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User Submitted 21 September 1. User Submitted 18 September 1. User Submitted 15 September 1. User Submitted 12 September 1. If I used ml of hydrochloric acid how much CO2 would that produce? The concentration of the acid determines how many protons hydrogen ions it can donate to react with the marble. You need 2 hydrogen ions per carbonate group.

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The stronger the acid, the more protons and the more CO 2 you can make:. Sorry forgot to mention that. What stone material would you recommend for a CO2 generator, Limestone, Calcite Marble or Dolomite Marble?

I want to create water soluble calcium for agriculture. Since its so expensive I wanted to try using cheap limestone and acid to create my own. Does the hydrogen carbonate precipitate to the bottom, while pure calcium stays dissolved in the water? Is there a way to separate them so I'm just left with calcium? How long does it take for the reaction between sulphuric acid in acid rain and calcium carbonate to proceed?

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There are a lot of factors. Sulphuric acid reacting with calcium carbonate will actually produce calcium sulphate, which is insoluble; this will coat the carbonate surface, reducing access to the carbonate by fresh hydrogen ions.

So the reaction will initially appear to go fast, then very slowly once the sulphate layer builds up Limestone in rock form is not available sor some reason in my country now a days. We fill tank with water and hcl and limestone rock in tanks to neutralize hcl We have calcium carbonate in powder form can we neuterlize hcl with it? Kindly please help me with a solution to neutralize hcl. We make calcium stearate. Why not just pop your teacher's name and email address in the box and we'll send the homework answer directly to them on your behalf, to save you the bother since we're already being asked to do the homework itself for you What type of chemical reaction is it?

I was thinking it was a neutralization reaction, although salt is not produced.

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It is a neutralisation reaction, and there is a resulting salt: calcium bicarbonate - Ca HCO 3 2 aq. I have a hundred pounds of common opal covered in what appears to be limestone.

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Is there a way to dissolve it? I'm stuck on this question and I need to prove how you can tell that the gas limestone is giving off when added to acid is carbon dioxide can someone tell me how you prove it please? The classic test for carbon dioxide is that, when bubbled through limewater, the solution turns milky. This is because the limewater - which is calcium hydroxide - Ca OH 2 - reacts with carbon dioxide to form calcium carbonate - CaCO 3 which is insoluble; this precipates as fine particles, which impart a milkiness to the solution.

VR Submitted Video Section - Thousands of private porn videos submitted by users exclusively for Voyeur Russian Community Limestone is mostly made up of the mineral calcium carbonate (CaCO3). This is not very soluble, so rocks don't dissolve very quickly. But if you add an acid, you add hydrogen ions (H+), which will react with the carbonate to form hydrogen carbonate HCO3- ions, which are very soluble in water, and the limestone will dissolve. Or, if there is more acid, two hydrogen ions will Get an ad-free experience with special benefits, and directly support

Limestone - calcium carbonate, CaCO3 - dissolves and at a low rate. Sodium carbonate Na2CO3 dissolves faster than limestone; it reacts with acids in a chemical reaction, producing carbon dioxide.

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Limestone is calcium carbonate CaCO 3. Carbonates react with acids according to the equation:. However, the rate of the reaction will be determined by a number of factors.

First, the strength of the acid.

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Temperature is also important, because the rates of all chemical reactions are proportional to temperature. Another factor to consider is the salt produced when the acid and the carbonate react.

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Sulphuric acid is a very strong acid but it won't react very well with calcium carbonate because one product of the reaction is calcium sulphate. This is plaster of paris and is insoluble.

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As a result, it forms a protective layer around the limestone, preventing further access by the acid and effectively stopping the reaction. Morning, Peg. Happy Birthday Jamie!

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