no they act stronger
Because the conjugate acid of a strong base is a much weaker acid than water. Since the conjugate acid is so weak, its chemical action as an acid is negligible in solution. Strong bases have very weak conjugate acids. Weak bases have relatively strong conjugate acids. The same is true for the conjugate bases of strong acids, such as HCl. Cl- is a much weaker base than than water, so its effects are also negligible.
Yes if u add 2 acids or bases or and acid and base together if both contain acids or bases it creates a poisounos gas that can kill or knock you out and will make pH higher. Dont try it though buy pH paper and use on ammonia ammonia is about a 11-12 on pH scale its very powerful. that was extra but yes it can cause sudden change matter what acids or bases you combine it with.
base
litmus is a dye obtained from lichens. These dyes react with acids and bases, showing a color change.
Chlorine is not a digestive substance, it is a gas that can be corrosive in solutions, as strong acids and bases. Sodium hypochlorite (bleach) breaks down organic substances in water by forming hydrochloric acid and oxygen.
no they act stronger
yes
Yes, it is correct.
No, the other way around would be correct
Lowest pH, strong acids, then weak acids, then salts of strong acids and strong bases, then salts of weak acids and strong bases, then weak bases, then strong bases. All very confusing!
Buffer systems. They convert strong acids or bases into weak acids or bases.
Strong acids and strong bases are both usually corrosive.
No. Many strong electrolytes are bases or neutral salts.
They either have a high concentration of H+ ions (acids) or OH- ions (bases). Strong acids and bases are also highly corrosive relative to weaker more neutral acids/bases.
Solubility. If the acid dissociates in water easily then it is a stong acid (same goes for bases). Strong acids: H2SO4, HF weak acids: HBr, CH3COOH
Strong acids do several things easily burn skin, neutralize bases and react with/ corrode metals. This is all because of the free movement of the H+ ion
buffers