Answer :
The fraction at pH 10.00 = 0.850
How do you determine the pH ratio?
When the moles of base added equal half the total moles of acid, the weak acid and its conjugate base are in equal amounts. The CB/WA ratio is one, and pH = pKa + log(1) or pH = pKa according to the HH equation.
How do you calculate the fraction of dissociation?
The fraction of dissociation, can be calculated directly as x / F. At this concentration, the acid is dissociated 99.9% of the time! Calculate the pH of a 0.0500 M solution for a weak acid HA with pKa = 2.328.
According to the given information:
pH 10.00
the formula for [tex]\frac{\left[\mathrm{NH}_3\right]}{\left[\mathrm{NH}_3\right]+\left[\mathrm{NH}_4^{\dagger}\right]}[/tex] and the value for Ka solve for the[H₃O⁺]
first :
pH = -log[H₃O⁺]
[H₃O⁺] = 10^-pH
[H₃O⁺] = 1 x 10^-10
solve for the[tex]\frac{\left[\mathrm{NH}_3\right]}{\left[\mathrm{NH}_3\right]+\left[\mathrm{NH}_4^{\dagger}\right]}[/tex]
[tex]\frac{\left[\mathrm{NH}_3\right]}{\left.\mathrm{NH}_4^{+}\right]+\left[\mathrm{NH}_3\right]}=\frac{K_a}{\left[\mathrm{H}_3 \mathrm{O}^{+}\right]+K_a}[/tex]
[tex]=\frac{5.68 \times 10^{-10}}{1 \times 10^{-10}+5.68 \times 10^{-10}}[/tex]
= 0.850
the fraction at pH 10.00 = 0.850
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