0.116 M NaOH 50.0 mL + 0.0750 M HCl 적정. b) 50 mL

0.116 M NaOH 50.0 mL + 0.0750 M HCl 적정. b) 50 mL

 

 

Consider the titration of 50.0 mL of 0.116 M NaOH with 0.0750 M HCl.

Calculate the pH after the addition of each of the following volumes of acid:

a) 5.0 mL b) 50 mL c) 0.10 L

 

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▶ 참고: 강산-강염기 적정 [ https://ywpop.tistory.com/2732 ]

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0.116 M NaOH 50.0 mL에 들어있는 NaOH의 몰수

= (0.116 mol/L) (50.0/1000 L) = 0.00580 mol NaOH

( 참고 https://ywpop.tistory.com/7787 )

 

 

 

0.0750 M HCl 50 mL에 들어있는 HCl의 몰수

= (0.0750 mol/L) (50/1000 L) = 0.00375 mol HCl

 

 

 

HCl + NaOH → NaCl + H2O

HCl : NaOH = 1 : 1 반응.

 

 

 

중화 반응 후 남아있는 NaOH의 몰수

= 0.00580 – 0.00375 = 0.00205 mol NaOH

 

 

 

[NaOH] = 0.00205 mol / [(50.0+50)/1000 L]

= 0.0205 M = [OH^-]

 

 

 

pH = 14.00 – pOH

( 참고 https://ywpop.tistory.com/2706 )

 

= 14.00 - (-log(0.0205))

= 12.31

 

 

 

 

[키워드] 강산-강염기 적정 기준문서, HCl + NaOH 적정 기준문서