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Sodium carbonate (also known as washing soda, soda ash and soda crystals) is the inorganic compound with the formula Na 2 CO 3 and its various hydrates.All forms are white, odourless, water-soluble salts that yield alkaline solutions in water.
The carbonate buffer system is a series of reactions that uses carbonate as a buffer to convert into bicarbonate. [12] The carbonate buffer reaction helps maintain a constant H+ concentration in the ocean because it consumes hydrogen ions, [13] and thereby maintains a constant pH. [12]
The residual sodium carbonate (RSC) index of irrigation water or soil water is used to indicate the alkalinity hazard for soil. The RSC index is used to find the suitability of the water for irrigation in clay soils which have a high cation exchange capacity .
The following packages calculate the state of the carbonate system in seawater (including pH): CO2SYS Archived 2011-10-14 at the Wayback Machine, available as a stand-alone executable, Excel spreadsheet, or MATLAB script. seacarb, a R package for Windows, Mac OS X and Linux (also available here) CSYS, a Matlab script
Sodium percarbonate or sodium carbonate peroxide is a chemical substance with empirical formula Na 2 H 3 CO 6. It is an adduct of sodium carbonate ("soda ash" or "washing soda") and hydrogen peroxide (that is, a perhydrate ) whose formula is more properly written as 2 Na 2 CO 3 · 3 H 2 O 2 .
The pH at the end-point is greater than 7 and increases with increasing concentration of the acid, T A, as seen in the figure. In a titration of a weak acid with a strong base the pH rises more steeply as the end-point is approached. At the end-point, the slope of the curve of pH with respect to amount of titrant is a maximum.
In a solution where only CO 2 affects the pH, carbonate hardness can be used to calculate the concentration of dissolved CO 2 in the solution with the formula CO 2 = 3 × KH × 10 (7-pH), where KH is degrees of carbonate hardness and CO 2 is given in ppm by weight. [citation needed]
Acid-neutralizing capacity or ANC in short is a measure for the overall buffering capacity against acidification of a solution, e.g. surface water or soil water.. ANC is defined as the difference between cations of strong bases and anions of strong acids (see below), or dynamically as the amount of acid needed to change the pH value from the sample's value to a chosen different value. [1]