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I have no clue how to do the double displacement method thing so if anyone wants to help me that would be great :-)
The question is:
Write the complete ionic equation for the double displacement reaction that occurs when aqueous solutions of barium nitrate, Ba(NO3)2 and sodium chromate (Na2CrO4) are mixed.
I didn't understand it when we did it in class and when I went to her for help she refused to help me
<3 Ashley
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First of all, double replacement not double displacement.
Ba(NO3)2 + Na2CrO4 => NaNO3 + BaCrO4 I believe.. Then cancel spectator ions then you got your net ionic equation.
Armando wrote:First of all, double replacement not double displacement.
Ba(NO3)2 + Na2CrO4 => NaNO3 + BaCrO4 I believe.. Then cancel spectator ions then you got your net ionic equation.
You forgot to balance it, but the method is correct. There should be a two in front of NaNO3
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Correct, I accidentally oversaw that ;)
Armando wrote:First of all, double replacement not double displacement.
Ba(NO3)2 + Na2CrO4 => NaNO3 + BaCrO4 I believe.. Then cancel spectator ions then you got your net ionic equation.
Thanks. And it can be called double displacement. Its either or.
<3 Ashley
Write the complete ionic equation for the double displacement reaction that occurs when aqueous solutions of barium nitrate, Ba(NO3)2 and sodium chromate (Na2CrO4) are mixed.
Since nitrates and alkali metals are always soluble, the reactants should have been broken up into ions.
Ba 2+ + NO3 - + Na + + CrO4 2-
Then switch the ions over, hence double replacement, to get
Ba 2+ + CrO4 2- + Na + + NO3 -
BaCrO4 is insoluble, so it should be written as BaCrO4 (s) while NaNO3 is soluble, so it should still be written as two ions in the product side as Na + and NO3 -. Since Na + and NO3 - appear on both sides of the equation, you can cancel them out and the final complete ion reaction is
Ba 2+ + CrO4 2- --> BaCrO4 (s)