alkalinity is higher when magnesium is present. Is this because mg itself counts towards alkalinity or because mg inhibits the precipitation of calcium carbonates which count towards alkalinity?
201939
Alkalinity is usually measured by the presence of bicarbonate (HCO3-) and carbonates (CO3=) and acts to buffer water from acidic inputs, thus is a measure of the buffering capacity of water. Water with high alkalinity have high pH values while water with low alkalinity have low pH values. The hardness of the water is usually determined by the amount of calcium and magnesium salts present in water and is associated with the presence of carbonates. Hard water is generally more productive than soft water waters and can accept more input of salts, nutrients, and acids to their system without change than can soft water waters. So basically, it’s because of the presence of the magnesium. \n\nHope this helps and hope I didn’t confuse you.
88645
Actually, Calcium in it's pure form doesn't exist in nature, as it is highly reactive with water.  It is only found in compounds such as chalk (CaCO3), lime (Ca(OH)2) or gypsum (CaSO4), which can erode to very fine particles which then become SUSPENDED in water.
191934
manesiun and fluorine....magnesium forms a positively charged ion, while fluorine forms a negatively charged ion, different charges attract, so they form ionic bond to each other forming a ionic compound.\n\nnitrogen and sulphur both form negative charged ions, so there is noway to make them react unless in a prescence of a catalyst.\n\nionic compounds generally fom using, metals and nonmetals. magnesium is a metal, and fluorine nitrogen and sulphur are all non metals
88442
Apart from the precipitation reactions (AgCl and BaCO3 form insoluble compounds, although HCl will dissolve BaCO3), there is flame colouring for identifying the alkali and earth alkali metals (Na yellowish orange, Li reddish, Ba green), there are pH measurements (HCl acidic, NaOH and Na2CO3 basic, rest neutral), and you need to test an oxidant to identify the sugar solution. This ought to give you a matrix which gives only one possible identification for each test (with deionized water failing all tests).
255319
DO NOT add sodium bicarbonate! The pH is already too high. Bicarb will only COMPOUND the problem, not fix it. What you need is acid. Bicarb has an alkaline pH.
353348
When you boiled the water, you evaporated some of it. This increases the salt concentration in the water which alters the ph. Since it went toward the alkaline side, it probably increased the calcium salts in the water.
49042
carbonate + acid = salt + carbon dioxide + water, so:\n\nsodium carbonate + sulphuric acid = sodium sulphate + carbon dioxide + water.
64288
1. \nMoles of Ca(HCO3)2 produced = 3.05 x 10^10/Molecular Mass of Ca(HCO3)2\n=3.05 x 10^10/162\n=0.018 x 10^10\n\nFrom the equation we know on dissolving 1 mole of limestone we get 1 mole of Ca(HCO3)2 \nThus, if 0.018 x 10^10 moles of Ca(HCO3)2 are produced moles of limestone dissovled should be 0.018 x 10^10\nWeight of limestone dissolved = Moles x its Molecular Mass of limestone\n=(0.018 x 10^10) x(100)\n=1.8 x 10^10 gm.\n\n2.\na.) CO + 2H2 --> CH3OH\n\nb.)Moles of methanol to be produced = 45/Molecular Mass of CH3OH\n=45/32\n=1.40625\n\nFrom the equation we know 2 moles of H2 are required to produced 1 mole of methanol\nThus to produce 1.40625 moles of H2 required = 2*1.40625\nWeight of H2 required = Moles X Molecular mass of H2\n=(2 x 1.40625) x 2\n=5.625 gm
30178
Magnesium acts as a sacrificial anode.\n\nOxygen in the atmosphere reacts with iron to oxidize it in what is called a redox reaction (oxidation/reduction). The redox reaction is defined by the exchange of electrons--uncharged iron will lose two electrons to an oxygen molecule, creating iron oxide. Water quicken rusting by serving as a catalyst. Dissolved oxygen in the water reacts, and as the water dries, the oxygen becomes increasingly concentrated.\n\nEngineers will prevent wide-spread rusting by creating what is called a "sacrificial anode." You might know the names anode and cathode from the ends of a battery. Batteries function by employing two seperate redox reactions, where one end corrodes to release electrons, which travel to the other end and react with metal cations in solution, turning them to a solid metal. The corrosion of iron is prevented by creating a sacrificial anode out of something even more reactive than the iron (usually magnesium). The corrosion of the magnesium releases excess electrons in the iron, which delays corrosion of the iron--oxygen can grab the free electrons created by the corrosion of magnesium without needing to corrode the iron.
