also more commonly called total alkalinity – A measure of the pH-buffering capacity of water. Also defined as the water's resistance to change in pH. Composed of the hydroxides, carbonates and bicarbonates in the water expressed in ppm or mg/L. One of the basic water tests necessary to determine water balance. The ideal range is from 60 to 140 ppm.
The quantitative capacity of a water or water solution to neutralize an acid. It is usually measured by titration with a standard acid solution of sulfuric acid, and expressed in terms of its calcium carbonate equivalent.
The capacity of a water to neutralize acids; a measure of the buffer capacity of a water. The major portion of alkalinity in natural waters is caused by (1) hydroxide, (2) carbonates, and (3) bicarbonates.
The relative acidity of any solution expressed in a pH range of numbers. The pH value is the negative common logarithm of the hydrogen-ion concentration in a solution, expressed in moles per liter of solution. A neutral solution, that is, one that is neither acidic nor alkaline, such as pure water, has a concentration of 10 moles per liter; its pH is thus 7. Acidic solutions have pH values ranging with decreasing acidity from 0 to nearly 7; alkaline or basic solutions have a pH ranging with increasing alkalinity from just beyond 7 to 14. In seawater, the alkalinity is a measure of the excess of hydroxyl ions over hydrogen ions, generally expressed as milliequivalents per liter.
The amount of excess base in a solution, measured in millimoles/kilogram--basically in these muds, a measure of dissolved carbonate.
An abnormal condition resulting from a decrease in acids or from an increase of alkali in the blood and body tissues.
The opposite of acidity, alkalinity is the prevalence of ions which neutralize H+ ions. A "base" is highly alkaline, or "basic." Usually alkalinity is due to OH- ions which can neutralize H+ ions, although other bases can be responsible for alkalinity.
The concentration of alkali, an acid-neutralizing chemical substance, in a solution measured in terms of pH.
the total amount of bicarbonate and carbonate ions present in water, reported in mg/L of calcium carbonate (CaCO). Water alkalinity helps protect against abrupt pH changes, limiting its range to between 7.5 and 8.5. Alkalinity and hardness also control pipe scale formation. There is no drinking water standard for alkalinity.
The amount of bicarbonate, carbonate or hydroxide compounds presents in water solutions.
helps to buffer pH levels in water by neutralizing acids. Also provides a carbon (food) source for aquatic microorganisms.
(also referred to as total alkalinity): a measure of the pH buffering capacity of water. Alkalinity is generally expressed in terms of the equivalent concentration of calcium carbonate in ppm or mg/l. In pool or spa water, alkalinity should be 80â€“140 ppm. (N)
An alkaline water contains carbonates or hydroxides, highly alkaline waters are called "hard" and can precipitate deposits on your teapots and cooking vessels. Water softeners are used to remove this alkalinity from hard waters. Acidic mine waters tend to have very little alkalinity and this prevents the precipitation reactions that allow metals removal. It is typically necessary to add alkalinity to such waters to allow treatment.
a measure of the ability of a solution to neutralize acid without a change in pH.
Alkalinity is the characteristic of soils with a pH level that is greater than 7, that is suitable for plants that thrive in a isweet (alkaline) soil, as opposed to a sour or acid soil.
a measure of how stable the pH is. A low total alkalinity level will cause the pH to fluctuate drastically whenever small amounts of acid or base are added to the pool water. A high total alkalinity level will make the water more susceptible to scale and high pH.
The quantitative capacity of aqueous solutions to react with acids.
The extent to which the pH value of a solution exceeds 7. Cf. Acidity. ( BCFT )
Alkalinity is measured in mg/l as calcium carbonate (CaCO3). It represents a measure of a solution's ability to buffer or neutralize acids. Lakes located in areas of calcareous glacial till (common throughout central and southern Minnesota) will have higher alkalinity than lakes formed on non-calcareous bedrock (common in northeastern Minnesota). Water with alkalinity less than about 75 mg/L could be considered soft, 76-150 moderately hard, 151-300 hard, and greater than 300 very hard. Alkalinity has also been used as a basis for estimating sensitivity to acid precipitation. For this purpose, lakes with alkalinity values less than 5 to 10 mg/L could be considered potentially sensitive to acid precipitation based on current levels of deposition across Minnesota. At this point we have identified no "culturally acidified" lakes in Minnesota.
Capacity of a lake to neutralize acid.
A property of sea water operationally defined as the excess positive charge to be balanced by CO3 and HCO3 ions. The carbonate ion content of any unit of sea water is equal to its alkalinity (i.e. excess positive charge) minus its total dissolved carbon content. See Broecker and Peng (1982).
Emäksisyys, alkaliteetti Alkalitet, alkalinitet A water's buffering capacity or its' ability to neutralize acids.
The ability of water to maintain a stable pH. Controlled by the amount of carbonate ions present in the water. Also called Buffering Capacity. See KH.
The amount of bicarbonate, carbonate, and hydroxide compounds present in the water. Total Alkalinity is a measure of the water's ability to resist pH change due to the presence of these compounds in the water.
