why Sulphuric acid do not react with limestone?
968530
A lot of silly answers here. It does reac slightly to make calcium sulphate. Calcium sulphate is only slightly soluble and coats the limestone making a barrier between the limestone and the acid.
256628
if we are talking just Vinegar (acetic acid) and sulfur there is a possibility it would react to form hydrogen sulfide (H2S). H2S is toxic so you need to do it in small amounts and a WELL VENTILATED AREA!!!
929088
Explain the reaction of Potassium Nitrate mixed with Amonia Sulfite,with a pinch of Magnesium powder,and a foot of Magnesium Ribbon,and last but not least Benzyl Chloride. It is very important you use Benzyl Chloride.
488315
Carbonic acid is the one that usually affects limestone bedrock.\n\nCarbonic acid forms when decaying matter interacts with filtering water.\n\nAs it moves down through cracks in the bedrock, it slowly dissolves the limestone. Over time the cracks grow & enlarge eventually making miles of underground caves & caverns.\n\nThe type of topography associated w/ dissolution of limestone bedrock is called Karst Topography.\n\nKarst simply refers to that which you can see above ground like sinkholes (collapsed caverns/caves) & Karst lakes (sinkholes filled w/ water).
578806
The full reactions are:\n\nSulfur dioxide reacts with water in the air to form sulfurous acid:\n\nSO2(g) + H2O(l)  H2SO3(aq)\n\nSulfur dioxide (SO2) can also be oxidized gradually to form sulfur trioxide:\n\n2SO2(g) + O2(g) -----> 2SO3(g)\n\nSulfur trioxide then reacts with water to form sulfuric acid:\n\nSO3(g) + H2O(l) -----> H2SO4(aq)
986564
I'm not 100% sure, but it seems like this procedure would neutralize any acids in the solution.  The Hydroxide would turn acid to water.  Any remaining hydroxide would combine with Calcium to form Calcium Hydroxide, which has a low solubility.  This would then precipitate out of the solution.  If the solution is mostly organic, it would also adsorb most of the water and remove it form the organic phase.
559378
Sulphuric acid is a strong oxidizing agent and does not complex ions easily. It thus is a wonderful reagent to activate ions for study.
1044878
Cement, known as Portland cement, which is used in concrete is not calcium carbonate and is in fact a silicate compound. There is no similarity between the reaction of cement and the hydration of calcium oxide that is described in another answer here and the reaction that takes place when cement is mixed with water. The statement "If you add water to the CaO... it will form again CaCO3 capturing the CO2 dissolved in the water" is absolutely incorrect and does not describe the reaction of cement with water. \n\nThe elements of dry cement that you are refering to are:\ntricalcium silicate (3CaO × SiO2)\ndicalcium silicate (2CaO × SiO2)\n tricalcium aluminate (3CaO × Al2O3)\ntetra-calcium aluminoferrite (4CaO × Al2O3Fe2O3)\n\nAs you can see the only thing they have in common with calcium carbonate (CaCO3) is the CaO. In fact calcium carbonate is a raw material used in manufacturing cement, but the resulting chemical compound is NOT calcium carbonate and has no similarity. The raw materials used in manufacturing cement are limestone, shale or clay, and gypsum. These are heated in kilns to about 1550 degrees F. \n\nThe main chemical reaction that chemically combines cement and water (the water is incorporated into the molecular structure- it does not 'dry' out) is as follows:\n2 Ca3SiO5 + 7 H2O ---> 3 CaO.2SiO2.4H2O + 3 Ca(OH)2 + 173.6kJ  \n\n\nTo answer your question, yes cement is known to occur in nature. Geologists discovered a natural deposit in the 1960's that is about 12 million years old, that formed where an oil shale reacted with a limestone. The Greeks were probably the first to discover cement similar to what we know today. Here is a timeline:\nhttp://matse1.mse.uiuc.edu/concrete/hist.html
690069
Good question.\n\nLimestone is found in the earth.  Refined Limestone and limestone in it's pure form is known as Calcium Carbonate.  (CaCO3).\nIf you mix limestone with water, you'll get some mixing, but not all the limestone will go into solution.  What did go into solution can be "painted" onto a wall but it won't stay past the next few rains.  \nIn order to use limestone for paint, it has to be refined.  In other words, it has to go through a chemical reaction such as Carbonation, in order to get the product that you desire.  \nPlease see my sources for more information.
