Explanation:
Let the reaction equation for the dissociation of weak acid is as follows.
                        
 
Initial:         0.87            0         0
Change:      -x               +x         +x
Equilibrium:  0.87 - x    +x         +x
Hence, expression for the dissociation constant will be as follows.
            ![k_{a} = \frac{[H^{+}][A^{-}]}{[HA]}](https://tex.z-dn.net/?f=k_%7Ba%7D%20%3D%20%5Cfrac%7B%5BH%5E%7B%2B%7D%5D%5BA%5E%7B-%7D%5D%7D%7B%5BHA%5D%7D)
Now, putting the given values into the above formula as follows.
         ![k_{a} = \frac{[H^{+}][A^{-}]}{[HA]}](https://tex.z-dn.net/?f=k_%7Ba%7D%20%3D%20%5Cfrac%7B%5BH%5E%7B%2B%7D%5D%5BA%5E%7B-%7D%5D%7D%7B%5BHA%5D%7D)
        
                x = 0.000283
Hence, at equilibrium the concentration of hydrogen ions is 0.000283.
or,     ![[H^{+}] = 2.83 \times 10^{-4}](https://tex.z-dn.net/?f=%5BH%5E%7B%2B%7D%5D%20%3D%202.83%20%5Ctimes%2010%5E%7B-4%7D)
             ![[H^{+}] = C \times \alpha](https://tex.z-dn.net/?f=%5BH%5E%7B%2B%7D%5D%20%3D%20C%20%5Ctimes%20%5Calpha)
Also,   ![\alpha = \frac{[H^{+}]}{C}](https://tex.z-dn.net/?f=%5Calpha%20%3D%20%5Cfrac%7B%5BH%5E%7B%2B%7D%5D%7D%7BC%7D)
                       = 
                       = 0.00151 
And, the percentage of dissociation is  = 0.151%
 = 0.151%
Thus, we can conclude that percent dissociation of given weak acid is 0.151%.
 
        
             
        
        
        
Answer:
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Step-by-step explanation:
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Answer:
1km is 1000m 
so 100ratio 1000m 
1 ratio 10
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