What element is undergoing oxidation (if any) in the following reaction? 2 hcl(aq) + ca(oh)2(aq) → 2 h2o(l) + 2 cacl2(aq)

None of the elements oxidized.

Explanation:

The oxidation reduction reactions are called redox reaction. These reactions are take place by gaining or losing the electrons and oxidation state of elements are changed.

Oxidation:

Oxidation involve the removal of electrons and oxidation state of atom of an element is increased.

Reduction:

Reduction involve the gain of electron and oxidation number is decreased.

Chemical equation:

2HCl + Ca(OH)₂   →   2H₂O + 2CaCl₂

with oxidation state:

2{H⁺Cl⁻} + [Ca⁺²{(O⁻²)H⁺)}₂]   →   [2{(H⁺)₂O⁻²}] + [2{(Ca²⁺)(Cl⁻)₂}]

None of the elements oxidized. The oxidation sates of all elements are same in reactants and products.

i believe the answer is true.

the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. completely dissociates to and ions. a is incorrect because does not fully ionize to and ions and some remain as the compound . c and d are incorrect because, and do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise,   if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both and have a complete octet so can not accept any electrons which disqualifies them as acids.