Looking for trustworthy answers? Westonci.ca is the ultimate Q&A platform where experts share their knowledge on various topics. Discover in-depth solutions to your questions from a wide range of experts on our user-friendly Q&A platform. Get quick and reliable solutions to your questions from a community of experienced experts on our platform.
Sagot :
To determine the acid dissociation constant ([tex]\( K_a \)[/tex]) for the dissociation of hydrocyanic acid ([tex]\( HCN \)[/tex]) in an aqueous solution, we start by considering the dissociation reaction:
[tex]\[ HCN_{(aq)} \rightarrow H^+_{(aq)} + CN^-_{(aq)} \][/tex]
The acid dissociation constant ([tex]\( K_a \)[/tex]) is expressed as the ratio of the concentration of the products to the concentration of the reactant:
[tex]\[ K_a = \frac{ [H^+] [CN^-] }{ [HCN] } \][/tex]
Now we can match this expression with the given options:
A. [tex]\( K_2 = \frac{ \left[ H^+ \|\| C N^- \right] }{ [HCN] } \)[/tex]
- This option closely resembles the correct form of the acid dissociation constant but has extra characters making it incorrect.
B. [tex]\( K_2 = \frac{ [HCN] }{ H^+|C| \Gamma \mid } \)[/tex]
- This option incorrectly places the concentrations of the reactants and products in the denominator and numerator.
C. [tex]\( K_2 = [HCN][H^+ \|\| C N ] \)[/tex]
- This option incorrectly suggests the multiplication of the initial reactant and the products which would not match the definition of [tex]\( K_a \)[/tex].
D. [tex]\( K_2 = \left. | H^+ \|\| C N \right] \)[/tex]
- This option only includes the products' concentrations without considering the reactant, which is incorrect.
From these options, the one that matches the correct expression for the acid dissociation constant is:
[tex]\[ K_a = \frac{ [H^+] [CN^-] }{ [HCN] } \][/tex]
Therefore, the correct answer is:
A. [tex]\( K_2=\frac{\left[ \ H^+ \|\| C N^- \right]}{[ HCN ]} \)[/tex]
(Note: In a more appropriate option formatting, without any extra characters, the correct option would solely match the correct ratio provided.)
[tex]\[ HCN_{(aq)} \rightarrow H^+_{(aq)} + CN^-_{(aq)} \][/tex]
The acid dissociation constant ([tex]\( K_a \)[/tex]) is expressed as the ratio of the concentration of the products to the concentration of the reactant:
[tex]\[ K_a = \frac{ [H^+] [CN^-] }{ [HCN] } \][/tex]
Now we can match this expression with the given options:
A. [tex]\( K_2 = \frac{ \left[ H^+ \|\| C N^- \right] }{ [HCN] } \)[/tex]
- This option closely resembles the correct form of the acid dissociation constant but has extra characters making it incorrect.
B. [tex]\( K_2 = \frac{ [HCN] }{ H^+|C| \Gamma \mid } \)[/tex]
- This option incorrectly places the concentrations of the reactants and products in the denominator and numerator.
C. [tex]\( K_2 = [HCN][H^+ \|\| C N ] \)[/tex]
- This option incorrectly suggests the multiplication of the initial reactant and the products which would not match the definition of [tex]\( K_a \)[/tex].
D. [tex]\( K_2 = \left. | H^+ \|\| C N \right] \)[/tex]
- This option only includes the products' concentrations without considering the reactant, which is incorrect.
From these options, the one that matches the correct expression for the acid dissociation constant is:
[tex]\[ K_a = \frac{ [H^+] [CN^-] }{ [HCN] } \][/tex]
Therefore, the correct answer is:
A. [tex]\( K_2=\frac{\left[ \ H^+ \|\| C N^- \right]}{[ HCN ]} \)[/tex]
(Note: In a more appropriate option formatting, without any extra characters, the correct option would solely match the correct ratio provided.)
Thank you for visiting our platform. We hope you found the answers you were looking for. Come back anytime you need more information. We appreciate your visit. Our platform is always here to offer accurate and reliable answers. Return anytime. Westonci.ca is your trusted source for answers. Visit us again to find more information on diverse topics.