7) Calculate the K a of a 0.53 M solution of H X that has a p H of 1.6. Answer to three significant figures. When solving this problem do not assume the 5% rule is valid (even if it is) or else you may be marked wrong.

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7)

Calculate the K a of a 0.53 M solution of H X that has a p H of 1.6. Answer to three significant figures.

When solving this problem do not assume the 5% rule is valid (even if it is) or else you may be marked wrong.

Expert Solution
Step 1

Ka is the dissociation constant of an acid. The dissociation equilibrium for the given acid as follows:

      HX            H+ +   X-I:  0.53                  0          0C: -x                +x        +xE: 0.53-X       +x        +x

Expression for Ka is as follows:

Ka=xx0.53-x 

where x=H+ and x=X-

 

 

 

Step 2

It is given that pH =1.6. From pH,H+ ion concentration can be calculated as follows:

pH=-log(H+)1.6=-log(H+)antilog-1.6=(H+)So, H+=0.0251 M

Thus, x=0.0251 

Substitute it in the expression for Ka

Ka=0.025120.53-0.0251      = 0.000630.5049 = 0.00124

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