Nov 4, 2020 · The reaction $\ce{CaO + SiO2 -> CaSiO3}$ is considered a neutralization reaction despite not producing water, because both reactants are reacting with water to produce a hydroxide ($\ce{Ca(OH)2}$ and an acid $\ce{H2SiO3}$.

Dec 30, 2021 · A neutralisation reaction is a reaction during which an acid reacts with a base to form a salt and water only. I understand the part : A neutralisation reaction is a reaction during which an acid reacts with a base. since, given that the acid is an H+ donor and the base and H+ acceptor, they will react to form water and bring the pH back to 7.

Sep 30, 2017 · Of course, a base reaction can be considered essentially the reverse, meaning that the acid constant typically given is actually $\mathrm pK_\mathrm a (\ce{HB+})$ rather than anything directly corresponding to the free base. If we now take the reaction of a (weak) acid and a (weak) base, we get equation $(3)$ and the equilibrium constant as ...

Sep 15, 2014 · While not an acid-base reaction, an example of mixing two relatively "safe" chemicals to form dangerous ones is bleach (sodium hypochlorite) plus ammonia - both common household chemicals. This reaction yields chloramine, dichloramine, and nitrogen trichloride, all more toxic and hazardous than bleach or ammonia.

Jul 18, 2018 · One can think of it as simply because of electrostatic attraction. Basically, an acid produces $\ce{H+}$ ions in water while a base produces $\ce{OH-}$ ions in water. So when you mix an acid and a base (e.g. sulfuric acid and sodium hydroxide) in a beaker, you get a solution containing $\ce{H+}$ and $\ce{OH-}$ ions.

You are right in that the reaction is $\mathrm{H}^+ + \mathrm{OH}^- \rightarrow \mathrm{H_2O}$, but recognise that bonds are formed in this reaction. Bond formation releases energy (and similarly bond breakage is endothermic), and thus neutralisation reactions are exothermic.

An acid-base reaction is not the exchange of a hydrogen atom $\ce{H}$. It is the exchange of a hydrogen ion (or proton) $\ce{H+}$. Thus your answer should be: $$\ce{NH3(aq) +HNO3(aq) -> NH4+(aq) + NO3-(aq)}$$ The given answer combines the two ions produced into a single compound. $$\ce{NH4+(aq) + NO3-(aq) ->NH4NO3(aq)}$$

Dec 25, 2017 · The Brønsted-Lowry theory describes acid-base reactions as proton transfers. The acid is the species which donates a proton while the base is the species that accepts a proton. Usually, $\ce{HCl}$ and $\ce{NaOH}$ are considered dissolved …

Jul 20, 2019 · The neutralization of a strong acid with a strong base then is always the same reaction: $$\ce{H+(aq) + OH-(aq) -> H2O(l)}$$ We can calculate the enthalpy of reaction from the enthalpies of formation at a temperature of $\pu{25 ^\circ C}$ .

I need help on identifying precipitation, acid-base, and redox reactions. I know what each one is in theory: Precipitation: Creating a solid; Acid-Base: neutralization; Redox: exchange of electrons; But given a chemical reaction like: HCl (aq) + NaOH (aq) → H2O (l) + NaCl (aq) I need to understand how to classify them.