Home
Class 12
CHEMISTRY
Calculate pH of (a) 10^(-1)MCH(3)COOH (b...

Calculate `pH` of (a)` 10^(-1)MCH_(3)COOH (b) 10^(-3)CH_(3)COOH (C )10^(-6)M cH_(3)COOH` Take `K_(a)=2xx10^(-5)` at `25^(@)C`.

Text Solution

AI Generated Solution

To calculate the pH of the given acetic acid solutions, we will follow a systematic approach using the dissociation constant \( K_a \) and the concentration of acetic acid. The formula for the dissociation of acetic acid is: \[ CH_3COOH \rightleftharpoons H^+ + CH_3COO^- \] ### Given: - \( K_a = 2 \times 10^{-5} \) ...
Promotional Banner

Topper's Solved these Questions

  • IONIC EQUILIBRIUM

    RESONANCE ENGLISH|Exercise Solved Example Miscellaneous solved problems|13 Videos

  • IONIC EQUILIBRIUM

    RESONANCE ENGLISH|Exercise Board Level Exercise|27 Videos

  • HYDROCARBON

    RESONANCE ENGLISH|Exercise ORGANIC CHEMISTRY(Hydrocarbon)|50 Videos

  • IUPAC NOMENCLATURE & STRUCTURAL ISOMERISM

    RESONANCE ENGLISH|Exercise Advanced Level Problems Part-5|2 Videos

Similar Questions

Explore conceptually related problems

Calculate pH of the solution which is 10^(-1)M in HCl & 10^(-3)M in CH_(3)COOH[K_(a)=2xx10^(-5)] .Also calculate [H^(+)] form CH_(3)COOH .

Calculate the pH of a solution containing 0.1 M CH_(3)COOH and 0.15 M CH_(3)COO^(-) . (K_(a) "of" CH_(3)COOH=1.8xx10^(-5))

Calculate pH of 10^(-6) M acetic acid solution , if K_(a) (CH_(3)COOH) = 1.80xx10^(-5) .

Calculate the percentage hydrolysis & the pH of 0.02M CH_(3)COONH_4 . K_(b)(NH_(3))-1.6xx10^(-5),K_(a)(CH_(3)COOH)=1.6xx10^(-5)

The correct order of K_(a) is : (i) CH_(3)-CH_(2)-COOH (ii) OHC-CH_(2)-COOH (iii) Ph-CH_(2)-COOH

Calculate pH of the mixture ( 50 mL of 0.05 M NH_(4)OH + 50 mL of 0.05 M CH_(3)COOH ) Given that K_(a) = 1.8 xx 10^(-5) , and K_(b) = 1.8 xx10^(-5)

Calculate the pH of a given mixtures. (a) (4g CH_(3)COOH+6g CH_(3)COONa) in 100 mL of mixture, ( K_(a) for CH_(3)COOH=1.8xx10^(-5)) (b) 5 mL of 0.1M MOH+250 mL of 0.1 M MCI , ( K_(b) for MOH=1.8xx10^(-5)) (c ) ( 0.25 mole of CH_(3)COOH+0.35 mole of CH_(3COOH=3.6xx10^(-4))

What is the concentration of CH_(3)COOH(aq.) in a solution prepared by dissolving 0.01 mole of NH_(4)^(+)CH_(3)COO^(-) in 1 L H_(2)O ? [K_(a) (CH_(3)COOH))=1.8xx10^(-5)),K_(b) (NH_(4)OH)=1.8xx10^(-5))]

Calculate pH of 0.05 M Acetic acid solution , if K_(a)(CH_(3)COOH) = 1.74 xx 10^(-5) .

Find the Van't Hoff factor of a. CH_(3)COOH in H_(2)O , b. CH_(3)COOH in benzene