Why is ammonia considered a weak base?
819664
The lone pair of electrons on the Nitrogen atom of Ammonia, is available for donation. That is why ammonia is considered as a base. \nBut it not as readily available as it is From OH- radical or other basic radicals. So it is much weaker than them.\nIn aq. soln, NH3 combines with water to form a very weak electrolyte NH4OH, which gets dissociated to a very small extent furnishing only a few OH- ions. So the aq. soln. of NH3 is also mild basic.\n\n Ammonia acts both as a weak base in the Brernsted-Lowry sense\nNH3 + H2O = NH4(+) + OH(-)and\nas a complexing agent (Lewis acid) with some metal ions\nZn(2+)+ 4NH 3 + Zn(NH3)4(2+)\nBoth weak and strong bases produce hydroxide ion in solution which precipitates some metal ions, e.g.\nA13(+) + 30H- + Al(OH)3(s)\nand Zn92+) + 20H- + Zn(OH)2(s).\nThese precipitates appear as flocculent white solids which settle slowly from solution. In higher\nconcentrations hydroxide ion acts as a complexing agent for amphoteric cations, e.g.\nZn(OH)2(s) + 2OH- -+ Zn(OH),2-\nAl(OH)3(s) + OH- -+ A1(OH)4-\nThis experiment demonstrates the action of OH- and NH3 on Al”(aq) and Zn*‘(aq) ions.\n\nAlthough ammonia is well-known as a base, it can also act as an extremely weak acid. It is a protic substance, and is capable of dissociation into the amide (NH2−) ion, for example when solid lithium nitride is added to liquid ammonia, forming a lithium amide solution:\n\n        Li3N(s)+ 2 NH3 (l) → 3 Li+(am) + 3 NH2−(am)\n\nThis is a Brønsted-Lowry acid-base reaction in which ammonia is acting as an acid.\n\nI think you are interested about dry ammonia.
419911
That's easy. [Co(NH3)6]Cl3. This is coordination chemistry, dude. There can be other products depending on the ammonia concentration. But this is your best bet. I've been doing these reaction in the lab way way back.
618488
Look at their conjugate bases and whichever is more stable will have the weakest acid. PKA values are also easy to prove this becuase it is a realtion of the H+ content.
438289
Co(NH3)4 would be more likely
656515
I hate it too. By the way it's NH3 - Ammonia that is formed. I got little time left. I'll answer later.
263373
Are you sure this is a weak acid? Because to solve a weak acid dissociation problem you'll need the Ka value for that specific acid. Strong acids dissociate fully, so those are easier.\n\nFor a strong acid, it's simple stoichiometry. The HY acid dissociates completely, and you'll end up with 0.02 M HY left.\n\nFor a weak acid, you'll need to set up an ice table, with the K value.\n\n   HY + OH- --> Y- + H2O K = ?\nI 1.0  0.980    0    ---\nC -x   -x       +x   ---\nE 1-x  .98-x    x    ---\n\nSo, the equation you'll get is K = x/((1-x)(0.98-x)). If you can find the Ka value (from a book or something, then you can figure out the rest of the values by solving the equation.\n\nEDIT: My table isn't displaying correctly, but just move those values over to the correct columns.
518533
first one: no, your missing an Mn on the right.\nSecond one: yes\nthird one: no, you're missing 5 ammonia on the left\n\nthe rest as standard metathesis reactions, use the ones u've done as a guide
787213
Ammonium (NH4+) is a polyatomic ion.  That means that it is composed of a group of atoms that are covalently bound together.  As a whole, that group has a charge of +1.  \n\nBecause this group of atoms has a charge, it is an ion, and can form ionic bonds with other ions.  So in summary, ammonium itself is a covalent compound, but it is able to form ionic bonds with other substances.
