Will rate best explaination The solubility product constant for Ba(IO3)2 is 1.57
ID: 795206 • Letter: W
Question
Will rate best explaination
The solubility product constant for Ba(IO3)2 is 1.57timesl0-9 at 25 degree C. What is the molar concentration of IO3- ions in a saturated solution of Ba(IO3)2? Assume an ideal solution at 25 degree C. How many grams of Ba(IO3)2 (487.1 g/mol) can be dissolved in 600 mL of pure water at 25 degree C?. How many grams of Ba(IO3)2 can be dissolved in 600 mL of a 0.100 M KIO3 solution at 25 degree C? Use activities for this calculation. Activity coefficients can be found in Table 12-1 of your textbook.Explanation / Answer
Ba(IO3)_2 ---> Ba^+2 +2IO3-
SO Ksp= [Ba^+2][IO3-]^2
let concentration of Ba^+2 be X molar..then we have 2X molar concentration of IO3- ions
=> Ksp=[X][2X]^2 GIVEN Ksp=1.5 *10^-9
=> 4X^3=1.5*10^-9
=> X^3=.375*10^-9 => X=.721 *10^-3 MOLAR
WE HAVE THE MOLARITY OF Ba+2 IONS .. IF X MOLES OF Ba+2 ARE FORMED ..THAT IMPLIES X MOLES OF Ba(IO3)_2 WERE DISSOLVED
USING MOLRITY= NO. OF MOLES/VOLUME IN LITRES
.721*10^-3 = m/.6 (m BE THE MOLES FORMED.. VOLUME IS .6 L)
=> m=.433*10^-3 MOLES...SINCE THIS MUCH NUMBER OF MOLES OF Ba=2 ARE FORMED..SAME NUMBER OF Ba(IO3)_2 MOLES ARE DISSOLVED TOO...
USING MOLES = WEIGHT/MOLECULAR WEIGHT
=>.433*10^-3 = W/487.1 (MOLECULAR WEIGHT =487.1 g/mol)
=> W=.211 GRAMS .. THEREFORE .211 g OF Ba(IO3)_2 WAS DISSOLVED
KIO3 IS IONIC AND COMPLETELY DISSOSCIATES.. KIO3--->K+ + IO3-SO THE CONCENTRATION OF IO3- IS MAXIMUM CONTRIBUTED FROM KIO3..WHICH IS VERY LARGE COMPARED TO THAT FROM Ba(IO3)_2
SO NOW CONCENTRATION OF Ba+2 =X AND CONCENTRATION OF IO3- IS .1M..
kSP=[X][.1]^2
=>1.5*10^-9 =.01*X
X= 150*10-9 M
AS STATED EARLIER WE HAVE THE SAME NUMBER OF MOLES OF Ba+2 FORMED AND Ba(IO3)_2 DISOLVED
USING MOLES = WEIGHT/MOLECULAR WEIGHT
150*10^-9 =W/487.1
=> W =.073 mg OF Ba(IO3)_2 WAS DISSOLVED
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