The solubility of AgCN will be minimum in pure water/acidic buffer/basic buffer/remain same in all.?
471060
basic buffer... beacuse CN- will need H+ which is least in basic buffer
911906
....Sorry, but your question is unclear.  \n\nRephrase?\n\nMethyl Alchohol is soluble in water, so there is usually some slight energy expended as the solute dissolves in the solvent.  But other than that, I can't see what effect could occur related to pH or buffer capacity.
962694
Tehe answer is:\nAg + HNO3 -> AgNO3 + H\nAgNO3 + KBr -> AgBr + KNO3
828232
As I've answered elsewhere, the solubility of the Group 2 sulphates decreases as you go down the group. MgSO4 is reasonably soluble, therefore, but BaSO4 is pretty insoluble.
1022579
This is a poorly worded question.  All chemicals have some solubility in water, however minute.\n\nOf these selections, I would go with A\n\nAdding a charge facilitates dissolution.\nMany covalent materials (oil) have low solubility \nMany large molecules are water soluble (Poly Ethylene Glycol)
271476
pH = 4.75\n\ntechnically, the pH can be anything.  But, for the most effective acetic acid buffer, the pH would be 4.75 because the pKa of acetic acid is 4.75.  When the pH = pKa, the amount of acid and base are equal, thus its resistant to pH changes is greatest.
670034
Ag+ will precipitate in HCL solution as AgCl, but as for Ag(NO3), i am not so sure.
760563
N=aM where a is the valency (depending on the type of chemical and reaction, e.g. number of H+/OH- for acid/bases per molecule, number of electrons gained/lost in redox reactions).\n\nFor AgNO3 a=1 (it is Ag+ so for redox or precipitation reactions it gives one equivalent group per molecule)\n\nSo M= N/a = N/1 =N\n\n1 M is 169.87 g/L =16.987g/100mL =16.987%\n\nUse M1*V1=M2*V2\n16.987*V1=1*V2\nV1 is the volume in mL of the stock solution that you will use to prepare V2 mL of 1%\nYou didn't specify how much you want to prepare...\n\nAlternatively you could have converted 1% to mole/L and do the math with molarities.
799604
If the ionic compound is soluble, no precipitate is formed.\n\nOn the other-hand, if an ionic compound is not very soluble in the solvent, then it will precipitate out of solution.\n\nFor example, Sodium chloride is soluble and Silver nitrate is soluble, but if these solutions are mixed, some of the Silver ions will react with chloride ions and form solid Silver chloride precipitate.
238675
If the reactants are in aqueous solution, in high enough concentrations, then solid silver chloride (AgCl) will precipitate. Sodium nitrate wiill remain in solution as sodium and nitrate ions. No chloride ions should remain - they will all have reacted with the silver ions.\n\ni.e.   AgNO3 + NaCl  + NaNO3   ->    AgCl  +   NaNO3\n\nDon't forget to balance the equation.
518629
not too much, they are both basic, and don't really react. even if it is an aqueous solution of ammonia (thus avoiding the gas problem above)
122833
pH level, buffering capacity (alkalinity), general hardness and salinity
320284
It is not possible.  Observe the chemical equation:\nAg2SO4(s) + AgNO3(s) --> Ag2SO4(s) + AgNO3(s)\n\nIn order for a substance to dissolve, it must be in an aqueous solution.
416321
There is no such thing as a concentrated solution of the carbonic acid, as only a small amount of carbon dioxide will dissolve in water. Also, they are the same color, colorless in the pure form.
982289
low solubility; im sure
763435
It will decrease if the solubilizing of the solid is endothermic, and increase if it is exothermic.\n\nIn most cases, solubilizing is endothermic (it takes heat to break up a solid and get the ions to stay in solution) so it will generally decrease, but this is not always the case.
766207
The pH of the buffered aspirin is between 8-10.  What is really important is not the pH itself but the pH at which the coating will disoolve.  You do not want the coating to dissolve at low pH in the stomach, but to do that in the relatively higher pH of the intestin where it can be absorbed.