Consider the reaction of 30.0 mL of 0.235 M BaI₂ with 20.0 mL of 0.315 M Na₃PO₄. 3 BaI₂(aq) + 2 Na₃PO₄(aq) → Ba₃(PO₄)₂(s) + 6 NaI(aq) If you have 0.00705 moles of BaI₂, What quantity in moles of precipitate are produced if all the BaI₂ were consumed based on the balanced chemical equation?
Consider the reaction of 30.0 mL of 0.235 M BaI₂ with 20.0 mL of 0.315 M Na₃PO₄. 3 BaI₂(aq) + 2 Na₃PO₄(aq) → Ba₃(PO₄)₂(s) + 6 NaI(aq) If you have 0.00705 moles of BaI₂, What quantity in moles of precipitate are produced if all the BaI₂ were consumed based on the balanced chemical equation?
Chemistry
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Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Consider the reaction of 30.0 mL of 0.235 M BaI₂ with 20.0 mL of 0.315 M Na₃PO₄.
3 BaI₂(aq) + 2 Na₃PO₄(aq) → Ba₃(PO₄)₂(s) + 6 NaI(aq) If you have 0.00705 moles of BaI₂, What quantity in moles of precipitate are produced if all the BaI₂ were consumed based on the balanced chemical equation?
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