Please clarify the units of concentration of carbonate and bicarbonate. "mgl" is not a unit of concentration (it's not a unit of anything to my knowledge. To answer this question, you need the concentration of both ions. So either provide the amount of both ions AND the amount of water, or just specify the concentration (in unit of molarity, or moles per liter preferably).
Alkalinity primarily refers to the capacity of water to neutralize acids and is commonly categorized into three types: bicarbonate (HCO3-), carbonate (CO3^2-), and hydroxide (OH-). Bicarbonate is the most prevalent form in natural water systems, while carbonate becomes more significant at higher pH levels. Hydroxide ions contribute to alkalinity when pH levels are extremely high. Together, these forms help buffer pH changes in aquatic environments.
When an acid is neutralized by an antacid containing a carbonate or bicarbonate, carbon dioxide gas is produced as an additional product along with water and a salt.
Alkalinity is different from basicity, which is directly related to the pH. The higher the pH, the more basic the water.Like acidity, there are different ways to measure and report alkalinity;The first is to titrate the water with acid titrant to the phenolphthalein end point. This is called the phenolphthalein alkalinity. Since phenolphthalein changes color at pH~8.3, this corresponds to a pH where all the CO32- present would be protonated.Second, acid titration to a methyl orange end point, pH~4.3, further converts the bicarbonate to aqueous carbon dioxide. At this end point, some of the weaker conjugate bases are protonated. The methyl orange end point titration indicates total alkalinity.
The pH range for carbonate-bicarbonate buffer is 9,2.
You mean alkalinity? Alkalinity measures the ability of a solution to neutralize acids to the equivalence point of carbonate or bicarbonate. The alkalinity is equal to the stoichiometric sum of the bases in solution.
carbonate containing rocks
When sodium carbonate and sodium bicarbonate are titrated together, the sodium carbonate will react with the acid first due to its higher alkalinity compared to sodium bicarbonate. The sodium bicarbonate will then react next, producing carbon dioxide gas as a byproduct due to its weaker alkalinity. This reaction can be observed by the effervescence or bubbling of carbon dioxide gas during the titration.
Alkalinity refers to the capacity of water to neutralize acids and is primarily due to the presence of bicarbonate, carbonate, and hydroxide ions. The main types of alkalinity include bicarbonate alkalinity, which is the most common form found in natural waters; carbonate alkalinity, which occurs at higher pH levels; and hydroxide alkalinity, which is less common and typically found in very basic conditions. These types of alkalinity play a crucial role in maintaining pH levels and supporting aquatic life.
Phenolphthalein alkalinity measures the hydroxide ion concentration in water, specifically the amount that can be neutralized by strong acids. Total alkalinity, however, measures the water's ability to neutralize acids, including carbonate, bicarbonate, and hydroxide ions. In summary, phenolphthalein alkalinity focuses on the hydroxide ions, while total alkalinity considers a broader range of alkaline substances.
1. M-Alkalinity (also known as Total Alkalinity) measures the amount of carbonate, bicarbonate and hydroxide present in terms of "ppm as calcium carbonate". ( M-Alkalinity measurement is based on a sulphuric acid titration using a Methyl orange indicator that goes from yellow at a pH of 4.5 to orange at pH of 4.4 at the endpoint.) 2. P-Alkalinity measures the amount of carbonate and hydroxyl alkalinity present in terms of "ppm as calcium carbonate". P-alkalinity is measured down to a pH of 8.3. The M-alkalinity is measured down to a pH of 4.3.
Alkalinity of water is its acid-neutralizing capacity. It is the sum of all titratable bases. Because the alkalinity of many surface water is primarily a function of carbonate, bicarbonate and hydroxide content, it is taken as an indication of the concentration of these constituent.
The carbonate alkalinity would be higher in temporary hard water compared to permanently hard water. Temporary hard water primarily contains bicarbonate ions, which contribute to the carbonate alkalinity, while permanently hard water contains other ions, such as sulfate or chloride, which do not significantly contribute to carbonate alkalinity.
1. M-Alkalinity (also known as Total Alkalinity) measures the amount of carbonate, bicarbonate and hydroxide present in terms of "ppm as calcium carbonate". ( M-Alkalinity measurement is based on a sulphuric acid titration using a Methyl orange indicator that goes from yellow at a pH of 4.5 to orange at pH of 4.4 at the endpoint.) 2. P-Alkalinity measures the amount of carbonate and hydroxyl alkalinity present in terms of "ppm as calcium carbonate". P-alkalinity is measured down to a pH of 8.3. The M-alkalinity is measured down to a pH of 4.3.
Alkalinity primarily refers to the capacity of water to neutralize acids and is commonly categorized into three types: bicarbonate (HCO3-), carbonate (CO3^2-), and hydroxide (OH-). Bicarbonate is the most prevalent form in natural water systems, while carbonate becomes more significant at higher pH levels. Hydroxide ions contribute to alkalinity when pH levels are extremely high. Together, these forms help buffer pH changes in aquatic environments.
When an acid is neutralized by an antacid containing a carbonate or bicarbonate, carbon dioxide gas is produced as an additional product along with water and a salt.
Alkalinity is different from basicity, which is directly related to the pH. The higher the pH, the more basic the water.Like acidity, there are different ways to measure and report alkalinity;The first is to titrate the water with acid titrant to the phenolphthalein end point. This is called the phenolphthalein alkalinity. Since phenolphthalein changes color at pH~8.3, this corresponds to a pH where all the CO32- present would be protonated.Second, acid titration to a methyl orange end point, pH~4.3, further converts the bicarbonate to aqueous carbon dioxide. At this end point, some of the weaker conjugate bases are protonated. The methyl orange end point titration indicates total alkalinity.
The pH range for carbonate-bicarbonate buffer is 9,2.