Advertisements
Advertisements
प्रश्न
\[\ce{K_a}\] for \[\ce{CH3COOH}\] is 1.8 × 10–5 and \[\ce{K_b}\] for \[\ce{NH4OH}\] is 1.8 × 10–5 . The \[\ce{pH}\] of ammonium acetate will be ______.
पर्याय
7.005
4.75
7.0
Between 6 and 7
उत्तर
\[\ce{K_a}\] for \[\ce{CH3COOH}\] is 1.8 × 10–5 and \[\ce{K_b}\] for \[\ce{NH4OH}\] is 1.8 × 10–5 . The \[\ce{pH}\] of ammonium acetate will be 7.0.
Explanation:
The equation for weak acid and weak base is given as
\[\ce{pH = 7 + 21 (pK_a − pK_b)}\]
\[\ce{K_a}\] = 1.8 × 10–5
\[\ce{pK_a = - log (1.8 × 10^{-5})}\] = 5 − log1.8 = 4.744
\[\ce{pK_b = −log (1.8 × 10^{-5)}}\] = 4.744
\[\ce{pH = 7 + 21 (pK_a − pK_b)}\] = 7.
APPEARS IN
संबंधित प्रश्न
Calculate the degree of ionization of 0.05M acetic acid if its pKa value is 4.74.
How is the degree of dissociation affected when its solution also contains
- 0.01 M
- 0.1 M in HCl?
The ionization constant of dimethylamine is 5.4 × 10–4. Calculate its degree of ionization in its 0.02 M solution. What percentage of dimethylamine is ionized if the solution is also 0.1 M in NaOH?
Calculate the hydrogen ion concentration in the following biological fluids whose pH are given below:
Human muscle-fluid, 6.83
Calculate the hydrogen ion concentration in the following biological fluids whose pH are given below:
Human stomach fluid, 1.2
Calculate the hydrogen ion concentration in the following biological fluids whose pH are given below:
Human blood, 7.38
Calculate the hydrogen ion concentration in the following biological fluids whose pH are given below:
Human saliva, 6.4.
A 0.02 M solution of pyridinium hydrochloride has pH = 3.44. Calculate the ionization constant of pyridine.
\[\ce{pH}\] of 0.08 mol dm–3 \[\ce{HOCl}\] solution is 2.85. Calculate its ionisation constant
Assertion (A): Aqueous solution of ammonium carbonate is basic.
Reason (R): Acidic/basic nature of a salt solution of a salt of weak acid and weak base depends on Ka and Kb value of the acid and the base forming it.
Its solution in water will be basic.