The acid-neutralizing capacity of water. It is primarily a function of the carbonate, bicarbonate, and hydroxide content in water. The lower the alkalinity, the less capacity the water has to absorb acids without becoming more acidic.
The quality of a material to be basic or alkaline when exposed to moisture or water producing a blue reaction to litmus paper. A pH over 7. Insulation that creates an basic (alkaline) acidic environment when exposed to water can contribute to corrosion of the system. Dyplast's polyisocyanurate and expanded polystyrene products do not react with water, creating neither a basic nor acidic environment; therefore they do not contribute to corrosion. ASTM C871 provides the methodolgy for the determination of water-leachable chloride, fluoride, silicate, and sodium ions in thermal insulation materials.
is a measure of the proton-accepting capacity of a solution. This property is also referred to as its "acid-neutralizing capacity", and is equal to the sum concentration of all proton acceptors in the solution or the total strong base concentration. Total alkalinity is operationally defined as the alkalinity neutralized by titration with a strong acid to the carbonic acid equivalence point. (IT = incremental titration, DIS = dissolved, TOT = total)
Alkalinity means the buffering capacity of water; the capacity of the water to neutralize itself. It prevents the water pH levels from becoming too basic or acid. It also adds carbon to water. Alkalinity stabilizes water at pH levels around 7. However, when the acidity is high in water the alkalinity decreases, which can cause harmful conditions for aquatic life.
having the nature of a class of substrates that liberate hydroxide ions in water, pH 7.
The presence of excess hydroxide ions compared to hydrogen ions (protons). The opposite of acidity; high on the pH scale.
The acid combining capacity of a (carbonate) solution, also describes its buffering capacity.
The quantitative capacity of aqueous media to react with hydroxyl ions. The equivalent sum of the bases that are titratable with strong acid. Alkalinity is a capacity of an aqueous system.
The measurement of constituents in a water supply which determine alkaline (opposite of acidic) conditions.
Alkalinity is the amount of carbonates, bicarbonates and hydroxides in water.
The amounts of certain minerals in the water. A too high total alkalinity causes PH to resists adjustment to the desired range. A too low total alkalinity makes it difficult to maintain PH within the desired range. Each condition has its set of problems.
This is the measure of a solution's resistance to changes in pH. It is commonly measured as carbonate alkalinity or total alkalinity, and is expressed in meq, dKH, or ppm of C03 ions. The alkalinity can be raised by adding a buffer.
A condition in which the urine becomes more alkaline, and consequently less acid, than normal.
A general term applying to substances on the base side of neutral-principally the degree of alkalinity (7 - 14 on the Ph scale, 7 being neutral).
the measurement of constituents in a water supply which determine alkaline conditions. The alkalinity of water is a measure of its capacity to neutralize acids. See pH.
The capacity of water to neutralize acids, a property imparted by the water's content of carbonates, bicarbonates, hydroxides, and occasionally borates, silicates, and phosphates. Alkaline fluids have a pH value over 7
The capacity of bases to neutralize acids. An example is lime added to lakes to decrease acidity.
The alkalinity of water is its acid-neutralising capacity, otherwise known as buffering capacity. It is the sum of the titratable bases in a sample.
ppm None 110 40-143
Sometimes referred to as Carbonate Hardness. The amount of your aquarium water's ability to resist changes in pH. The alkalinity can be raised by using a catalyst such as baking soda. Alkalinity is usually expressed in PPM (parts per million)
Also known as Total Alkalinity, is a measure of the pH buffering ability of water or resistance to change in pH. Tested to determine water balance.
Is a measure of the ph-buffering capacity of water. It tells us the water's resistance to change of ph. This is one of the basic water tests necessary to determine if the water is in balance.
The concentration of this parameter is an indication of the natural hardness and pH of the water. No standard
The measurement of the ability of water's capacity to neutralize acids.
A measure of a material's ability to neutralize acids. Alkalinities are usually determined using titration.
A measure of the capacity of water to neutralize a strong acid. In natural waters this capacity is attributable to basic ions such as bicarbonate, carbonate and hydroxyl ions as well as other ions often present in small concentrations such as silicates and borates. See also pH. [Fr. alcali, calcined ashes.
Capacity for neutralizing acid, usually due to presence of bicarbonate or carbonate ions. Hydroxide, borate, silicate, and phosphate ions may contribute to alkalinity in treated waters.
An expression of the total basic anions (hydroxyl groups) that is present in a solution. It also represents, particularly in water analysis, the bicarbonate, carbonate, hydroxyl and occasionally the borate, silicate, and phosphate salts which will react with water to produce acid neutralizable anions.
Measure of the water's ability to neutralize acid and maintain the pH level within the recommended range.
The capacity of water to neutralize acids by its content of bicarbonates, carbonates or hydroxides (alkaline substances).
The measurable ability of solutions or aqueous suspensions to neutralize an acid.
Alkalinity represents the sum total of the bases in the water, and thus is the acid-neutralizing capacity of the water. It is due largely to the presence of calcium, magnesium and sodium carbonates and bicarbonates. Most natural drinking water has an alkalinity in the range of 10-500 mg/l. Alkalinity testing is used in combination with other tests for sizing the proper equipment.
the total measurable bases (OH, HCO3, CO3) in a volume of water; a measure of a material's capacity to neutralize acids.
