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Chapter 4: 4.59P (page 180)

Is the following a redox reaction? Explain

NH3(aq)+HCl(aq)→NH4Cl(aq)

Short Answer

Expert verified

No, this is not a redox reaction.

Step by step solution

01

Definition of redox reaction

Oxidation-reduction (or redox) reactions are a type of chemical reaction in which the net movement of electrons from one reactant to the other occurs.

Such movement of electron charge occurs in the formation of both ionic and covalent compounds.

Or we can say that a reaction in which one compound oxidizes and the other is reduced simultaneously in the same reaction and elements change their oxidation state in a chemical reaction are known as redox reactions.

Example: 2Mgs+O2g→2MgOs

02

Determine the types of reaction when ammonia reacts with hydrochloric acid

NH3aq+HClaq→NH4Claq

No, this is not a redox reaction because in the redox reaction two or more elements must change their oxidation states.

In the above reaction there is no change in oxidation state of the elements. Consequently there is no net movement of electrons in the above reaction.

This is a neutralization reaction between an acid and a base.

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Most popular questions from this chapter

Predict the product(s) and write a balanced equation for each of the following redox reactions:

(a)Fe(s)+HClO4(aq)→

(b)S8(s)+O2(g)→

(c)BaCl2(l)→electricity

Que Complete the following acid-base reactions with balanced molecular, total ionic, and net ionic equations:

(a) Potassium hydroxide(aq) + hydrobromic acid(aq)

(b) Ammonia(aq) + hydrochloric acid(aq)

In a titration of HNO3, you add a few drops of phenolphthalein indicator to 50.00 mL of acid in a flask. You quickly add 20.00 mL of 0.0502 MNaOH but overshoot the end point, and the solution turns deep pink. Instead of starting over, you add 30.00 mL of the acid, and the solution turns colorless. Then, it takes 3.22 mL of the NaOH to reach the end point. (a) What is the concentration of the HNO3solution? (b) How many moles of NaOH were in excess after the first addition?

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