How many moles of ammonium ions are in 8.754g of ammonium carbonate?

A 22.5 gram sample of ammonium carbonate contains 4.5 moles of ammonium ions.

As the formula for ammonium carbonate is (NH4)2CO3, there are two moles of ammonium for every mole of ammonium carbonate. Just double the given number.

There are 9 moles of NH4 (Ammonium ions) in Ammonium carbonate. There are 2 moles of NH4 per molecule and 4.5 molecules, so 2 moles times 4.5 is 9 moles.

Ammonium carbonate = (NH4)2CO3. Its molar mass is 96g/mol. 6.965g/96 = 0.7255mol.

Number of moles = Weight (in g) / Molecular mass (in g/mol) = 8.718 / 96.09 = 0.0907 moles

Yes. An aqueous solution of ammonium carbonate would consist of dissociated ammonium ions and carbonate ions.

There are 2.8604 moles of ammonium ions in 6.955.

Ammonium carbonate is (NH4 )2 CO3 and the molar mass is 96.0878 so you just divide 8.790 g/96.0878 and you get 0.91478835 and since there are two ammonium (NH4 )2 ions you multiply 0.91478835 * 2 and get 0.1830 mol.

The most common form of solid ammonium carbonate is a hydrate with formula (NH4)2CO3.H2O and a gram formula unit mass of 114.10. The formula shows that each formula unit contains 2 ammonium ions. The number of formula units of ammonium carbonate is 8.903/114.10 or 0.078028. The number of formula units of ammonium ions is twice this, or 0.1561, to the justified number of significant digits.

assuming that 8.778 is in grams then there are 0.1069 moles in 8.778 grams of ammonium carbonate here is the math:(NH4)2CO3 N2=14.01g H8=8.08g C=12.01g O3=48.00 14.01+8.08+12.01+48.00=82.10g/mole 8.778g X 1 mole/82.10g=0.1069moles

It is ionic as it is composed of polyatomic ions.

5,0 moles (NH4)2S contain 60,22140857.10e23 ammonium ions.

All ammonium salts (containing NH4+ ions) are soluble.

"Polyatomic ions", like carbonate (CO32-) and ammonium (NH4+)

Ammonia bicarbonate is nothing at all (nor is ammonia carbonate). Ammonium bicarbonate is a real chemical, and it has formula NH4HCO3 (the combination of ammonium ion (NH4+) and the bicarbonate ion (HCO3-). Ammonium carbonate is a similar chemical with formula (NH4)2CO3, and is the combination of 2 NH4+ ions with one carbonate ion (CO32-).

Yes these ions are soluble. They form ammonium chloride.

Ammonium ions have a charge of +1 and Chromate ions have a charge of -2. When these ions react, they form Ammonium Chromate; 2NH4CrO4

Calcium carbonate is rather INsoluble, so there is no solution of it. I do not know why ammonium oxalate is added to a calcium carbonate solution. Calcium oxalate will then precipitate out of the solution. The ammonium and carbonate will create a weakly bond compound. Actually, more of the ammonium ion will be in solution as free ammonia and more of the carbonate ions will be in solution as free carbon dioxide. That is the nature of those two substances. So, you will have a solution that has a calcium oxalate precipitant on the bottom and is slowly giving off ammonia and carbon dioxide.

NH4+ is the ammonium ion. Ammonium phosphate is (NH4)3PO4 containing ammonium ions and phosphate ions, PO43-

As a compound the substance has neither a valence nor an atomic number. Only elements have atomic numbers. Only atoms and ions have valences.

No. If you add ammonium chloride solution to potassium chloride solution all that happens is a solution with all the ions in it - ammonium ions, potassium ions, chloride ions and hydroxide ions.

examples include: hydroxide ions carbonate ions nitrate ions Sulphate ions Hydrogen Carbonate ions

Ammonium chloride is NH4Cl, it contains NH4+ ions and Cl- ions

K2SO4 ==> 2K^+ and SO4^2- ions. So, each mole of K2SO4 produces 3 moles of ions.2.40 moles K2SO4 x 3 moles ions/mole K2SO4 = 7.2 moles of ions.

Carbonate ions have a negative charge, and they therefore repel other carbonate ions (like charges repel, as described by Coulomb's Law). You can only have a group of carbonate ions in a material if that material also contains positively charged ions which will attract the negatively charged carbonate ions. Calcium carbonate is an example of such a material.