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The artificial solution described by Dennis Hoagland in 1933, [1] known as Hoagland solution (0), has been modified several times, mainly to add ferric chelates to keep iron effectively in solution, [6] and to optimize the composition and concentration of other trace elements, some of which are not generally credited with a function in plant nutrition. [7]
Ferric EDTA can be used as a component for the Hoagland solution or the Long Ashton Nutrient Solution. [7] According to Jacobson (1951), [2] the stability of ferric EDTA was tested by adding 5 ppm iron, as the complex, to Hoagland's solution at various pH values. No loss of iron occurred below pH 6.
Standard solutions are generally prepared by dissolving a solute of known mass into a solvent to a precise volume, or by diluting a solution of known concentration with more solvent. [1] A standard solution ideally has a high degree of purity and is stable enough that the concentration can be accurately measured after a long shelf time. [2]
The United States has established a secondary water quality standard of 500 mg/L to provide for palatability of drinking water. Total dissolved solids are differentiated from total suspended solids (TSS), in that the latter cannot pass through a sieve of 2 micrometers and yet are indefinitely suspended in solution.
Fluorescein aqueous solutions, diluted from 10,000 to 1 parts-per-million in intervals of 10 fold dilution. At 1 ppm the solution is a very pale yellow. At 1 ppm the solution is a very pale yellow. As the concentration increases the colour becomes a more vibrant yellow, then orange, with the final 10,000 ppm a deep red colour.
Solution (2) contains ammonium and nitrate salts and may sometimes be preferred to solution (0, 1) (cf. Table 2) because the ammonium ion delays the development of undesirable alkalinity (Hoagland and Arnon, 1938, 1950). However, it is toxic to most crop species and is rarely applied as a sole nitrogen source. [20]