?Consider the reaction \(\mathrm{IO}_{4}^{-}(a q)+2 \mathrm{H}_{2} \mathrm{O}(l)
Chapter 15, Problem 15.95(choose chapter or problem)
Consider the reaction \(\mathrm{IO}_{4}^{-}(a q)+2 \mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons\) \(\mathrm{H}_{4} \mathrm{IO}_{6}^{-}(a q) ; K_{c}=3.5 \times 10^{-2}\). If you start with 25.0 mL of a 0.905 M solution of \(\mathrm{NaIO}_{4}\), and then dilute it with water to 500.0 mL, what is the concentration of \(\mathrm{H}_{4} \mathrm{IO}_{6}^{-}\) at equilibrium?
Text Transcription:
IO_4^-(a q)+2 H_2 O(l) rightleftharpoons
H_4 IO_6^-(a q) ; K_c=3.5 \times 10^-2
NaIO_4
H_4 IO_6^-
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