55898
All active metals whose activity is more than H react with water under some or the other condition. For eg. Na metal reacts violently with cold water(the colder the better) liberating hydrogen gas which ignites due to the heat produced in the reaction whereas Mg shows a similar reaction with hot water. The energy liberated is due to the Hydration enrgy which gives the respective metal hydroxides. Even dissolution is a slightly exothermic.
427667
1. is the reaction of acid on sugar. It leaves a pillar of carbon and gives off steam. The acid is still there and should be neutralized.\n\nI do not know what lye does to sugar\n\nMg and sodium hydroxide do not react. Na is stronger than Mg\n\nNa2CO3+NaOH both have a sodium ion and havae no reason to react.
333189
Alkaline batteries contain basically Manganese Oxide and Dioxide coupled with Zinc oxide.  Manganese and zinc are known as transitional metals not alkali metals or alkaline earth metals.  The reason why alkalines batteries are called alkaline batteries is due to the potassium hydroxide electrolyte.  \nMixing an alkali or alkaline earth metal with a halogen will produce a salt known as a ionic salt.
397465
When NaOH is added Sodium carbonate remains unaffected but \nbicarbonate is affected as it releases a proton from bicarbonate ion.\nNaHCO3 + NaOH ~~~~~~ Na2 CO3  + Water\n\nWhen Barium Chloride is added to Sod.Carbonate BariumCarbonate and Sodium Chloride is formed.\nBaCl2 + Na2CO3 ~~~~~ BaCO3 + 2NaCl\n\nWith bicarbonate no rxn occurs.
514142
Given   X  amount of magnesium, it will form MgO to the extent of the amount of magnesium. The magnesium is the limiting factor. \n\nOxygen is much more reactive than nitrogen. The magnesium would rather react with the oxygen because it takes less energy, despite the very hot and bright light given off when Mg burns.\n\nAbout the only way that nitrogen ever combines with anything from the air is when it is compressed in a cylinder of an internl combustion engine and  forced to combine under pressure and heat and  nitrogen oxides are released to form smog.
509333
(1) NaHCO3    --->  Na(+) + HCO3-\n(2) Ca(NO3)2  ---> Ca2(+) + 2NO3-\n(3) Al2(CO3)3  ---> 2Al(3+) + 3CO3(2-)\n\nThis is all taking place in water (ideally), so you should consider that too.
205398
pH (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..\n\npH = -log(concentration of H+)\njust use the equation to figure it out.\nhttp://en.wikipedia.org/wiki/PH
472077
1. Molarity = concentration and it expressed as mol per dm^3\n    Change the mass to mole and the 851 ml to dm^3. Then find   \n    the ratio of the number of moles to volume in dm^3\n\n2. Soluble ionic compounds breaks up the water molecules in H^+ ions and OH^- ions. Sodium carbonate give Na^+ ions and CO3^2- ions......Other ions that are present are HCO3^- ions called hydrogen carbonate ions. I have found that a solution of sodium carbonate is alkaline: implying that there are more OH^- ions to H^+ ions, due to the formation of HCO^- ions.\n3. OH^- (aq) + H^+(aq) ----> H2O (l)\n4. H^+ ions (ie. hydrogen ions), OH^- ions (ie. hydroxyl ions),\n   Ca^2+ calcium ions and Cl^- chloride ions\n5. Hydrogen ions, hydroxyl ions. ammonium ions and sulphate ions.\n6. Actually the calcium metal reacts with water to give hydrogen gas and calcium hydroxide. At the same time, calcium reacts with nitric acid to give calcium nitrate, water and brown nitrogen dioxide gas.\nHence there is no simple ionic equation for your question\nYou may want to consider this one:\nCa^0  +  2H^+   + 2OH^-  -----> H2(g)  + Ca^2+  + 2OH^-\n7. Hydrogen ions, hydroxyl ions, iron (III) ions Fe^3+  and sulphate ion SO4^2-