Question

Calculate the pH of each of the following strong acid solutions (Remember in dilution M1V1 =...

Calculate the pH of each of the following strong acid solutions (Remember in dilution M1V1 = M2V2 for part (b)). (a)0.0526 M HNO3

(b)6.00 mL of 1.00 M HCl diluted to 0.650 L

(c) (This is a tricky one that brings the students to my office, Ha Ha)A mixture formed by adding 30.0 mL of 0.018 M HCl to 30.0 mL of 0.015 M HI

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Answer #1

(a)0.0526 M HNO3

HNO3------->H+ + NO3-

[HNO3]=[H+]=0.0526

pH=-log[H+]=-log(0.0526)=1.279

(b)6.00 mL of 1.00 M HCl diluted to 0.650 L

[HCl]=[H+]=9.23*10-3

pH=-log[H+]=-log(9.23*10-3)=2.03

c)A mixture formed by adding 30.0 mL of 0.018 M HCl to 30.0 mL of 0.015 M HI

net mole of H+=mole of HCl+mole of HI=M1V1+M2V2=(30*10-3*0.018)+(30*10-3*0.015)=9.9*10-4 mole

volume of solution=V1+V2=60*10-3 L

[H+]=net mole/net volume=9.9*10-4/60*10-3=0.0165 M

pH=-log[H+]=-log(0.0165)=1.7825

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