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8_murik_8 [283]
3 years ago
8

Write a chemical equation for nh4+(aq) showing how it is an acid or a base according to the arrhenius definition.

Chemistry
2 answers:
GuDViN [60]3 years ago
3 0

An Arrhenius acid by definition dissociates in water to form H3O+ (or H+) ions while an arrhenius base dissociates in water to form OH- ions.

NH4+(aq) can be categorised as an arrhenius acid since it releases H3O+ ions in aqueous media

NH4+(aq) + H2O (aq) ↔ NH3 (aq) + H3O+(aq)

nekit [7.7K]3 years ago
3 0

Answer:

NH₄⁺ will act as acid according to the arrhenius definition.

NH₄⁺ will not act as a base according to the arrhenius definition.

Explanation:

According to the Arrhenius Acid-Base Theory, acids are those substances that dissolved in water divide by generating H⁺ together with an anion (ion with a negative charge). In an aqueous solution, the H⁺ protons react immediately with the water molecules to form H₃O⁺ hydronium ions. A base, on the contrary, according to this theory, is a substance that releases OH- ions in aqueous solution.

This theory is valid only in aqueous medium. And it does not consider non-protic acids (without the presence of H⁺), which are unable to release hydrogen ions, or dehydroxylated bases (they are OH- ions in their structure), unable to release OH- hydroxyl ions.

NH₄⁺ will act as acid because it has an H⁺ proton that can be released into the aqueous solution by:

NH₄⁺(aq) + H₂O (aq) ↔ NH₃ (aq) + H₃O⁺(aq)

NH₄⁺ will not act as a base because it does not have hydroxide ions that can be released into the aqueous medium.

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What is the ph of a 0.25 m solution of c6h5nh2 given that its kb is 1.8 x 10-6?
IrinaK [193]

The pH a 0.25 m solution of C₆H₅NH₂ is equal to 3.13.

<h3>How do we calculate pH of weak base?</h3>

pH of the weak base will be calculate by using the Henderson Hasselbalch equation as:

pH = pKb + log([HB⁺]/[B])

pKb = -log(1.8×10⁻⁶) = 5.7

Chemical reaction for C₆H₅NH₂ is:

                          C₆H₅NH₂ + H₂O → C₆H₅NH₃⁺ + OH⁻

Initial:                     0.25                           0            0

Change:                    -x                             x             x

Equilibrium:        0.25-x                           x             x

Base dissociation constant will be calculated as:
Kb = [C₆H₅NH₃⁺][OH⁻] / [C₆H₅NH₂]

Kb = x² / 0.25 - x

x is very small as compared to 0.25, so we neglect x from that term and by putting value of Kb, then the equation becomes:

1.8×10⁻⁶ = x² / 0.25

x² = (1.8×10⁻⁶)(0.25)

x = 0.67×10⁻³ M = [C₆H₅NH₃⁺]

On putting all these values on the above equation of pH, we get

pH = 5.7 + log(0.67×10⁻³/0.25)

pH = 3.13

Hence pH of the solution is 3.13.

To know more about Henderson Hasselbalch equation, visit the below link:
brainly.com/question/13651361

#SPJ4

5 0
2 years ago
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