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Masteriza [31]
3 years ago
8

According to the Arrhenius theory, an acid is a substance that

Chemistry
1 answer:
barxatty [35]3 years ago
4 0

Answer:

which produces hydrogen ion in water, called acid. A substance which produces hydroxide ion in water, called base. According to Bronsted-Lowry theory, an acid is proton donor and base is proton acceptor. Actually, Arrhenius theory is limited only to the aqueous solution.

Explanation:

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Lysosomes are found in all animal cells, but are most numerous in disease-fighting cells, such as white blood cells. This is because white blood cells must digest more material than most other types of cells in their quest to battle bacteria, viruses, and other foreign intruders.

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Which of the statements correctly describes the reactivity of halogens, according to the octet rule?
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They have seven electrons in their valence shell, so halogens are very reactive.
Hope this helps! :)
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Four pennies are heated to different temperatures. At which temperature
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c

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A what is the part that doesn't change during the experiment
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Consider the insoluble compound silver bromide , AgBr . The silver ion also forms a complex with ammonia . Write a balanced net
Degger [83]

Answer:

- AgBr(s)+2NH_3(aq)\rightleftharpoons Ag(NH_3)_2^+(aq)+Br^-(aq)

- K=1.2x10^{-5}

Explanation:

Hello,

In this case, by considering the dissolution of silver bromide:

AgBr(s)\rightleftharpoons Ag^+(aq)+Br^-(aq) \ \ \ Ksp=[Ag^+][Br^-]=7.7x10^{-13}

And the formation of the complex:

Ag^+(aq)+2NH_3(aq)\rightleftharpoons Ag(NH_3)_2^+(aq)\ \ \ Kf=\frac{[Ag(NH_3)_2^+]}{[Ag^+][NH_3]^2}=1.6x10^7

We obtain the balanced net ionic equation by adding the aforementioned equations:

AgBr(s)+Ag^+(aq)+2NH_3(aq)\rightleftharpoons Ag(NH_3)_2^+(aq)+Br^-(aq)+Ag^+(aq)\\\\AgBr(s)+2NH_3(aq)\rightleftharpoons Ag(NH_3)_2^+(aq)+Br^-(aq)

Now, the equilibrium constant is obtained by writing the law of mass action for the non-simplified net ionic equation:

AgBr(s)+Ag^+(aq)+2NH_3(aq)\rightleftharpoons Ag(NH_3)_2^+(aq)+Br^-+Ag^+\\\\K=[Ag^+][Br^-]*\frac{[Ag(NH_3)_2^+]}{[Ag^+][NH_3]^2}

So we notice that the equilibrium constant contains the solubility constant and formation constant for the initial reactions:

K=Ksp*Kf=7.7x10^{-13}*1.6x10^{7}\\\\K=1.2x10^{-5}

Best regards.

4 0
3 years ago
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