# How can I make AgNO3 more basic? [closed]

Is there anything that I can add to the AgNO3 solution that will make it more basic without forming a precipitate such as reacting with OH or HCl? Please be more specific and give an example.

• You are requesting to be more specific but could you explain more of this context, why do you want to increase the pH of the silver salt? What is the experimental requirement? – M. Farooq Apr 8 at 15:45
• Because I am trying to then react to the solution of AgNO3 with NaCl to check if a more basic solution could affect the amount of precipitate formed because there will be a change in activation energy. I also used HNO3 solution to make the solution of AgNO3 more acidic and it worked so I wanted to see if there will be a difference with a basic solution. Do you also think if I used complexation of ammonia, would that give us a strong base and would that work for my experiment? – General MO7 Apr 8 at 16:59
• The reaction of AgNO3 with NaCl is $quantitative$ as long as the silver ions are in solution (as long as the pH is acidic ,say < 6). By definition, a basic solution implies the presence of -OH ions in water, so silver ions will react with base and NaCl (both). There is no way to circumvent this problem. There is no point in spending time on this problem. – M. Farooq Apr 8 at 17:09
• Just one last question for your valuable comments. I want to do a catalyst in my experiment, so then I decided on doing acid-base catalysis and the problem is that I won't be able to do a base as a catalyst (would [Cu (NH3)4(H2O)2] 2+ work or does it also has OH ions?) so in conclusion, do you have any idea for any other way to add a catalyst or if not even a variable apart from temperature and concentration that would probably result in a higher amount of precipitate. I know these are a lot of questions to ask but I have an essay due very soon and you're comments are very useful. thanks!!! – General MO7 Apr 8 at 18:22
• I still do not understand your research topic. What is the topic? Every alkaline solution in water has -OH ions. That is it. You cannot avoid them by any means. – M. Farooq Apr 8 at 20:56

If you dissolve silver nitrate $$\ce{AgNO_3}$$in water, and add some NaOH solution to make it basic, it will destroy your substance, and produce a brown precipitate of silver oxide $$\ce{Ag_2O}$$ : $$\ce{2 AgNO_3 + 2 NaOH -> Ag_2O + 2 NaNO_3 + H_2O}$$
But instead of using a hydroxide like $$\ce{NaOH}$$, you may add some ammonia solution $$\ce{NH_3}$$. In this case you will produce some $$\ce{Ag_2O}$$ in the very beginning, but this dark precipitate will soon be dissolved by more ammonia, and a nearly colorless solution of diamminosilver(I) is obtained : $$\ce{2 Ag^+ + 2 NH_3 + H_2O -> Ag_2O + 2 NH_4^+}$$$$\ce{Ag_2O + 4 NH_3 + H_2O -> 2 [Ag(NH_3)_2]^+ + 2 OH^-}$$