What is the actual charge on hydrogen and actual charge on chlorine in HCl?
820135
it depends on the medium the H-Cl is in.\n\n---------------------------\n\nin its pure gaseous form, there is no charge on either H or Cl.  It is just a covalent bond.  Because Cl is considerably more electronegative than H, this covalent bond is polar, giving a partial positive charge to the H and a partial negative to the Cl.\n\nif you dissolve H-Cl in water, then the water splits (solvates) the H-Cl into its ions, H+ and Cl-, thus giving H a plus 1 charge and Cl a minus 1 charge.
476459
The difference between \n\n1) HCl-->.H(g)+.Cl(g)   and\n\n2) HCl(g)-->H^+^(g)+ Cl^-^(g)\n\nis that in equation 2, you have two charged species.  We know that a positively charged species likes to interact with a negetively charged species (coulombic effect), thus making them much harder to dissociate.  This is what your hint was trying to address.  \n\nIn the gas phase, there also do not exist any solvents or counterions to stabalize the charged products in reaction 2.  The only reason that NaCl dissociates in water is due to the dipole moment of water which helps stables the Na^+^ abd CL^-^ ions.  In the gas phase, these don't exist so you would be hard pressed to acheive equation 2.
127210
Hydrochloric acid will react with metals ABOVE Hyrogen in the activity series of metals to produce Hydrogen gas.\nThe metals will displace Hydrogen from the acid and make a metal salt (which is usually in solution).\n\nSo if we say that [A] is a generic metal above Hydrogen in the activity series that has a normal oxidation state of +1, then the reaction would be as follows,\n[A] (s) + HCl (aq) --> H2 (g) + [A]Cl (aq)
133194
This usually happens in solution, the Chlorine is a chloride ion.\n\nAgNO3(aq) + Cl-(aq) --> AgCl(s) + NO3-(aq)
237970
Hi,\n\nThe number of neutrons is the atomic mass minus the atomic number. \n\nThe isotopes of chlorine vary from 031 to 047 out of which isotope 35 and 37 are the stable ones. \n\nChlorine has 17 protons. So,\n\nfor Chlorine 35, it is 35 - 17 = 18 neutrons. \n\nthe same way,\n\nfor Chlorine 37, it is 37 - 17 = 20 neutrons. \n\nThus,\n\n17 protons plus 18 neutrons make chlorine-35. \n\n17 protons plus 20 neutrons make chlorine-37.
732214
Ca is II A elements which have 2 valence electron. Therefore it charges are 2+. Chlorine charges is -1 because of it have 7 valence electron. \nHence, to make a compound neutral one Ca must make bonds with two Chlorine, making CaCl2.\n\nNa is I A elements which have 1 valence electron. It have a charge of +1. Hence, to make the chloride of natrium, one natrium only can make a bond with one chlorine atom, resulting in NaCl.\n\npeace\nvixklen
1030535
Well, this is easy. Just look at each species and see if its oxidation state is going up or down. I'll do the first one--the rest are the same.\n\nH2S + Cl2 --> 2HCl + S\n\nWell, the sulfur is going from a -2 state to a 0 state. This means it's oxidizing. The chlorine is going from a 0 state to a -1 state. This means it's reducing. So, the sulfur is the reducing agent (because it's making the chloringe reduce) and the chlorine is the oxidizing agent. Be careful--oxidizing agent actually means it's reducing.\n\nSolve the other two the same way.
608403
NaOH (aq) + HCl (aq) --> NaCl (aq) + H2O (l)
1167951
HgCl2 - 0.48 mol / 100 mol water at 25 degrees C\nHg2Cl2 - very insoluble in water
242316
Add up the charges in the molecule. Like, in ClO4-,\n\nOxygen has an oxidation state of -2 by default. Therefore, Cl must have an oxidation state of +7 to balance out the oxygens. Notice that 7 + (-2)*4 = -1, which is the charge of the ion.\n\nThe oxidation state of Pb in PbSO4 is +2, because the sulfate ion has an charge of -2. To balance this out, the Pb must be +2, as there is no charge on the molecule.\n\nHope this helped.
573821
I think this question is incomplete because the Ka of HF hasn't been provided.  The amount of H+ that is formed from HF can only be calculated from its Ka value.
971905
First, look at the oxygen.  Oxygen has a charge of 2-, and there are 4, so in the entire molecule, oxygen gives a charge of 8-. The total charge of the molecule is 1-, therefore to find Cl, create the equation -8+x = -1\nx=7\nTherefore chlorine has a charge of 7+\nThe total charge of the molecule = the sum of the charges of each atom
272349
Ca(s) + 2HCl(aq)-->CaCl2 + H2(g)\n\nor...\n\nCalcium Chloride and Hydrogen Gas... you know... the stuff that fuels rockets! :)
272575
let me explain this with an example.take Cl atom which has 17 protons in the nucleus and equal no. of electrons(17)revolving around the nucleus.this means tht the 17 positive charges are attracting the 17 negative charges.\nnow let us consider the chloride ion Cl(-1). the protons are again 17 here but one negative charge is extra ie there are 18 electrons.so,in this case the 17 positive charges are pulling the 18 negative charges.\nnow u can imagine in which case is the pull less efficient atom or anion?\nobviously it is less efficient in case of anion because of the inequality of charges thus making it bigger in size.\nhope ,i ve made it clear with an example...
208043
It is a positive charge, since there is no electron. Often, a naked hydrogen atom also won't have a neutron either, so you will often see the term proton depicted as H+ and vice versa.
151049
Yes, everyone is correct.  They are all the same thing.  \nHowever, because HCl is not an ionic compound (it is a molecule), molecular nomenclature may apply.  Molecular nomenclature for binary compounds utilizes prefixes, so another name for HCl may be hydrogen monochloride.  \nAnother note is that hydrogen chloride is a gas, whereas hydrochloric acid is that gas dissolved in water.  They're not exactly the same thing.  Without a phase symbol, HCl could refer to either.
811335
when bonding takes place by sharing of electrons then it is said to be covalent bond. now it can be possible in two ways.\n\nfor eg if two hydrogen are combining to form a bond then they both will share one electon each and the force applied from there nucleus will be same so the elecron pair will remain nearly equal with both the hydrogen.so you can say that it remains exactly at centre from both the nucleus\n\nbut if you consider HCl. here also both hydrogen and chlorine are going to share one elctron each when bond formation takes place. but as electronegativity of chlorine is quite high(ie its attraction from nucleus is quite high) compared to that of hydrogen so eventhough they both have shared one electron each but still electron pair will remain towards chlorine.\n\ni hope this will help you out