because they dissociate more rapidly and donate hydrogen ion for reduction as soon as it is ionized
No. Most monoprotic acids are weak.
HCl, HNO3, CH3COOH, H2BO3H (only the last one written H's are acidic!) also called monoprotic acids.
It is a strong monoprotic base. Monoprotic means it can accept a proton (and Bronsted-Lowry theory calls proton acceptors BASES) So yes it can accept 1 (mono) proton. Strong acids or bases dissociate completely in aqueous solutions. Therefore this strong monoprotic base would dissociate completely into component ions in solution (this case water) yielding Na+, OH- and H20 (and heat).
The strong acids have pH=2 as HCl or H2SO4.
If a weak acid is poured into a strong acid, if the solution aqueous, the solution will become more acidic.
No. Most monoprotic acids are weak.
HCl, HNO3, CH3COOH, H2BO3H (only the last one written H's are acidic!) also called monoprotic acids.
The reaction that occurs between a strong monoprotic acid and sodium hydroxide is H++OH- => H2O. This reaction is the same for all strong monoprotic acids and sodium hydroxide so, in theory, they should all have the same standard enthalpy of reaction. In practice, there are very slight differences between acids. If you are in a freshman or sophmore chemistry class, say yes. If you are in physical or analytical chemistry say no.
It is a strong monoprotic base. Monoprotic means it can accept a proton (and Bronsted-Lowry theory calls proton acceptors BASES) So yes it can accept 1 (mono) proton. Strong acids or bases dissociate completely in aqueous solutions. Therefore this strong monoprotic base would dissociate completely into component ions in solution (this case water) yielding Na+, OH- and H20 (and heat).
The strong acids have pH=2 as HCl or H2SO4.
By Arrhenius's definition it isdissociatesin water to release H+. Which it does:HCl (in water) --> H+ + Cl-By the Bronsted-Lowry definition it is a proton donor, which it is. It only becomes an acid in water.Water has a limiting effect on the strength of acids and bases. All strong acids behave the same in water -- 1 M solutions of the strong acids all behave as 1 M solutions of the H3O+ ion -- and very weak acids cannot act as acids in water. Acid-base reactions don't have to occur in water, however.
If a weak acid is poured into a strong acid, if the solution aqueous, the solution will become more acidic.
No, household bleach is a strong base. Both strong acids and strong bases are caustic.
Strong acids are strongly acidic. Strong alkalies are strongly alkaline. And both strong acids and strong alkalies are equally corrosive, though I would say that strong acids and more dangerous to handle than strong alkali.
Yes, both sulfur oxides are acidic: with water the give sulfurous (weak -) and sulfuric (strong -) acids
They are highly corrosive in nature and dissociate extensively in solutions. They behave as good electrolytes.
Believe it or not, almost everything we eat or drink is acidic. Some foods are relatively strong acids such as lemon juice or vinegar. Others are only very mildly acidic, such as milk.