Ammonium carbonate if put in solution will it yeild acidic or basic solution?
350928
AMMONIUM ion is NH4+, people!  Check your books occasionally ey lads?\n\n(NH4)2 CO3 -->  2 NH4+   +    CO3 2-\n\nNH4+ is more than 10,000 times weaker an acid than acetic acid; CO3 2-  will form HCO3-  so i'd say the solution will be basic ( but only weakly! )
634552
an ion with both acidic and basic part
8783
It depends on what you are adding the NaOH to.  If you add NaOH to pure H2O the ideal solution mixture will become more alkaline...i.e. higher pH.  If you add NaOH to a stronger organic base such as an Azide (N3-) the solution will be come more acidic...i.e. lower pH.
756170
It's a salt - ammonium acetate. Ammonium is an acid, but the acetate ion is actually alkaline.
1092099
to determine whether an acid or a base is soluble in say the universal polar solvent water, u should be knowing whether the substance is strong or weak\nnow bases like NaOH, CsOH, RbOH, Mg(OH)2 are strong bases and in solution they give us the cations and anions(mostly the hydroxyl grp)\nbases like Be(OH)2, Fe(OH)2 or 3, Cu(OH)2 or any of their oxides are weak and hence in solution they do not undergo complete dissociation and most of these are insoluble\nso in case ur not in a lab, the only way is to identify their degree of weakness
1180992
depends on the strength of the base actually.  water is amphoteric which means it can act like an acid or a base.  if a weak base is put in water the water can neutralize it, but water is quickly overrun yielding the below equation.\n\nB + H2O yields HO- +BH\n\nthis makes the water basic.
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.
441451
Well, there's a decomposition reaction.\n\nH2CO3 <--> H2O + CO2\n\nCarbonic acid (H2CO3) doesn't not exist much at all, because it decomposes into H2O and CO2. But some of the carbonic acid remains, pushing up the hydronium concentration, which by definition makes water more acidic. Therefore, getting rid of the CO2 in water makes water less acidic (raising the pH).
211023
wow, well put mrjeffy! I have one thing to add though. Because all acids and bases are electrolytes, you can use pH to determine what is and isn't an electrolyte in a solution. If it come out as acidic or basic, it is and electrolyte(the darker, the more basic or acidic). If it comes out neutral, like Distilled Water, it is not. Also don't forget that non-electrolytes will not completely dissolve into solution in water.
14648
Most acids form ions in solutions by _protolysis_ (transferring a hydrogen ion to the solvent), and most bases form ions in solution by disassociation (if they contain OH-ions) or by accepting a hydrogen ion from the solvent.\n\nExample: Na3PO4 + H2O --> 3 Na+ +HPO4(2-) + OH-
621304
If you are dealing with a reaction involving ammonium carbonate in solution, and are then measuring the temperature rise, you need the heat capacity of water, not ammonium carbonate!\n\nPlease post the whole problem if that is not enough to get you started.
997096
Without consulting any reaction energy tables, my money's on HNO3.  Nitric acid is one of about a half dozen really strong acids and will give off a tremendous amount of heat when dissolved in water.  I don't think any of these will actually react with water, but nitric acid will certainly dissolve the most violently.  If you have access to reference tables, you'll want to look up reaction enthalpies, or dissolution enthalpies.  \n\nOf the compounds you listed, Ammonia (NH3) is a weak base that will not do anything special when added to water, Nitric Acid (HNO3) is a very strong mineral acid that dissolves exothermically, Sodium Sulfide (Na2S) is an ionic salt that should dissolve without any fireworks, and Hydrogen Cyanide (HCN) is a somewhat weaker acid that I would expect to give off less heat than HNO3 when dissolved in water.
356281
MgCO3 + 2HCl ---> MgCl2 + CO2 + H2O\n\n2HCl + MgO ---> H2O + MgCl2\n\nBarium hydroxide is a base so can be neutralised with any acid.  An example being HCl.\n\nBa(OH)2 + 2HCl ---> BaCl2 + 2H2O\n\nor H2SO4\n\nBa(OH)2 + H2SO4 ---> BaSO4 + 2H2O
774296
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.
720236
1) Bi carbonate buffer system will contain HCO3- ion\n\nwhen a base is added it will liberate the H+ and produce water combining with OH- ion of the base there for reducing the effect of the base\n\nand when an acid is added it will accept the H+ ion and for H2CO3 therefor the effect of the acid will be nullified!!!\n\n2)phosphates are H2O4- or HPO42-\n\nand it will also have the functions as mentioned in the above!!\n\n3)proteins have an NH2 group and well as a COOH group both attached to the same molecule!!!\n\ntherefor when acid is added the NH2 group will neutralize it\n\nand when a base is added COOH group will neutralize it  reducing the alkalinity!\n\nthere for all these chemicals found in the blood and other body tissue will maintain the blood pH level at a constant level acting as natural buffers!!\n\nhope you understood!!!!!\n\ncheers!!
752752
Basic aluminum carbonate.
774155
This dissociates into Cl- and\n(CH3)2NH2+\n\nCl- is an extremely weak base, so weak in fact that it is neutral\n\n(CH3)2NH2+ on the other hand is a regular weak acid that will make the solution acidic.