The equilibrium constant of reaction, usually denoted as K, is a unit of ratio. The ratio involves concentrations of products to reactants. But you also have to incorporate their stoichiometric coefficients in the reaction as their respective exponents. Note that substances in their aqueous state are the ones that are included only in the expression. To properly show you how it's done, consider this equilibrium reaction:
aA (aq) + bB (l) ⇆ nN (aq)
Since only reactant A and product N are aqueous, the equilibrium constant for this reaction is:
K = [N]ⁿ/[A]ᵃ
where the [] brackets denotes concentration in molarity
Now, let's apply this to the given equation:
Cr₂O²⁻ (aq) + 6 I⁻ (aq) + 14 H⁺ (aq) → 3 I₂ (s) + 2 Cr³⁺ (aq) + 7 H₂O<span> (l)
</span>I think there is a typographical error because Cr₂O²⁻ has a negative 2 charge rather than -27. Remember that only substances in aqueous states are included in the K expression. Therefore, the expression for K is:
K = [Cr³⁺]² / [Cr₂O²⁻][I⁻]⁶[H⁺]¹⁴
I think i wrote it already
it didn't help ?
Answer: the pH of the solution is 4.52
Explanation:
Consider the weak acid as Ha, it is dissociated as expressed below
HA H⁺ + A⁻
the Henderson -Haselbach equation can be expressed as;
pH = pKa + log( [A⁻] / [HA])
the weak acid is dissociated into H⁺ and A⁻ ions in the solution.
now the conjugate base of the weak acid HA is
HA(aq) {weak acid} H⁺(aq) + A⁻(aq) {conjugate base}
so now we calculate the value of Kₐ as well as pH value by substituting the values of the concentrations into the equation;
pKₐ = -logKₐ
pKₐ = -log ( 7.4×10⁻⁵ )
pKₐ = 4.13
now thw pH is
pH = pKₐ + log( [A⁻] / [HA])
pH = 4.13 + log( [0.540] / [0.220])
pH = 4.13 + 0.3899
pH = 4.5199 = 4.52
Therefore the pH of the solution is 4.52
Answer:
1.829 meters is the answer
Explanation:
Question:
Each liter of air has a mass of 1.80 grams. How many liters of air are contained in 2.5 x103) kg of air?
Answer:
11.48106 L
