![]() ![]() Once I have the correct molarity of the Lithium Phosphate that is being mixed with the Magnesium Chloride and since the molar ratio of the two compounds. (this is where the discrepency between 0.0544 M and 1.63 M comes from).Īctually I see now that I have made this mistake in my explanation to you I was using 0.163 M (which is molarity of Li 1+ ion in solution) whereas I should have used 0.0544 M (the molarity of Li3PO4). I calculated this from the Ksp equation substituting the variable 'x' for the molarity of the solution and then assigning the ion concentrations appropriate values of 'x'. however I now realize that the figure of 0.163 M is actually not the molarity of Lithium Phosphate but the molarity of the ion in solution. Now I won't go into too much detail of how I calculated the Molarity of the Lithium Phosphate suffice to say I got this problem correct. Which solution has a higher lithium cation concentration? One is made by dissolving lithium carbonate ( Ksp = 8.15 x 10−4) in 100.0 mL of water until excess solid is present, while the other is prepared by dissolving lithium phosphate ( Ksp = 2.37 x 10−4) in 200.0 mL of water until excess solid is present. Īgain, two saturated aqueous solutions are prepared at 25 ✬. ![]() If I give you details of the previous problem referred to in this problem and how I calculated the molarity of the Lithium Phosphate solution being used in this precipitation reaction maybe the situation will become clearer.īelow are the details of problem 3 (the prior problem referred to) and they are as follows. I am afraid I have given you an inadequate and erroneous description of the problem I seek to understand. Doesn't your net ionic equation give you a clue? Is this correct ? If not where have I gone wrong ? Can anybody help ?Īlso note that you are going wrong because your precipitation reaction equation is not balanced. Ĭalculating it's molar mass (g/mol) and multiplying this by it's actual molarity (mol) giving the mass present of precipitate in solution after the reaction. So we now convert from moles to mass (grams) of the precipitate by. Then the molarity of Mg3(PO4)2 is also 0.163 M. Now the previously prepared saturated solution of Li3PO4 has a calculated molarity of 0.163 M so as the molar ratio of this to our saturate is 1:1 1 mole of LI3PO4 produces 1 mole of Mg3(PO4)2 (which is the precipitate). So from the reaction equation - MgCl2 + Li3PO4 -> Mg3(PO4)2 + LiCl Also the net ionic equation talked about in the problem is listed in the equations section above, but I repeat here. Note - The molarity of the prepared lithium phosphate mentioned above from a previous problem was 0.163 moles/litre (I know this is correct from the exam feedback). How many grams of the new solid precipitates? In problem #4, you wrote the net ionic equation for the reaction that results. This is my subsequent attempt to solve it after the exam (so I don't know if this attempt is correct or not) and would appreciate any input reassuring me that this, my last attempt, is correct or if wrong where I am going wrong with this type of problem.Īn aqueous solution containing excess magnesium chloride is mixed with the saturated solution of lithium phosphate prepared in problem #3. The most common examples of precipitation are Rain, Snowfall, hail, sleet, dew etc.I have a problem from an exam which I passed recently, however this was one problem I got wrong and I want to understand how to solve the thing. Question: What are examples of precipitation occur in nature?Īnswer: The precipitation occurs in nature, Type and size of ions, the concentration of an aqueous solution, pH of the solution, solubility etc. Question: What are the factors that affect the precipitation reaction?Īnswer: Factors affecting precipitation reaction are, It is a type of double displacement reaction. ![]() It is used to check out elements present in the solution. ![]() The precipitate is shown by the down arrow in the chemical reaction. The chemical reaction in which two ions combined to form one of the insoluble products in an aqueous solution that precipitated. Frequently Asked Questions: Question: What is a precipitation reaction? It affects by the type and size of ions, the concentration of an aqueous solution, pH of the solution, solubility etc.It is a type of double displacement reaction.The precipitate is shown by the down arrow in a reaction.The chemical reaction in which two ions combined to form one of the insoluble products in an aqueous solution that precipitated out.Also Read On: Alkyl Halide Examples: Detailed Insights And Facts Facts ![]()
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