Ionic EquilibriumHard
Question
Equilibrium constant for the acid ionization of Fe3+ to Fe(OH)2+ and H+ is 9.0 × 10–3. What is the maximum pH, which could be used so that at least 90% of the total Fe3+ in a dilute solution exists as Fe3+? (log 3 = 0.48)
Options
A.3.0
B.1.08
C.1.92
D.2.04
Solution
$Fe^{3 +} + H_{2}O \rightleftharpoons Fe(OH)^{2 +} + H^{+} $$$0.9x\text{ M0.1}x\text{ M}?$$
$9 \times 10^{- 3} = \frac{0.1x \times \left\lbrack H^{+} \right\rbrack}{0.9x} \Rightarrow \left\lbrack H^{+} \right\rbrack = 0.081 \Rightarrow P^{H} = 1.08$
Create a free account to view solution
View Solution FreeMore Ionic Equilibrium Questions
Which of the following will show common ion effect and form a buffer solution ?...How many moles of acetic acid should be added to 100 ml of 0.6 M formic acid solution such that the percentage dissociat...A buffer solution is prepared by mixing ′a′ moles of CH3COONa and ′b′ moles of CH3COOH such that...In which of the following, the solubility of AgCl will be maximum?...Let the solubility of an aqueous solution of Mg(OH)2 be x then its ksp is...