pH of 0.0037 M H2CO3 solution

pH of 0.0037 M H2CO3 solution

H2CO3 용액의 pH. 탄산 용액의 pH

 

 

Find the pH of a 0.0037 M solution of H2CO3.

This acid has two protons that can be dissociated, and two Ka values.

 

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Ka1 = 4.3×10^(-7)

Ka2 = 5.6×10^(-11)

 

 

[계산공식]

 

[H2CO3] = H2CO3의 초기농도(C)

[HCO3^-] = [Ka1 × C]^(1/2)

[CO3^2-] = Ka2

[H^+] = [Ka1 × C]^(1/2)

( 식 설명 https://ywpop.tistory.com/12727 )

 

 

[H^+] = [Ka1 × C]^(1/2)

= [(4.3×10^(-7)) × 0.0037]^(1/2)

= 3.9887×10^(-5) M

 

 

pH = -log(3.9887×10^(-5))

= 4.3992

 

 

답: pH = 4.4