an equal proportion. The pH is closely linked with the level of carbon dioxide (CO2) because CO2 produces carbonic acid. The hardness also impacts pH, since the carbonates bind to acids as they appear; as mentioned previously, this buffering will prevent or limit changes in pH.

The pH is measured with a scale from 1 to 14 with 7 being neutral. Numbers below 7 indicate acidic water, increasingly more acidic as they lower, while numbers above 7 indicate basic or alkaline water, increasingly as the numbers rise. This scale is logarithmic, meaning that each unit is a ten-fold increase/decrease; so a pH of 5 is ten times more acidic than a pH of 6, and 100 times more acidic than a pH of 7, and a thousand times more acidic than a pH of 8. Fish must never be exposed to sudden pH changes approaching one unit, as this is very stressful and may kill some species.

The impact of pH on fish is significant; water constantly enters the fish via osmosis through the cells, and the pH of the water can shift the pH of the fish’s blood if they are different. The fish must therefore regulate its internal pH accordingly, and this takes energy. Fish do this regularly in nature in response to changes in its environment, but these are usually minimal. Some fish species have a wider range of tolerance than others, for reasons that are not certain.[3] Fish that are wild caught show intolerance for hardness and pH levels that are not close to their origins. Maintaining a species in water that is reasonably close to its natural habitat is usually advisable.

Adjusting water hardness and/or pH should only be done by natural means, never with chemicals and preparations because these will often be “blocked” by the initial KH and may have or lead to other effects that can be highly detrimental to fish and bacteria. Water should always be prepared outside the aquarium and then used to gradually replace the aquarium water over a period of time to avoid shock to the fish.

Hard water can be made softer by diluting it; Reverse Osmosis (RO) water, distilled water, and rainwater can be used. Water will soften in proportion to the dilution; mixing hard tap water half and half with one of the afore-mentioned waters will result in water that is half the original hardness. A caution on home water softeners: many of these work by replacing the calcium [Ca] and magnesium [Mg] ions with sodium (=common salt) [Na] ions. Each Ca and Mg ion is exchanged for two Na ions. Therefore, the end result is water containing twice the ions--or double the total dissolved solids--it previously had, and for soft water fish this is an even worse situation, plus there is the detrimental impact of the sodium (salt).


Soft water can be made harder by using calcareous substances in the filter (preferably) or the substrate. Dolomite is the best, since it is composed of both calcium and magnesium. Crushed coral, marble and limestone also work but need to be in crushed form (grzavel, sand) to have more of an effect. If these latter are used, magnesium can be added with Magnesium Sulphate [pure Epsom Salt] at each water change; very little is needed. The amount required can vary depending upon the softness of the original water, but in general, very little calcareous material is required.

Adjusting pH should not be attempted except in conjunction with altering the GH and KH, since these are closely related. Most municipal water supplies will be medium hard to hard with a correspondingly higher pH in the basic range (7-9). It would not normally be necessary to raise this further, but if the tap water range is medium hard with a pH in the 7’s, adding a calcium or magnesium base to increase both the GH and KH will naturally result in a higher pH, as one might do for rift lake cichlids.

The GH and KH will remain steady once adjusted, provided no substances to increase it are present in the aquarium. Once the KH is low, the pH will naturally lower due to the carbonic acid being added to the water from natural biological processes such as fish and plant respiration, bacteria through the breakdown of organics such as fish waste, uneaten food, plant matter, etc. Regular partial water changes using either similarly-prepared water or even tap water [in smaller amounts] should not overly impact the hardness and pH if the tank is biologically stable.

A final comment on using baking soda (sodium bicarbonate) to raise pH. This can be useful in an emergency, but should not be used long-term. Sodium bicarbonate has no effective buffer action and cannot stabilize pH when additional acids are being produced such as by waste products. Further, the sodium ions will eventually reach levels that are intolerable for soft water fish (Weitzman et al. 1996). Commercial preparations such as rift lake mineral salts and others are effective though they are very expensive long term or in larger aquaria.

Footnotes:

[1] Sands (1995), p. 9.
[2] Baensch & Riehl (1987), p. 29.
[3] Muha (2006), p. 68

References:

Baensch, Hans A. and Rudiger Riehl (1987), Aquarium Atlas, Volume 1, First English Edition.

Ghadially, Feroze N. (1969), Advanced Aquarist Guide, The Pet Library Ltd.

Hiscock, Peter (2003), Encyclopedia of Aquarium Plants, Interpet Publishing, First Edition for the United States and Canada by Barron’s Educational Series, Inc.

Hiscock, Peter (2003), Aquarium Designs Inspired By Nature, Interpet Publishing, First Edition for the United States and Canada by Barron’s Educational Series, Inc.

Muha, Laura (2006), “The Skeptical Fishkeeper,” Tropical Fish Hobbyist, April 2006, pp. 66-69.

Sands, David D. (1995), “Four New Corydoras (Callichthyidae) species from Upper Negro River tributaries and a range extension, together with a discussion of C. bicolor Nijssen & Isbrucker,” Freshwater and Marine Aquarium, Volume 18, Number 7 (July 1995), pp. 8-18.

Weitzman, Stanley H., Lisa Palmer, Naercio A. Menezes and John R. Burns (1996), "Maintaining Environmental Conditions Suitable for Tropical and Subtropical Forest-adapted Fishes, Especially the Species of Mimagoniates," Tropical Fish Hobbyist, Volume 44, No. 11, June 1996 (Part One), pp. 184-194 and July 1996 (Part Two), pp. 196-201.

Byron Hosking
June 19, 2011
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