The capacity of water to neutralize acids. This capacity is caused by the water's content of carbonate, bicarbonate, hydroxide, and occasionally borate, silicate, and phosphate. Alkalinity is express in milligrams per liter of equivalent calcium carbonate. Alkalinity is not the same as pH because water does not have to be strongly basic (high pH) to have a high alkalinity. Alkalinity is a measure of how much acid must be added to a liquid to lower the pH to 4.5 SU.
a measure of the capacity of water to neutralize acid. Alkali substances in water include hydroxides or bases.
The characteristic of water that registers a pH above neutral (7).
property of water containing alkaline substances; expressed as parts per million (ppm).
Alkalinity is useful in removing acidic, fatty and oily soils. Soap and soap-based products are alkaline and perform well only in an alkaline medium. Detergent products can be formulated at any level of alkalinity determined by the cleaning task to be performed.
a measure of the charged carbon species in water;
Alkaline refers to the condition where the water's pH is above 7.0 (neutral) on the pH scale. It is the opposite of acidic. Alkalinity is the amount of carbonates and bicarbonates in the water, measured in ppm of Total Alkalinity.
Alkalinity is a measure of the capacity of water to neutralize acids. This is known as the buffering capacity of water that is the ability of water to resist a change in pH when acid is added. Alkalinity in water is due primarily to the presence of bicarbonate, carbonate, and hydroxide ions.
concentration of alkali metals that form salts (e.g. Li, Na, K). High alkalinity raises pH and precipitates metals out of solution and is often associated with limestone substrates.
The capacity of water to neutralize acids; a property imparted by carbonates, bicarbonates, hydroxides, and occasionally borates, silicates, and phosphates. It is expressed in milligrams of equivalent calcium carbonate per liter (mg/L CaCO3).
A property of water soluble substances (or mixtures) causing the concentration of hydroxyl ions (OH-) in water solutions to be higher than the concentration of hydrogen ions (H+).
(basic) a measure of the ability of a solution to absorb positively charged hydrogen ions without a significant change in pH. Also referred to as buffering capacity. Alkaline solutions have a pH greater than 7.0.
The capacity of water to neutralize acids, a property imparted by the water's content of carbonates, bicarbonates, hydroxides and occasionally borates, silicates and phosphates. It is expressed in milligrams per liter of equivalent calcium carbonate.
The alkali concentration or alkaline quality of an alkali-containing substance.
The concentration of basic or alkaline components in a mixture determined by titration with an acid.
the capacity of water for neutralizing an acid solution.
Represents the amount of carbonates, bicarbonates, hydroxides and silicates or phosphates in the water and is reported as grains per gallon, or ppm, as calcium carbonate.
The capacity to buffer against pH drops. The greater the alkalinity, the more stable the pH will be and the less likely that there will pH swings. Alkalinity can be raised by adding a carbonate buffer material. Alkalinity can also be maintained through the use of substance called kalkwasser.
The condition of pH between 7-14. The chief cause of alkalinity in brewing water is the bicarbonate ion (HCO3-1).
The ability of water, or other substances, to absorb high concentrations of hydrogen ions. Substances with a pH greater than 7.0 are considered alkaline. A measure of the amount of carbonates, bicarbonates, and hydroxide present in water. Low alkalinity is the main indicator of susceptibility to acid rain. Increasing alkalinity is often related to increased algae productivity. Expressed as milligrams per liter (mg/1) of calcium carbonate (CaCO3), or as microequivalents per liter (ueq/1). 20 ueq/1 = 1 mg/l of CaCO3.
A measure water hardness, expressed as ppm of calcium carbonate.
Also called Total Alkalinity. A measure of the pH-buffering capacity of water or the water's resistance to change in pH. It is composed of the hydroxides, carbonates and bicarbonates in the water. When we measure the total alkalinity, we usually only measure the carbonate alkalinity level.
A measure of the amount of compounds in water that are able to neutralize acid deposition.
The degree or intensity of alkalinity of a solution, expressed by a pH value greater than 7.0.
The amount of carbonates, bicarbonates, hydroxides, and silicates or phosphates in the water; reported as grains per gallon, or parts per million as calcium carbonate.
a measure of the amount of anions of weak acid in water and of the cations balanced against them.
1. The quantitative capacity of water to neutralize an acid; that is, the measure of how much acid can be added to a liquid without causing a significant change in pH.
Alkalinity represents the amount of bicarbonates, carbonates and hydroxides in water. It is a measure of the buffering capacity (its degree of resistance to change in pH) of water.
Alkalinity or AT is a measure of the ability of a solution to neutralize acids to the equivalence points of carbonate or bicarbonate. Alkalinity is closely related to the acid neutralizing capacity (ANC) of a solution and ANC is often incorrectly used to refer to alkalinity. However, the acid neutralizing capacity refers to the combination of the solution and solids present (e.g., suspended matter, or aquifer solids), and the contribution of solids can dominate the ANC (see carbonate minerals below).