What is an alkaline earth hydroxide?
455088
Alkaline earth elements are the elements of the 2nd group in the periodic table. The hydroxides formed by Calcium(Ca),Magnesium(Mg),Beryllium(Be),Strontium(Sr),Barium(Ba  \n\nSo the chemical formula for alkaline earth hydroxides can be:\nCa(OH)2-Calcium hydroxide\nMg(OH)2-Magnesium hydroxide\nBe(OH)2-Berellium hydroxide(unstable)
972591
Hydroxyl,any compound that has OH is an alcohol,like CH3OH, or CH3CH2OH,etc....)\n\nCarboxyl,is a group that has c=o (carbon double bondedwith oxygen)\n\nHalide: Any element from group 7 like chlorine or iodine
417834
Something that requires water in order to become a true Base\n\ne.g. CaO + H2O -> Ca(OH)2
186625
llinois groundwater scientists have found microbial communities thriving in the slag dumps of the Lake Calumet region of southeast Chicago where the water can reach extraordinary alkalinity of pH 12.8. That's comparable to caustic soda and floor strippers -- far beyond known naturally occurring alkaline environments.\n\nThe closest known relatives of some of the microbes are in South Africa, Greenland and the alkaline waters of Mono Lake, California.
602608
Confusion between base and alkali\nThe terms "base" and "alkali" are often used interchangeably, since most common bases are alkalis. It is common to speak of "measuring the alkalinity of soil" when what is actually meant is the measurement of the pH (base property). Similarly, bases which are not alkalis, such as ammonia, are sometimes erroneously referred to as alkaline.\n\nNote that not all or even most salts formed by alkali metals are alkaline; this designation applies only to those salts which are basic.\n\nWhile most electropositive metal oxides are basic, only the soluble alkali metal and alkali earth metal oxides can be correctly called alkalis.\n\nThis definition of an alkali as a basic salt of an alkali metal or alkali earth metal does appear to be the most common, based on dictionary definitions
386434
http://www.ebroadcast.com.au/lookup/encyclopedia/so/Soil_pH.html\n\nSoil pH\n\nSoil pH is an indication of the alkalinity or acidity of soil. It is based on the measurement of pH, which is based in turn on the concentration of hydrogen ions (H+) in a water or salt solution.\n\n\nWhen in balance (pH 7) the soil is said to be neutral. The pH scale covers a continuum ranging from 0 (very acidic) to 14 (very alkaline or basic). It is however uncommon to find soils at either extreme of this range. Under many conditions soils tend to become more acid or alkaline over time if steps are not taken to maintain a balance. \n\npH is important for the organic gardener for several reasons, including the fact that many plants and soil life forms prefer either acid or alkaline conditions, that some diseases tend to thrive when the soil is alkaline or acidic, and that the pH can affect the availability of nutrients in the soil. \n\nTable of contents [showhide]  \n1 Nutrient availability in relation to soil pH \n2 Soils and acidity \n3 Soil life and pH \n4 pH and plant diseases \n5 Determining pH \n6 Altering soil pH \n7 See also \n \n \n\n\n\nNutrient availability in relation to soil pH \nThe majority of food crops prefer a neutral or slightly acidic soil, because the solubility of most nutrients necessary for healthy plant growth is highest at at pH 6.3-6.8. Some plants however prefer more acidic (e.g., potatos, strawberries) or alkaline (brassicas) conditions. \n\nWhen the pH falls below 5.5, most major plant-nutrient minerals (those needed in substantial quantities to promote healthy plant growth include nitrogen (N), phosphorus (P), potassium (K), sulphur (S), magnesium (Mg), and calcium (Ca)) and some micronutrients[?] (elements important to plant growth in very small amounts) become insoluble and hence unavailable for uptake by plant roots. \n\nMany cationic (positively charged) nutrients such as zinc (Zn2+), aluminium (Al3+), iron (Fe2+), copper (Cu2+), cobalt (Co2+), and manganese (Mn2+) are soluble and available for uptake by plants below pH 5.0, although their availability can be excessive and thus toxic in more acidic conditions. In more alkaline conditions they are less available, and symptoms of nutrient defficiency may result, including thin plant stems, yellowing (chlorosis[?]) or mottling of leaves, and slow or stunted growth. \n\npH levels also affect the complex interactions among soil chemicals. Phosphorus (P) for example requires a pH between 6.0 and 7.0 and becomes chemically immobile outside this range, forming insoluble compounds with iron (Fe) and aluminium (Al) in acid soils and with calcium (Ca) in calcareous soils. \n\nThis table indicates the availability of several nutrients at various pH values: \n\n  Acid  Neutral Alkali  \n  4   4.5 5   5.5 6   6.5 7   7.5 8   8.5 9   9.5 10 \nnitrogen, N       \nphosphorus, P         \npotassium, K         \ncalcium, Ca       \nmagnesium, Mg       \nsulfur, S     \niron, Fe     \nmanganese, Mn       \nboron, B       \ncopper, Cu       \nzinc, Zn       \nmolybdenum, Mo     \n\n\n\nSoils and acidity \nUnder conditions in which rainfall exceeds evapotranspiration (leaching) during most of the year, the basic soil cations (Ca, Mg, K) are gradually depleted and replaced with cations helds in colloidal[?] soil reserves, leading to soil acidity. Clay soils often contain Fe and hydroxy Al, which affect the retention and availability of fertilizer cations and anions in acidic soils. \n\nSoil acidification may also occur by addition of hydrogen, due to decomposition of organic matter, acid-forming fertilisers, and exchange of basic cations for H+ by the roots. \n\nSoil acidity is reduced by volatilization and denitrification of nitrogen. Under flooded conditions, the soil pH value increases. In addition, nitrate fertilizers containing cations such as Ca, K, or Na also increase the soil pH value. \n\n\nSoil life and pH \nA pH level of around 6.3-6.8 is also the optimum range preferred by
167648
Alkaline: the oxides, when mixed with water, form alkaline solutions.\n\nEarth: Calcium and Magnesium are major constituents for most kinds of rock and soil.
