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Household ammonia ranges in concentration by weight from 5% to 10% ammonia. [9] Because aqueous ammonia is a gas dissolved in water, as the water evaporates from a surface, the gas evaporates also, leaving the surface streak-free. Its most common uses are to clean glass [10], porcelain, and stainless steel. It is good at removing grease and is ...
Ammonium chloride is an inorganic chemical compound with the chemical formula N H 4 Cl, also written as [NH 4]Cl.It is an ammonium salt of hydrogen chloride.It consists of ammonium cations [NH 4] + and chloride anions Cl −.
What we see is formulations like "a 3:1 mixture of ammonium hydroxide (NH4OH) with hydrogen peroxide" (from article on Piranha solution). What does this say about stoichiometry? This suggests that "ammonium hydroxide" (NH4OH) should be used (if at all) only if it is really about ammonia (NH3) and water (H2O) in a 1:1 ratio, right?
Buffer capacity falls to 33% of the maximum value at pH = pK a ± 1, to 10% at pH = pK a ± 1.5 and to 1% at pH = pK a ± 2. For this reason the most useful range is approximately pK a ± 1. When choosing a buffer for use at a specific pH, it should have a pK a value as close as possible to that pH. [2]
The molar ionic strength, I, of a solution is a function of the concentration of all ions present in that solution. [3]= = where one half is because we are including both cations and anions, c i is the molar concentration of ion i (M, mol/L), z i is the charge number of that ion, and the sum is taken over all ions in the solution.
The following table presents pK a values at 20 °C. Values change by about 0.01 per degree of temperature. [1] [3] Good's original 1966 paper had two older buffers (marked with italics) for comparison.
Any condition that changes the balance of one of the buffer systems, also changes the balance of all the others because the buffer systems actually buffer one another by shifting hydrogen ions back and forth from one to the other. The isohydric principle has special relevance to in vivo biochemistry where multiple acid/ base pairs are in ...
In atmospheric chemistry, mixing ratio usually refers to the mole ratio r i, which is defined as the amount of a constituent n i divided by the total amount of all other constituents in a mixture: