0.05 M Na2CO3​ 50 mL + 0.1 M HCl 40 mL

0.05 M Na2CO3​ 50 mL + 0.1 M HCl 40 mL

 

 

50 mL of 0.05 M Na2CO3​ is titrated against 0.1 M HCl.

On adding 40 mL of HCl, pH of the solution will be

 

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> (0.05 mol/L) (0.050 L) = 0.0025 mol Na2CO3

> (0.1 mol/L) (0.040 L) = 0.004 mol HCl

 

 

 

CO3^2- + H^+ → HCO3^-

[반응 전] 0.0025 : 0.004 : 0

[반응 후] 0 : 0.0015 : 0.0025

 

 

 

HCO3^- + H^+ → H2CO3

[반응 전] 0.0025 : 0.0015 : 0

[반응 후] 0.001 : 0 : 0.0015

 

 

 

Henderson-Hasselbalch 식

pH = pKa + log([짝염기]/[약산])

( 참고 https://ywpop.tistory.com/1926 )

 

= pKa1 + log([HCO3^-]/[H2CO3])

= 6.35 + log(0.001/0.0015) = 6.1739

 

 

 

답: pH = 6.17

 

 

 

 

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[ 관련 예제 https://ywpop.tistory.com/16805 ] 0.1 M Na2CO3 50 mL + 0.1 M HCl 10 mL

 

 

 

[키워드] Na2CO3​ + HCl 적정 기준문서, Na2CO3​-HCl 적정 기준문서, Na2CO3​ HCl 적정 기준문서, 2가 약산염​ + HCl 적정 기준문서, 2가 약산염​-HCl 적정 기준문서, 2가 약산염​ HCl 적정 기준문서