Asked by carolin
Consider the reaction of 14.20ml of 0.141 M H3PO4 and 0.0521 M Ba(OH)2.
2H3PO4 + 3Ba(OH)2 ->Ba3(PO4)2 + 6HOH
What volume of Ba(OH)2 is required to completely react with the H3PO4?
2H3PO4 + 3Ba(OH)2 ->Ba3(PO4)2 + 6HOH
What volume of Ba(OH)2 is required to completely react with the H3PO4?
Answers
Answered by
DrBob222
mols H3PO4 ==> M x L = ?
Use the coefficients in the balanced equation to convert mols H3PO4 to mols Ba(OH)2.
Now M Ba(OH)2 = mols Ba(OH)2/L Ba(OH)2. You know mols and M, calculate L.
Use the coefficients in the balanced equation to convert mols H3PO4 to mols Ba(OH)2.
Now M Ba(OH)2 = mols Ba(OH)2/L Ba(OH)2. You know mols and M, calculate L.
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