When widespread hydroxide salts (i.e. those of sodium or potassium) are added 1:1 to a strong acid, #HX#, a neutralization reaction occurs to offer #NaX#, or #KX#.

i.e. #HX + MOH rarr MX + H_2O#.

You are watching: What is true of a strong base?

Due to the fact that #X^-# is the conjugate base of a solid acid, by interpretation it is very weakly basic and will certainly not influence solution #pH#.


*

As you recognize, a salt is an ionic compound that is the product of a neutralization reaction, which occurs when an acid and also a base react.

Strong acids and solid bases are characterized by the fact that they dissociate completely in aqueous solution.

#HA_((aq)) + H_2O_((l)) rightleftharpoons H_3O_((aq))^(+) + A_((aq))^(-)#

#B_((aq)) + H_2O_((l)) rightleftharpoons OH_((aq))^(-) + BH_((aq))^(+)#

This means that the equilibrium reaction that is establiburned once they react through water will lie extremely much to the right. Essentially, this reaction can be seen as going to completion, interpretation that the acid and also the base will just exist as ions in solution.

#HA_((aq)) + H_2O_((l)) -> H_3O_((aq))^(+) + A_((aq))^(-)#

#B_((aq)) + H_2O_((l)) -> OH_((aq))^(-) + BH_((aq))^(+)#

Now, hydrolisys occurs once the cations and also anions that outcome from the neutralization reactivity react with water molecules, either via a hydroxide ion or with a hydronium ion.

For the conjugate base of a solid acid, this possible reactivity through water would certainly reform the solid acid, which is not feasible.

#A_((aq))^(-) + H_3O_((aq))^(+) color(red)(cancel(color(black)(->))) HA_((aq)) + H_2O_((l))#

The solid acid will be totally dissociated in aqueous solution, so any type of attempt to redevelop it would ssuggest not take location. Conjugate bvases of solid acids cannot accept protons from water.

See more: Why Does Pre Workout Make Me Poop ​, Jobs Ecityworks, (Explained For Beginners)

The very same is true for the conjugate acid of a solid base. It will not react with water to recreate the solid base because of the one-way street of the abovementioned dissociation equilibrium

#BH_((aq))^(+) + OH_((aq))^(-) color(red)(cancel(color(black)(->))) B_((aq)) + H_2O_((l))#

Conjugate acids of strong bases cannot donate protons to water.

An vital consequence of this reality is the neutral pH you gain once a strong acid and a strong base react completely.