I think you can react a soluble lead salt with a strong acid like HCl. \[Pb(NO_3)_2 + 2HCl \rightarrow PbCl_2 + 2HNO_3\]
if i conducted this in lab would i have to heat any of my reactants because i am not allowed to because or possible toxic gases forming.
Well I'm no chemist; I'm just a high school senior. You should ask your teacher or professor for supervision if you are thinking about carrying out an experiment. However, I think that reaction is spontaneous and wouldn't need any added heat to get started. With regards to safety, you might want to use Lead (II) acetate instead of Lead (II) nitrate because having acetic acid as a product would be much safer than having nitric acid (a strong acid) as a product.
all i am being provided by my teacher is lead (II) in solid form and chloride in solid form and i have to make and conduct an experiment that gives me lead (II) chloride in pure dry form
thank you so much for helping me i am a high school junior as much help as you can give would be great! this is part of one of my finals in this class and we aren't allowed to ask our teacher for help creating the process and i am stuck with this assignment
Well if you only have solid lead and chlorine, you can heat the chlorine to get chlorine gas, which will react with solid lead. \[Pb \space (s) + Cl_2 \space (g) \rightarrow PbCl_2\]
The only problem with that is that I have no idea to safely contain the chlorine gas, haha.
dang it haha i love chem but this assignment is really a pain in my butt haha there has to be another way there has to be loll would this work? \[Pb(aq) + Cl2 (aq) \rightarrow PbCl2 (s)\]
i know that would be in precipitate form? but it wouldnt be in pure dry form right?
Well, precipitate form just means that its an insoluble solid. I don't think solid lead & solid chlorine would react in water. I'm pretty sure you're going to have to apply heat somewhere.
i can apply heat to anything but not nitrate i read the email wrong but i still am stuck what would i apply heat to?
Okay, I'm a bit confused. What chemicals do you exactly have?
Sorry!! I am supplied with solid lead (II) and solid chloride
Are you sure you have solid Cl2 (s) because diatomic chlorine exists as a gas at room temperature?
hold on let me send you a picture of the sheet my teacher gave to us. it might help but i dont know if it will since it doesnt say much but it might clear up the confusion sorry its sideways i cant get it rightside up
oh nevermind its rightside up
Do you have silver nitrate or any other nitrates? There are lots of ways to make lead chloride, but the problem is that you have limited supplies...
yeah i believe we can use any chemical that is reasonable in a high school lab
Then you can use any of the following reactions to produce lead (II) chloride: If you don't have lead nitrate, but have silver nitrate, you can produce lead chloride via a two step reaction. \[Silver \space Nitrate + Solid \space Lead \rightarrow Lead \space Nitrate + Solid \space Silver\]\[2AgNO_3 (aq) + Pb (s) \rightarrow Pb(NO_3)_2 + 2Ag\]\[Lead \space Nitrate + Sodium \space Chloride \rightarrow Lead \space (II) \space chloride + Sodium \space Nitrate\]\[Pb(NO_3)2 (aq) + 2NaCl (s) \rightarrow PbCl_2 (s) + 2NaNO_3 (aq)\] If you have lead nitrate, you can just produce lead chloride via a one step reaction: \[Lead \space Nitrate + Sodium \space Chloride \rightarrow Lead \space (II) \space chloride + Sodium \space Nitrate\]\[Pb(NO_3)2 (aq) + 2NaCl (s) \rightarrow PbCl_2 (s) + 2NaNO_3 (aq)\] Instead of sodium chloride, you can also use hydrochloric acid (HCl). \[Pb(NO_3)_2 (aq) + 2HCl (aq) \rightarrow PbCl_2 (s) + 2HNO_3 (aq)\]
You should be able to find all of the reactants in those reactions in a typical chemistry lab. I would personally use the reaction with sodium chloride over HCl because you don't have to deal with a strong acid (HNO3) being formed.
Best of luck on your lab =)
THANK YOU SO SO MUCH!!!!! YOU HAVE HELPED A LOT!!!!