814242
Barium Hydroxide is a weak alkali which is not very soluble. If you try to neutralise it with dilute sulphuric acid you will get a precipitate of Barium sulphate. This means you won't be able to neutralise solid barium hydroxide just the solution. To neutralise either the solution or the solid use dilute hydrochloric acid.\nBa(OH)2  +  2HCl  =  BaCl2 +  2H2O\n\nIf you add carbonate ions CO3 2- to a solution of barium hydroxide Barium carbonate will be precipitated. Again carbonate ions (as in sodium carbonate solution) will not completely react with solid barium hydroxide.
903862
Sorry Voyager. Copper is not so reactive a metal that it will react with sulphuric acid.\nYou need either solid copper (II) carbonate or solid copper (II) oxide for the salt.\nSince it is a sulphate, sulphuric acid is used together with the solid.\nHeat the acid so that the reaction can proceed at a faster rate. Add solid till no more will react (no bubbles of gas produced, and the solid remains insoluble). This is to ensure that all the acid is used up. Filter to remove unreacted solid and heat the filtrate, which is the copper (II) sulphate solution, till saturated (approximately 1/3 to half the original volume left would be a good gauge). Let the hot saturated copper (II) sulphate solution cool and after some days, when the excess water evaporates off, you should get hydrated copper (II) sulphate crystals.\nDo not heat till dryness as this will evaporate off the water of crystallization needed for the blue copper (II) sulphate crystals to form. Without the water of crystallization, you would get anhydrous copper (II) sulphate powder (white) and not the blue crystals.\n\nHope this helps :)
449522
http://en.wikipedia.org/wiki/Sulphuric_acid
910098
Here is my best stab at this:\n\na)  Because limestone bleeds when in contact with water and is not a good exterior material choice, besides it is more brittle than ordinary bricks\n\nb)  Because adobe is also affected by water and compression is a big factor when using it over a story of height\n\nc)  Timber is not usable, not that it would not work and it compresses little, however it is not used for fire rating.  \n\nAll three have to do with life safety or erosion issues.  \n\nLook at the IBC (Internation Building Code) for further information on restrictions for each material.
604475
Carbon itself doesn't do anything at room temperature up to boiling point with sulfuric acid. Might just swim on it and adsorb a little of it (this being a process which gives out a little heat).\n\nIn case your carbon contains impurities, these might react with sulfuric acid and give out some smell and also colour and sediments, depending what the impurities are.\n\n(But the creation of CS2 as mentioned in GforGenius' answer in my opinion is just a joke against people who want to escape from doing their homework from their books and go the easy way on yahoo. If stinks something, the odour mostly comes from H2S (=rotten egg), because impure carbon depending on its origin might contain metallsulfides).
915724
the form just about everywhere in the world.  slightly acidic water (which most rain water is...it picks up CO2 on the way down....and makes a mild carbonic acid) dissolves limestone over long amounts of time.   it also happens with dolomite, marble, and gypsum....and it can happen with sandstone, as well - in the case of sandstone, carbonates act as a binder.
915462
This depends on why sulfuric acid is "king".  In industry, sulfuric acid is the most used chemical by weight (other than water).  The opposite, "the serf" or "fool" would be a chemical rarely used.  The choices are too numerous to list.
460512
In addition to the previous answer, the acidity of the water plays a significant factor.  Water alone is a great erosive tool, but rock is fairly resilient and it would take a long time to create the cave systems.  However, Calcium Carbonate (limestone) reacts with acids and disolves when in contact with them.  An eyedropper full of a diluted hydrochloric acid will create a small hole in a sample of limestone.  So the question now becomes where does the acid come from?  Well, pollution definately plays a factor, however natural acids in the soil are leeched down into the limestone as water works its way into the limestone.  This is also why sinkholes occur... imagine a cave system with a roof or ceiling allready in place, and years of acidic water leaching into the cave through the cieling.  Eventually it will disintigrate, collapsing in on itself.  You can check out www.geology.com and search Karst Topography for more information.