Ferrous sulfate (FeSO4) is obtained by the reaction of aqueous ferric sulfate with gaseous sulfur dioxide and water according to the equation below:
Aqueous ferric sulfate =
Gaseous sulfur dioxide =
Water =
Aqueous sulfuric acid =
Aqueous ferrous sulfate =
Thus, the balance equation becomes:
+
+
More on ferrous sulfate can be found here: brainly.com/question/10834028
Answer:
Explanation:
Hello.
In this case, for this equilibrium problem, we first realize that at the beginning there is just HI, it means that the reaction should be rewritten as follows:
Whereas the law of mass action (equilibrium expression) is:
That in terms of initial concentrations and reaction extent or change turns out:
And the solution via solver or quadratic equation is:
Whereas the correct answer is 0.183 M since the other value yield a negative concentration of HI at equilibrium (0.391-2*0.210=-0.029M).This, the equilibrium concentrations are:
Regards.
pH of 0.048 M HClO is 4.35.
<u>Explanation:</u>
HClO is a weak acid and it is dissociated as,
HClO ⇄ H⁺ + ClO⁻
We can write the equilibrium expression as,
Ka =
Ka = 4.0 × 10⁻⁸ M
4.0 × 10⁻⁸ M =
Now we can find x by rewriting the equation as,
x² = 4.0 × 10⁻⁸ × 0.048
= 1.92 × 10⁻⁹
Taking sqrt on both sides, we will get,
x = [H⁺] = 4.38 × 10⁻⁵
pH = -log₁₀[H⁺]
= - log₁₀[ 4.38 × 10⁻⁵]
= 4.35