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

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

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Luna 4 months 2021-08-01T11:12:10+00:00 2 Answers 0 views 0

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    0
    2021-08-01T11:13:29+00:00

    CH3COOH has a pH of 2.64

    Molarity of Hydrochloric Acid (HCl) = 12.1

    0
    2021-08-01T11:13:56+00:00
    • 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.

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