Precipitated Calcium Carbonate

About Precipitated Calcium Carbonate

2 Precipitated Calcium Carbonate Loading

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4 Precipitated Calcium Carbonate Loading

5 Precipitated Calcium Carbonate Loading

6 Precipitated Calcium Carbonate Loading

Popular Questions

Precipitated calcium carbonate vs Powdered Calcium carbonate. Which has a larger surface area? (same mass)? Thank you

coolchap_einstein replied: "powdered one . \i think cuz powdered one is spread through our the soloution while precipitate settles down. \if both are at same position the both have same surface area. \other wise if the precipitate one is down and the powdered one is sperad through the soloution powdered one has more surface area,."

Trevor H replied: "The finest and highest quality calcium carbonates are the precipitated grades. The precipitation reaction: Ca(OH)2 + CO2 → CaCO3 + H2O is very carefully controlled from the point of view of crystal growth and reaction speed. This not only gives a fine particle size end product, but the particle size distribution graph is much more uniform than the ground grades. Precipitated grades are extensively used in the pharmaceutical industry fot this reason. I was associted with a very large paper mill that installed on on site carbonate precipitation plant for CaCO3 in preference to using the more readily available ground grades, precisely for the reason of finer and more controlled particle size. This gives a direct benefit in surface area of the carbonate, leading to better whiteness and opacity in the paper. In contrast the ground grades can be quoted as having a similar average aprticle size as the precipitated grades. but they invariably do not have the tight particle size distribution of the precipitated product. In the context of your question, the product with the better particle size will have the larger surface area, and this is the precipitated type."

Name two compunds that could be combined to cause the formation of a calcium carbonate precipitate.? identify any spectator ions in the system you described in part a. write the net ionic equation for the formation of calcium carbonate.

reb replied: "calcium hydroxide and carbonic acid"

steve_geo1 replied: "Calcium nitrate and sodium carbonate. Nitrate and sodium are spectator ions. Ca2+ + CO3= ===> CaCO3(s)"

What compounds could be mixed together to produce a precipitate of calcium carbonate? Also, How could you obtain a sample of potassium sulfate and barium chloride? If anyone could help me out with these questions that would be great.

bixentz replied: "CaCl + H2CO3 = HCl + CaCO3 2KCl + H2SO4 = 2HCl + K2SO4"

calcium carbonate is precipitated from an? aqueous sltn of 0.2M calcium nitrate when carbonate ion exceeds 2.5 x 10 ^ (-8).what's the KSP of calcium carbonate?..

Dr.A replied: "Ca(NO3)2 is a strong electrolyte : Ca(NO3)2 >> Ca2+ + 2 NO3- [Ca2+] = 0.2 M [CO32-] = 2.5 x 10^-8 M The equilibrium for the saturated solution is : CaCO3 <----> Ca2+ + CO32- and Ksp has the form : Ksp = [Ca2+] [ CO32-] Ksp = 0.2 x 2.5 x 10^-8 = 5 x 10^-9"

Tuncay U replied: "The calcium carbonate is a natural stone of calcite."

In arid climates, calcium and carbonate ions are dissolved from the upper soils horizons and precipitated at t In arid climates, calcium and carbonate ions are dissolved from the upper soils horizons and precipitated at the K-horizon forming (A). Laterites (B). Caliche (C). Paleosols (D). Humus

pisgahchemist replied: "Wow. I don't actually know this, and ordinarily, I would keep my mouth shut so no one would know that I actually didn't know this. There is always the chance that if I were to speak up, I'd confirm the fact that I don't know. But I do this to make a point. Often you are faced with having to answer a multiple choice question where you don't have clue. So I give my students some strategies to make use of what they DO know to eliminate some wrong choices. Let me share some of my thinking. Humus is a type of soil that is made up of lots of organic matter. I know that. If it has organic matter then it wouldn't contain a lot of Ca and carbonates. Eliminate humus. Paleosols. The prefix "paleo" is used to mean "old" as in paleolithic meaning "old rocks". The "sols" part might refer to aerosols which are particles that get airborne. Since calcium carbonate is limestone I doubt that it will get airborne. Laterites and caliche. Laterites may imply something that is lateral which can mean horizontal or along a line. Calcium carbonate may get deposited in a horizontal line. But caliche has too much in common with calcium. At least the first three letters anyway, so I'm going with caliche. This is the point were we google caliche and here is the first hit: Caliche (mineral), a hardened deposit of calcium carbonate. Am I good or what!!! My point is that when it's crunch time on a test, you can use what you do know to figure out stuff you don't know."

Sodium Carbonate + Calcium Chloride lab, possible sources of error? Help pleasee!? we did the basic lab many people do this one we mix 10 mL of sodium Carbonate with 20 mL of calcium chloride we filter out the precipitate calcium carbonate using a funnel and filter paper and then measure the mass of the filter paper with the precipitate what could be some non-human sources of error helpp would be GREATLY appreciated getting a bit desperate heree!

Sean replied: "i had a lab today where we used CaCO3 (calcium carbonate) also, but our teacher said it is a carcinogen and that we shouldsnt get near it. Funny stuff..."

When strontium choride and calcium carbonate react, it forms a precipitate..? the equation i have is Na2CO3 + SrCl2 yields 2NaCl + SrCO3 out of the products, which one is the precipatate? or the how do i find the limiting reactant? thank you so much, you are a huge help!! i've done the calculations with the info i have and the limiting reactant is Na2CO3. would the reaction have worked if the SrCl2 was the limiting reactant?

sarahharrelson replied: "SrCO3 is the precipitate because NaCl is considered aqueous(it dissolves in water). Only group I and ammonium carbonates are soluble The reactant that produces the least amount of one of the products is the limiting reactant"

SHAWNA W replied: "SrCO3 is the precipitate formed I can't tell you the limiting reactant until you tell me how many grams or moles of each reactant you have."

Isabel D replied: "First of all you wrote calcium carbonate in your problem, but your equation states sodium carbonate, so which is it. On the product side sodium chloride is not a precipitate because all metal halides are ionic and fall apart in aqueous solutions into ions, so strontium carbonate is the precipitate. The limiting reactant is found if you are given the starting weights of the components, then you convert that into moles using their molecular weights, and then you see which component you have less of - that's the limiting reactant. In this particular problem your ratio of reactants is 1:1."

Calcium Carbonate?? Please help!!? Name two compounds in solution that could be to cause calcium carbonate to precipitate. Describe how you would perform the reaction in the lab. Identify any spectator ions in the solution and write the net ionic equation for the reaction.

DrSean replied: "calcium chloride and sodium carbonate will precipitate calcium carbonate. Mix an aqueous 0.1 M solution of each compound, and drop one into the other. The spectator ions are Na+ and Cl- CaCl2 (aq) + Na2CO3 (aq) -> CaCO3(s) + 2 NaCl (aq)"

How do you prove that a chemical reaction occured between Calcium Chloride and Sodium Carbonate? I did an experiment dissolving sodium carbonate and calcium chloride into water, and then mixing them together. There was this milky mixture that seemed to have formed ontop of water. I'm not quite sure how to prove a chemical reaction occured because there is no precipitate, temperature or colour change and there was apparently no gas produced.

Whoby M replied: "there should be precipitate in the milky mixture since the 2 combine is an ionic precipitation or double decomposition to make solid calcium carbonate and soluble sodium chloride"

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