Question

Hypochlorous acid, $HOCl$, reacts with water as shown below: What is the $pH$ of a $0.033{\text{ }}M$ aqueous solution of acetic acid? ${K_a} = 1.1e - 2$

Answer 1

This is a feeble acid at Low fixation, whose separation we most likely need to settle logically. $HOCl$ is delegated Non-Hazardous by the Environmental Protection Agency in the US. As any oxidizing specialist it very well may be destructive or aggravation relying upon its fixation and $pH$.

Complete step by step answer:
Hypochlorous acid ($HOCl$ or $HClO$) is a weak acid whose IUPAC name is hypochlorous acid, chloric acid, hydroxide chlorine. $HClO$ and $Cl{O^ - }$ are oxidizing agents, and the essential sanitization experts of chlorine solutions. $HOCl$ can't be confined from these arrangements because of fast equilibration with its antecedent. Sodium hypochlorite ($NaClO$) and calcium hypochlorite ($Ca{\left( {ClO} \right)_2}$), are blanches, antiperspirants, and disinfectants.
Hypochlorous acid ($HOCl$) is created chiefly in leukocytes, including neutrophils, macrophages, and monocytes, by myeloperoxidase ($MPO$)- catalyzed peroxidation of chloride particles. It assumes an indispensable part in slaughtering a wide scope of microorganisms and bears the cost of an inborn host guard. Then again, oxidative pressure because of exorbitant age of ROS is embroiled in numerous human infections, and it is felt that neutrophil-inferred $HOCl$ adds to aggravation related tissue injury, for example, hepatic ischemia-reperfusion injury, atherosclerosis, lung injury, and rheumatoid joint inflammation.
We address the condition...
where ${K_a} = 0.011 = \dfrac{{\left[ {{H_3}{O^ + }} \right]\left[ {^ - OCl} \right]}}{{\left[ {HOCl} \right]}}$
What's more, if $x \cdot mol \cdot {L^{ - 1}}$ separates,
$0.011 = \dfrac{{{x^2}}}{{0.033 - x}}$
Thus ${x^2} = 0.011 \times \left( {0.033 - x} \right)$
What's more, thus, ${x^2} + 0.011x - 3.63 \times {10^{ - 4}} = 0$
We get $x = 0.014 \cdot mol \cdot {L^{ - 1}}$ as the positive root.
Thus at equilibrium,
$\left[ {HOCl} \right] = \left( {0.033 - 0.014} \right) \cdot mol \cdot {L^{ - 1}} = 0.019 \cdot mol \cdot {L^{ - 1}}$
$\left[ {^ - OCl} \right] = 0.014 \cdot mol \cdot {L^{ - 1}}$
$\left[ {{H_3}{O^ + }} \right] = 0.014 \cdot mol \cdot {L^{ - 1}} = 0.014 \cdot mol \cdot {L^{ - 1}}$
What's more, it is common for a weak acid at LOW focuses, to separate more than it would regularly would...
$pH = - {\log _{10}}\left( {0.014} \right) = 1.85$

Note:
In natural blend, $HClO$ changes alkenes over to chlorohydrin. In science, hypochlorous acid is produced in enacted neutrophils by myeloperoxidase-interceded peroxidation of chloride particles, and adds to the obliteration of microorganisms. In water treatment, hypochlorous acid is the dynamic.