A 170.0 mL170.0 mL solution of 2.288 M2.288 M strontium nitrate is mixed with 220.0 mL220.0 mL of a 2.493 M2.493 M sodium fluoride solution. Calculate the mass of the resulting strontium fluoride precipitate. mass: Assuming complete precipitation, calculate the final concentration of each ion. If the ion is no longer in solution, enter a 0 for the concentration. [Na+]= [NO−3]= [Sr2+]= [F−]=
A 170.0 mL170.0 mL solution of 2.288 M2.288 M strontium nitrate is mixed with 220.0 mL220.0 mL of a 2.493 M2.493 M sodium fluoride solution. Calculate the mass of the resulting strontium fluoride precipitate. mass: Assuming complete precipitation, calculate the final concentration of each ion. If the ion is no longer in solution, enter a 0 for the concentration. [Na+]= [NO−3]= [Sr2+]= [F−]=
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Chapter4: Chemical Reactions
Section: Chapter Questions
Problem 4.81QP: A 8.50 g sample of KCl is dissolved in 66.0 mL of water. The resulting solution is then added to...
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A 170.0 mL170.0 mL solution of 2.288 M2.288 M strontium nitrate is mixed with 220.0 mL220.0 mL of a 2.493 M2.493 M sodium fluoride solution. Calculate the mass of the resulting strontium fluoride precipitate.
mass:
Assuming complete precipitation, calculate the final concentration of each ion. If the ion is no longer in solution, enter a 0 for the concentration.
[Na+]=
[NO−3]=
[Sr2+]=
[F−]=
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