The concept used is to calculate the concentration of .
The solubility product, is the equilibrium constant for a solid that is dissolved in a solution. It is the product of the concentration of the products raised to the power of their coefficients.
is the measure of hydrogen ion concentration. Lower the
, higher is the hydrogen ion concentration and lower is the hydroxide ion concentration.
Higher the , lower is the hydrogen ion concentration and higher is the hydroxide ion concentration.
The hydrogen ion concentration is calculated as follows:
The hydroxide ion concentration and
are related as follows:
1.
The hydrogen ion concentration is as follows:
The hydroxide ion concentration is as follows:
The given salt is .
Its dissociation in water is as follows:
The expression for the solubility product is as follows:
Substitute the values of solubility product and the hydroxide ion concentration in the formula for solubility product and calculate the concentration of as follows:
Therefore, the is
.
Above what Fe2+ concentration will Fe(OH)2 precipitate from a buffer solution that has a pH of...
Above what Fe2 concentration will Fe(OH)2 precipitate from a buffer solution that has a pH of 8.62? The Ksp of Fe(OH)2 is 4.87×10-17.
Above what Fe2+ concentration will Fe(OH)2 precipitate from a buffer solution that has a pH of 8.60? The Ksp of Fe(OH)2 is 4.87 x 10^-17.
above what Fe2+ concentration will Fe(OH)2 precipitate from a
buffer solution that has a pH of 8.42? the Ksp of Fe(OH)2 is
4.87x10^-17
Question 28 of 31 > Attempt 6 - Above what Fe2+ concentration will Fe(OH), precipitate from a buffer solution that has a pH of 8.42? The Kp of Fe(OH), is 4.87x10-17 [Fe2+1 = 1.95 x10-11
Above what Fe2+ concentration will Fe(OH)2 precipitate from a buffer solution that has a pH of 8.83 ? The ?sp of Fe(OH)2 is 4.87×10−17.
Above what Fe2+ concentration will Fe(OH)2 precipitate from a buffer solution that has a pH of 8.14 ? The ?sp of Fe(OH)2 is 4.87×10−17.
Above what Fe2+ concentration will Fe(OH)2 precipitate from a buffer solution that has a pH of 8.57 ? The ?sp of Fe(OH)2 is 4.87×10−17.
Above what Fe2+concentration will Fe(OH)2 precipitate from a buffer solution that has a pH of 9.30? The ?sp of Fe(OH)2 is 4.87×10−17. [Fe2+]=_______M
Above what Fe2+ concentration will Fe(OH), precipitate from a buffer solution that has a pH of 8.83? The Ksp of Fe(OH), is 4.87x10-17. [Fe2+] =
+ Above what Fe2+ concentration will Fe(OH), precipitate from a buffer solution that has a pH of 8.08? The Ksp of Fe(OH), is 4.87x10-17. [Fe2+] = M
Above what Fe2+ concentration will Fe(OH), precipitate from a buffer solution that has a pH of 9.56? ut The Ksp of Fe(OH), is 4.87x10-17 ЬВ Fe2]= ЬВ Ьвr