Based on the calculations, the [tex]H^+[/tex] is equal to [tex]7.9 \times 10^{-3}\;M[/tex]
Given the following data:
- Dissociation constant = [tex]1.8 \times 10^{-4}\;M[/tex].
- Dissociation ratio = 1:1.
- Volume of water = 1.0 liter.
- Number of moles of formic acid = 0.35.
How to determine the [tex]H^+[/tex].
First of all, we would write the properly balanced chemical equation for the dissociation of this weak acid:
[tex]HCOOH\; \rightleftharpoons \;HCOO^- +H^+[/tex]
Initial cond. c 0 0
At equib. [tex]c(1-\alpha )[/tex] c c
Mathematically, the dissociation constant is given by this formula:
[tex]k=\frac{ c^2\alpha^2 }{c} =c\alpha^2[/tex]
For the concentration:
[tex]c=\frac{No. \;of\;moles}{Volume} \\\\c=\frac{0.35}{1}[/tex]
c = 0.35 M.
Substituting the parameters into the formula, we have;
[tex]1.8 \times 10^{-4}=0.35\alpha ^2\\\\\alpha ^2=\frac{1.8 \times 10^{-4}}{0.35} \\\\\alpha =\sqrt{5.143 \times 10^{-4}} \\\\\alpha =2.27 \times 10^{-2}[/tex]
For the [tex]H^+[/tex]:
[tex]H^+=c\alpha \\\\H^+ =0.35 \times 2.27 \times 10^{-2}\\\\H^+ =7.9 \times 10^{-3}\;M[/tex]
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