856024
Alkali earths are the elements of group 2.\nAlkali metals are the elements of group 1.\n\nHere are the properties of group 2\nhttp://en.wikipedia.org/wiki/Alkaline_earth_metal\n\nHere are the properties of group 1\nhttp://en.wikipedia.org/wiki/Alkali_metal\n\nYou can compare them.\n\nHere is the water reaction with elements of group 1 (example K)\n\n2K (s) + 2H2O (l) → 2KOH (aq) + H2 (g)\n\nHere is the water reaction with elements of group 2 (example Mg)\n\nMg + 2H2O → Mg(OH)2 + H2\n\nAs you go to the extremes of the table and down the table the reactivity is higher because the electronegativiy is lower so they have a greater tendency to lose the electron and react.
53525
Sodium hydroxide is a very strong base, not an acid (the common name is lye).\nTriglycerides are fats, like beef tallow.  Mixing them and allowinging to react would produce Granny's lye soap.
772321
The alkali metals, found in group 1 of the periodic table (formerly known as group IA), are very reactive metals that do not occur freely in nature. These metals have only one electron in their outer shell. Therefore, they are ready to lose that one electron in ionic bonding with other elements. As with all metals, the alkali metals are malleable, ductile, and are good conductors of heat and electricity. The alkali metals are softer than most other metals. Cesium and francium are the most reactive elements in this group. Alkali metals can explode if they are exposed to water. \n\nThe alkaline earth elements are metallic elements found in the second group of the periodic table. All alkaline earth elements have an oxidation number of +2, making them very reactive. Because of their reactivity, the alkaline metals are not found free in nature.
617910
You missed to write 'metals'. This is customary.!!!\n\nAll answers are relevant.\n\nmurthy seems to be more relevant to the question.\n\nReview in the following way:\n\nOne thing common with 1A & 2A group is there nature to form alkalies with water; so they are alkaline in nature.\n\nThe second thing common is that they all are metals so they are alkaline metals.\n\nAn additional aspect only to 2A group is that the members of the group are normally more abundent in mineral form (in the earth crust) so to distingwish with the other alkaline metals they are referred as alkaline earth metals.
355623
The common definition of a base is a chemical compound that absorbs hydronium ions when dissolved in water (a proton acceptor). An alkali is a special example of a base, where in an aqueous environment, hydroxide ions are donated. Bases and acids are seen as opposites because the effect of an acid is to increase the hydronium ion (H3O+) concentration in water, whereas bases reduce this concentration. Arrhenius bases are water-soluble and these solutions always have a pH greater than 7.
19390
Zinc hydroxide - ZnOH2.
567214
name commonly used for a strongly alkaline solution. It originally meant a solution of potassium carbonate (potash) prepared by leaching wood ashes with water, but now the name also means a solution of sodium hydroxide or potassium hydroxide. Lye is also used to refer to the undissolved solute. Common household lye is usually sodium hydroxide. Lye should be used with caution as it is caustic and poisonous.
374165
PH\nFrom Wikipedia, the free encyclopedia\n \npH (potential hydrogen) is a measure of the activity of hydrogen ions (H+) in a solution and, therefore, its acidity or alkalinity. In aqueous systems, the hydrogen ion activity is dictated by the dissociation constant of water (Kw = 1.011 × 10−14 at 25 °C) and interactions with other ions in solution. Due to this dissociation constant a neutral solution (hydrogen ion activity equals hydroxide ion activity) has a pH of approximately 7. Aqueous solutions with pH values lower than 7 are considered acidic, while pH values higher than 7 are considered alkaline
1029104
acid has a ph value below 7\nand alkali has a value above 7\n\nAn acid (often represented by the generic formula HA) is traditionally considered any chemical compound that when dissolved in water, gives a solution with a pH of less than 7. That approximates the modern definition of Brønsted and Lowry, who defined an acid as a compound which donates a hydrogen ion (H+) to another compound (called a base). Common examples include acetic acid (in vinegar) and sulfuric acid (used in car batteries). Acids generally taste sour;\n\nIn chemistry, an alkali (from Arabic: al-qaly القالي) is a specific type of base, formed as a carbonate, hydroxide or other basic (pH greater than 7) ionic salt of an alkali metal or alkali earth metal element. The word alkali or the adjective alkaline are frequently used to refer to all bases, since most common bases are alkalis, although strictly speaking this is inaccurate.
283437
Sodium Hydroxide dissolves in water and dissassociated completely to form Sodium +1 and Hydroxide -1 ions in solution.\n\nNaOH --H2O--> Na+(aq) + OH-(aq)