4.2 HCN will react very slightly with water with a K = 6.2 x 10-10. %3D HCN(aq) + H,O() = H;O* (aq) and CN (aq) A chemist starts with a 0.50 M HCN solution. What is the equilibrium concentration of H,0*?. Then use the concentration of H,O* to calculate the pH of the solution with the equation pH = -log[H3O*] (you can do this!!!). Put your final answers in the box. If you need more space to show your work, you can use the backside of this page. [H,O'] at equilibrium M pH = -log(H,O'] pH = % of HCN that reacted
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Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
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![Explain why we can simplify the calculations for K when the value of K is very small (less
4.1
than -10*).
4.2
HCN will react very slightly with water with a K = 6.2 x 10-10.
HCN(aq) + H,O()
H,O* (aq) and CN" (aq)
A chemist starts with a 0.50 M HCN solution. What is the equilibrium concentration of
H;O*?. Then use the concentration of H3O* to calculate the pH of the solution with the equation
pH = -log[H3O*] (you can do this!!!). Put your final answers in the box. If you need more space
to show your work, you can use the backside of this
page.
[H;O'] at equilibrium
pH = -log(H,O]
pH =
% of HCN that
reacted](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb7f5cfe5-11ef-40c1-b16d-38d32fdf07ee%2F48e93853-de3c-4778-bcff-897910ca3378%2Fsgmpei_processed.jpeg&w=3840&q=75)
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