Chemistry, 20.09.2020 01:01, tytybruce2

Classify each reactant and product in this reaction as an acid or base according to the Brønsted theory. HF + H2O = F + H30+

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HF
H30+
F-
H2O

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answered: miguelc2145

Reaction: $\rm HF + H_2O \rightleftharpoons F^{-} + H_3O^{+}$ .

$\rm HF$ : Bronsted-Lowry Acid. $\rm H_3O^{+}$ : Bronsted-Lowry conjugate Acid of $\rm F^{-}$ : Bronsted-Lowry conjugate Base of $\rm HF$ . $\rm H_2O$ : Bronsted-Lowry Base.

Explanation:

In the Bronsted-Lowry acid-base theory, the acid in a reaction is the species that loses a proton, $\rm H^{+}$ . The resultant species would be the conjugate base of that acid.

On the other hand, the Bronsted-Lowry base in a reaction is the species that accepts a proton $\rm H^{+}$ . The resultant species would be the conjugate acid of that base.

Identify the conjugate acid-base pairs in this reaction. Note that the two species in each pair are related by the gain or loss of a single proton. Therefore, their formula should look similar to each other.

For this reaction, $\rm HF$ and $\rm F^{-}$ , as well as $\rm H_2O$ and $\rm H_3O^{+}$ form two similar-looking reactant-product pairs:

The reactant $\rm HF$ loses one proton to form the product $\rm F^{-}$ . Therefore, $\rm HF\!$ would be the Bronsted-Lowry acid, while $\rm F^{-}\!$ would be its conjugate base.The reactant $\rm H_2O$ gains one proton to form the product $\rm H_3O^{+}$ . Therefore, $\rm H_2O\!$ would be the Bronsted-Lowry base, while $\rm H_3O^{+}\!$ would be the conjugate acid.

answered: Guest

answer: - 3.) the oxidation state of nitrogen in no changes from +2 to 0, and the oxidation state of carbon in co changes from +2 to +4 as the reaction proceeds.

solution: - as per the rules, oxidation number of oxygen in its compounds is -2. the sum of oxidation numbers of all the elements of a molecule or compound is zero.

also, the oxidation number in elemental form is zero.

in no, the oxidation number of o is -2 so the oxidation number of n is +2 so that the sum is zero.

similarly, the oxidation number of c in co is +2 and o is -2.

on product side the oxidation number of n is 0 as it is in the elemental form( $n_2$ ) .

oxidation number of c in carbon dioxide is +4 as there are two oxygen in it and we know that each oxygen is -2.

so, oxidation number of n is changing from +2 to 0 and the oxidation number of c is changing from +2 to +4.

since nitrogen is reduced and hence no is acting as an oxidizing agent. carbon is oxidized and so co is acting as a reducing agent.

so, the right choice is number 3.)the oxidation state of nitrogen in no changes from +2 to 0, and the oxidation state of carbon in co changes from +2 to +4 as the reaction proceeds.

answered: Guest

Change in speed or direction : )

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Classify each reactant and product in this reaction as an acid or base according to the Brønsted the...