Stoichiometry Question
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K2HPO4 is a highly water-soluble salt that is used as a buffering agent, fertilizer, and food-additive. It can be formed by the neutralization of phosphoric acid with potassium hydroxide, as shown by the chemical equation below:
H3PO4+2KOH→K2HPO4+2H2O
1.00x102g of phosphoric acid (H3PO4) reacted with excess potassium hydroxide. The final mass of K2HPO4 produced is found to be 1.63×102g. How would you find the percent yield?
H3PO4+2KOH→K2HPO4+2H2O
1.00x102g of phosphoric acid (H3PO4) reacted with excess potassium hydroxide. The final mass of K2HPO4 produced is found to be 1.63×102g. How would you find the percent yield?
- Multiply the actual yield and the theoretical yield.
- Multiply the actual yield and the theoretical yield and divide by 100.
- Divide the actual yield by the theoretical yield and multiply by 100.
- There is no percent yield.