Ostwald Dilution Law Mathematical Interpretation
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Q. A 20 mL solution of 0.5 M NH4OH is to be titrated with 0.2 M HCl. Find the pH of solution initially i.e. when no HCl is added.
(Kb(NH4OH)=1.8×10−5)
(Kb(NH4OH)=1.8×10−5)
- 11.48
- 2.52
- 10.48
- 3.52
Q. 9.125 g of HCl is present in 0.5 L of solution at 25∘C. The pH of the solution is :
- 0.6
- 1.44
- 0.88
- 0.3
Q. Calculate the H+ ion concentration of a 0.01 N weak monobasic acid. The value of dissociation constant is 4.0×10−10.
- 2×10−6 mole L−1
- 2×10−5 mole L−1
- 3×10−6 mole L−1
- 3×10−5 mole L−1
Q. Dilution processes of different aqueous solution, with water, are given in LIST-I. The effects of dilution of the solutions on [H+] are given in LIST -II.
(Note: Degree of dissociation (α) of weak acid and weak base is << 1; degree of hydrolysis of salt << 1; [H+] represents the concentration of H+ ions)
LIST -ILIST-IIP. 10 mL of 0.1 M NaOH +20 mL of1. The value of [H+] does not0.1 M acetic acid diluted to 60 mLchange on dilutionQ. 20 mL of 0.1 M NaOH +20 mL of2. The value of [H+] changes to half0.1 M acetic acid diluted to 80 mLof its initial value on dilutionR. 20 mL of 0.1 M HCl + 20 mL of 0.13. The value of [H+] changes to twoM ammonia solution diluted to 80 mLtimes of its initial value on dilutionS. 10 mL saturated solution of Ni(OH)24. The value of [H+] changes to 1√2in equilibrium with excess solid Ni(OH)2times of its initial value on dilutionis diluted to 20 mL (solid Ni(OH)2is stillpresent after dilution).5. The value of [H+] changes to √2times of its initial value on dilution
Match each process given in LIST -I with one or more effect(s) in LIST -II. The correct option is
(Note: Degree of dissociation (α) of weak acid and weak base is << 1; degree of hydrolysis of salt << 1; [H+] represents the concentration of H+ ions)
LIST -ILIST-IIP. 10 mL of 0.1 M NaOH +20 mL of1. The value of [H+] does not0.1 M acetic acid diluted to 60 mLchange on dilutionQ. 20 mL of 0.1 M NaOH +20 mL of2. The value of [H+] changes to half0.1 M acetic acid diluted to 80 mLof its initial value on dilutionR. 20 mL of 0.1 M HCl + 20 mL of 0.13. The value of [H+] changes to twoM ammonia solution diluted to 80 mLtimes of its initial value on dilutionS. 10 mL saturated solution of Ni(OH)24. The value of [H+] changes to 1√2in equilibrium with excess solid Ni(OH)2times of its initial value on dilutionis diluted to 20 mL (solid Ni(OH)2is stillpresent after dilution).5. The value of [H+] changes to √2times of its initial value on dilution
Match each process given in LIST -I with one or more effect(s) in LIST -II. The correct option is
- P→4;Q→2;R→3;S→1
- P→4;Q→3;R→2;S→3
- P→1;Q→4;R→5;S→3
- P→1;Q→5;R→4;S→1
Q.
At 25∘C, the dissociation constant of a base BOH is 1.0 × 10−12. The
concentration of Hydroxyl ions in 0.01 M aqueous solution of the base
would be
2.0 × 10−6molL−1
1.0 × 10−5molL−1
1.0 × 10−6molL−1
1.0 × 10−7molL−1
Q. 0.2 M solution of formic acid is ionized 3.2%, its ionization constant is
- 9.6×10−3
- 2.1×10−4
- 1.25×10−6
- 4.8×10−5