233434
This is just a simple stoichiometry problem.  You have 200g of NH3, your first job is to calculate how many moles of NH3 this is.  From the periodic table, find the atomic weights of N and H to calculate the molar mass of NH3:  \n\nN=14 and H=1, so NH3 = 17.  \n\n200g NH3 X (1 mol NH3 / 17g NH3) = 11.76 mol NH3\n\nOkay, now that we know we're working with 11.76 moles of NH3, we can use the mole ratio from the given chemical equation to figure out how many moles of oxygen are needed.  Look at the coefficients in the equation -- we need 5 moles of O2 for every 4 moles of NH3:\n\n11.76 mol NH3 X (5 mol O2)/(4 mol NH3) = 14.7 mol O2\n\nNow we know we need 14.7 mol O2.  All we have to do now is convert that to grams, again using the atomic mass from the periodic table.  The atomic mass of O is 16, so O2=32  \n\n14.7 mol O2 X 32g/mol = 470.4 g O2\n\nSUMMARY:\nConvert grams ammonia to moles ammonia using atomic weights.\nUse the mole ratio to determine needed moles of O2.\nConvert moles O2 to grams O2 using atomic weights.
707264
Methylamine (CH3NH2) and methylammonium chloride (CH3NH3Cl) would be a good buffer in both are in solution together in appreciable concentrations.\n\nNitrates, chlorides, and sulfates (either as acids or salts) will not act as buffers as those anions have no tendency to act as bases (they are the anions from strong acids, which are "strong" because they dissociate completely in solution).  The same with alkali metal hydroxides, which are strong bases.
221937
N2+ is a meta director because it's positively charged. If something added o/p, there would be a +charge next to the already +ve N2, which is very bad. NH2 is an o/p director, because it has lone pairs which help stabilise an adjacent +charge.\n\nAbout toluene - it all depends on the relative strengths of the directing, so there's no general case, though resonance effects will usually take precedance over inductive effects.
771216
weak bases only dissociate a very small amount, while strong bases dissociate almost fully.
713316
HNO3\n\nIf you couldn't answer this question, you must be a real noob in chemistry!!  Well, for other times, here's the way to differentiate betwee acids and bases.\n\nAcids:   acids can be easily identified by the hydrogens they contain.  Most acids have their hydrogen in the beginning of their formula.  HNO3 can be easily identified as an acid: it is commonly called nitric acid.\n\nBases:  most bases can be identified by the (OH) group at the end of their formula... therefore, we can immediately label b) and d) as bases.   \n\nNow here, NH3 is kind of tough to define with the definitions given above.   I believe that the proper explanation is out of your scope for know (from what I can deduce).   So, you'll learn that later on.  But for your info, NH3 is ammonia, the stuff they use in cleaning fluids, and it is basic.\n\nHope this helps.
84416
Yeah, whoever said that Windex was acidic is a little confused.  \nWindex's main ingredient is ammonia, which is NH3.  When ammonia is dissolved in solution like in Windex, it forms ammonium hydroxide, NH4OH.  Windex has that ammonia smell to it, right?  This ammonia ingredient puts Windex's basic pH at around 12; ammonia is a weak base.  You can always find out for yourself by getting some pH or Hydrion paper and testing Windex.
364809
hey do u mean bases in chem.? well if it is in chem, then a base is not an alkali! a base is a compound which reacts with the hydronium ions of an acid to give salt and water only. they are insoluble in water but an alkali is soluble in water. Hence all alkali's are bases but all bases are not alkali's. eg of a base Cuo and of an alkali KoH
468312
Potassium hydroxide is a strong base.\nKOH -> K+ + OH-\n\nWater doesn't participate directly in the reaction, so you can leave out the H2O on both sides. Because KOH is a strong base, it's pretty accurate to just have the arrow pointing one way in the reaction -- almost all of the KOH disassociates. For weak acids and bases, instead of an arrow pointing just in one direction, you need a bidirectional arrow to show that both sides of the equation are present in the solution. For example,\nH2CO3 <---> H+ + HCO3-
486317
This might not make much sense, but I think it might be\n2,4-Cyclohexadiene with an ammonia substituent.