Using the Ksp for calcium iodate hexahydrate, calculate the molarity of calcium ions. Using the Ksp...
Using the Ksp for calcium iodate hexahydrate, calculate the molarity of calcium ions.
Using the Ksp for calcium iodate hexahydrate, calculate the molarity of iodide ions
Ksp=7.10*10^-7. This is the reaction: Ca(IO3)2--->Ca+2IO3
I did an ice table, and using the Ksp of calcium iodate hexahydrate, I derived the solution as following:
cuberoot(7.10*10^-7)/(4), the answer I got was .00561995. Since this is the value of S, twice that amount should be the Iodide ions, which is around .0112399.
So did I do my math correctly, and if so, how many sig figs should I use? Shouldn't it be 2? Thank you!
Homework Answers
Your maths is absolutely correct. The no of significant figure should be 3 as there are three significant figure in Ksp value. In that case concentration of iodate ions will be 0.011M
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Using the Ksp for calcium iodate hexahydrate, calculate the
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