Calculate pH in the end points and molarity of HCl and CH3COOH?

Calculate pH in the end points and molarity of HCl and CH3COOH?

2 thoughts on “Calculate pH in the end points and molarity of HCl and CH3COOH?”

    • pH of a solution depends upon the hydrogen ion concentration.
    • pH of a solution depends upon the hydrogen ion concentration.HCl is a strong acid and it will be almost completely (100%) ionised even at appreciable concentration.
    • pH of a solution depends upon the hydrogen ion concentration.HCl is a strong acid and it will be almost completely (100%) ionised even at appreciable concentration.But CH3-COOH being a weak acid will be weakly ionised at even dilute concentration. Acetic acid will be nearly 3- 5% dissociated at 0.1 M concentration.
    • pH of a solution depends upon the hydrogen ion concentration.HCl is a strong acid and it will be almost completely (100%) ionised even at appreciable concentration.But CH3-COOH being a weak acid will be weakly ionised at even dilute concentration. Acetic acid will be nearly 3- 5% dissociated at 0.1 M concentration.Let us consider HCl and CH3-COOH solutions of 0.1M concentration.
    • pH of a solution depends upon the hydrogen ion concentration.HCl is a strong acid and it will be almost completely (100%) ionised even at appreciable concentration.But CH3-COOH being a weak acid will be weakly ionised at even dilute concentration. Acetic acid will be nearly 3- 5% dissociated at 0.1 M concentration.Let us consider HCl and CH3-COOH solutions of 0.1M concentration.pH of 0.1M HCl=- log(0.1)=1
    • pH of a solution depends upon the hydrogen ion concentration.HCl is a strong acid and it will be almost completely (100%) ionised even at appreciable concentration.But CH3-COOH being a weak acid will be weakly ionised at even dilute concentration. Acetic acid will be nearly 3- 5% dissociated at 0.1 M concentration.Let us consider HCl and CH3-COOH solutions of 0.1M concentration.pH of 0.1M HCl=- log(0.1)=1The [H+] ion concentration of 0.1 M CH3-COOH
    • pH of a solution depends upon the hydrogen ion concentration.HCl is a strong acid and it will be almost completely (100%) ionised even at appreciable concentration.But CH3-COOH being a weak acid will be weakly ionised at even dilute concentration. Acetic acid will be nearly 3- 5% dissociated at 0.1 M concentration.Let us consider HCl and CH3-COOH solutions of 0.1M concentration.pH of 0.1M HCl=- log(0.1)=1The [H+] ion concentration of 0.1 M CH3-COOH= √(Ka xC)=√(1.8×10^-5x 0.1)
    • pH of a solution depends upon the hydrogen ion concentration.HCl is a strong acid and it will be almost completely (100%) ionised even at appreciable concentration.But CH3-COOH being a weak acid will be weakly ionised at even dilute concentration. Acetic acid will be nearly 3- 5% dissociated at 0.1 M concentration.Let us consider HCl and CH3-COOH solutions of 0.1M concentration.pH of 0.1M HCl=- log(0.1)=1The [H+] ion concentration of 0.1 M CH3-COOH= √(Ka xC)=√(1.8×10^-5x 0.1)=1.342 x 10^-3
    • pH of a solution depends upon the hydrogen ion concentration.HCl is a strong acid and it will be almost completely (100%) ionised even at appreciable concentration.But CH3-COOH being a weak acid will be weakly ionised at even dilute concentration. Acetic acid will be nearly 3- 5% dissociated at 0.1 M concentration.Let us consider HCl and CH3-COOH solutions of 0.1M concentration.pH of 0.1M HCl=- log(0.1)=1The [H+] ion concentration of 0.1 M CH3-COOH= √(Ka xC)=√(1.8×10^-5x 0.1)=1.342 x 10^-3pH of 0.1 M CH3-COOH =2.8277
    • pH of a solution depends upon the hydrogen ion concentration.HCl is a strong acid and it will be almost completely (100%) ionised even at appreciable concentration.But CH3-COOH being a weak acid will be weakly ionised at even dilute concentration. Acetic acid will be nearly 3- 5% dissociated at 0.1 M concentration.Let us consider HCl and CH3-COOH solutions of 0.1M concentration.pH of 0.1M HCl=- log(0.1)=1The [H+] ion concentration of 0.1 M CH3-COOH= √(Ka xC)=√(1.8×10^-5x 0.1)=1.342 x 10^-3pH of 0.1 M CH3-COOH =2.8277So with equal concentration, the weaker acid will have a higher pH than the strong acid.
    • pH of a solution depends upon the hydrogen ion concentration.HCl is a strong acid and it will be almost completely (100%) ionised even at appreciable concentration.But CH3-COOH being a weak acid will be weakly ionised at even dilute concentration. Acetic acid will be nearly 3- 5% dissociated at 0.1 M concentration.Let us consider HCl and CH3-COOH solutions of 0.1M concentration.pH of 0.1M HCl=- log(0.1)=1The [H+] ion concentration of 0.1 M CH3-COOH= √(Ka xC)=√(1.8×10^-5x 0.1)=1.342 x 10^-3pH of 0.1 M CH3-COOH =2.8277So with equal concentration, the weaker acid will have a higher pH than the strong acid.0.1 M HCl will be 0.1/(1.342 x 10^-3)= 74.5 times more dissociated than 0.1M CH3-COOH.

Leave a Comment