The ionisation constant of NH4+in water is 5.6×10−10 at 25∘C. The rate constant for the reaction of NH4+and OH−to form NH3 and H2O at 25∘C is 3.4×1010 L mol−1 s−1. Calculate the rate constant for proton transfer from water to NH3.

Name: Video solution 1: The ionisation constant of NH4+in water is 5.6×10−10 at 25∘C. The rate constant for the reaction of NH4+and OH−to form NH3 and H2O at 25∘C is 3.4×1010 L mol−1 s−1. Calculate the rate constant for proton transfer from water to NH3.
Uploaded: 2022-12-07T08:16:05.000Z
Duration: 4 min
Description: Video solution 1: The ionisation constant of NH4+in water is 5.6×10−10 at 25∘C. The rate constant for the reaction of NH4+and OH−to form NH3 and H2O at 25∘C is 3.4×1010 L mol−1 s−1. Calculate the rate constant for proton transfer from water to NH3.

NH3+H2Okb⇌kfNH4++OH−;Kb=3.4×1010NH4++H2O⇌NH4OH+H+;Ka=5.6×10−10KBase =kbKf=KAcid Kw…(i)KAcid ×KBase =Kw3.4×1010kf=5.6×10−1010−14 Kf=6.07×105

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Ionisation of acids and bases

The ionisation constant of {NH}_{4}^{+}in water is 5.6 10^{-1

Question

Hard

Solving time: 5 mins

The ionisation constant of $NH_{4}^{+}$ in water is $5.6 \times 1 0^{- 10}$ at $2 5^{\circ} C$ . The rate constant for the reaction of $NH_{4}^{+}$ and $OH^{-}$ to form $NH_{3}$ and $H_{2} O$ at $2 5^{\circ} C$ is $3.4 \times 1 0^{10} L mol^{- 1} s^{- 1}$ . Calculate the rate constant for proton transfer from water to $NH_{3}$ .

6.75 \times 1 0^{5}

4.47 \times 1 0^{5}

5.07 \times 1 0^{5}

6.07 \times 1 0^{5}

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Updated on: Dec 7, 2022

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Noah Discussed

The ionisation constant of

NH_{4}^{+}

in water is

5.6 \times 1 0^{- 10}

2 5^{\circ} C

. The rate constant for the reaction of

NH_{4}^{+}

and

OH^{-}

to form

NH_{3}

and

H_{2} O

2 5^{\circ} C

3.4 \times 1 0^{10} L mol^{- 1} s^{- 1}

. Calculate the rate constant for proton transfer from water to

NH_{3}

15 mins ago

Discuss this question LIVE

15 mins ago

Text solutionVerified

N H_{3} + H_{2} O k_{b} ⇌ k_{f} N H_{4}^{+} + O H^{-}; K_{b} = 3.4 \times 1 0^{10}

NH_{4}^{+} + H_{2} O ⇌ NH_{4} OH + H^{+}; K_{a} = 5.6 \times 1 0^{- 10}

K_{Base} = \frac{K _{f}}{k _{b}} = \frac{K _{w}}{K _{Acid}} \dots (i)

K_{Acid} \times K_{Base} = K_{w} \frac{k _{f}}{3.4 \times 1 0 ^{10}} = \frac{1 0 ^{- 14}}{5.6 \times 1 0 ^{- 10}}

K_{f} = 6.07 \times 1 0^{5}

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Question Text	The ionisation constant of $NH_{4}^{+}$ in water is $5.6 \times 1 0^{- 10}$ at $2 5^{\circ} C$ . The rate constant for the reaction of $NH_{4}^{+}$ and $OH^{-}$ to form $NH_{3}$ and $H_{2} O$ at $2 5^{\circ} C$ is $3.4 \times 1 0^{10} L mol^{- 1} s^{- 1}$ . Calculate the rate constant for proton transfer from water to $NH_{3}$ .
Updated On	Dec 7, 2022
Topic	Equilibrium
Subject	Chemistry
Class	Class 11
Answer Type	Text solution:1 Video solution: 1
Upvotes	114
Avg. Video Duration	4 min

Text solutionVerified

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The ionisation constant of NH4+​in water is 5.6×10−10 at 25∘C. The rate constant for the reaction of NH4+​and OH−to form NH3​ and H2​O at 25∘C is 3.4×1010 L mol−1 s−1. Calculate the rate constant for proton transfer from water to NH3​.

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