Consider the following reaction: Q + R --> S
15.0 mL of a 2.10 M solution of "Q" and 12.0 mL of a 1.50 M solution of "R" are mixed together. The concentration of S in the new, combined solution is found to be 0.37 M. What is the magnitude of the equilibrium constant (K) for this system?
I know the answer to this question is 1.57 but i cant figure out how to get that? Could you please show each step to reach that number?
Consider the following reaction: Q + R --> S 15.0 mL of a 2.10 M solution...
When 15.0 mL of a 9.60x10-4 M barium sulfide solution is combined with 12.0 mL of a 1.40x10-5 M potassium sulfate solution does a precipitate form? (yes or no) For these conditions the Reaction Quotient, Q, is equal to
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ksp was not provided in the question
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