Depends what the two solutions are.....but the classic example is
hydrochloric acid and sodium hydroxide.
HCl + NaOH === NaCl + H2O
This is a neutralization reaction that produces a salt called sodium chloride (table salt) and water.
When mixing a strong base with a weak acid, the strong base will completely neutralize the weak acid, resulting in the formation of water and a salt. The pH of the solution will be higher than 7 due to the remaining excess of hydroxide ions from the base.
In an acid-base titration experiment, a solution of known concentration (the titrant) is slowly added to a solution of unknown concentration until the reaction is complete. This allows for the determination of the unknown concentration by measuring the volume of titrant needed to reach the equivalence point. The pH at the equivalence point can indicate the nature of the reaction (e.g., strong acid-strong base, weak acid-strong base) and can be used to calculate the pKa of the weak acid or base involved.
Salt can be neutral, acidic, or basic. Salts are formed through the reaction of an acid and a base. If the reaction involves a strong acid and a strong base, the resulting salt is neutral (like NaCl table salt). A weak acid and a strong base result in a basic salt, and a strong acid and a weak base form an acid salt.
Dimethylamine is actually a weak base, not a strong acid. It is a derivative of ammonia and can accept protons in solution, making it a base.
Dissolved carbon dioxide in water (carbonic acid) is weak acid.
The mixing of a weak acid with a strong base is generally exothermic. The reaction generates heat as the acid and base neutralize each other.
When a strong base reacts with a weak acid, the base will completely neutralize the acid, forming water and a salt as the products of the reaction. This process is known as a neutralization reaction.
None of the above. Br- is neutral, with no acidic or basic properties
Ephedrine sulfate will act as a weak acid in solution because yes it is the salt of a weak base (ephedrine) and a strong acid (sulfuric acid)
NaHCO3 is a weak base, with a conjugate acid of H2CO3+.
In a weak base-strong acid titration, the balanced chemical equation is: Base (B) Acid (H) Conjugate Acid (BH) This equation represents the reaction between the weak base (B) and the strong acid (H), resulting in the formation of the conjugate acid (BH).
A weak acid/base will have a stronger conjugate base/acid. The conjugate acids/bases of strong bases/acids are very weak because they have no attraction to protons or hydroxides, which is why the reaction shifts all the way to the right and the Ka/b is large.
a weak acid and strong base. At the equivalence point of a titration between a weak acid and a strong base, the resulting solution will have a pH greater than 7, indicating a basic solution. For the solution to be noticeably acidic at the equivalence point, it would suggest an excess of the weak acid after the reaction, which means that the acid is likely weak and not completely neutralized by the strong base.
It is the product of a strong acid and a weak base, but is itself a mildly acidic salt.
If acid is strong then its conjugate base must be weak, if conjugate base is strong it again accept the H+ ions so acid can neither be strong, similarly if base is strong its conjugate acid must be weak.
No, potassium acetate is a salt formed by the reaction of a strong base (potassium hydroxide) with a weak acid (acetic acid). Potassium acetate is neutral and does not act as an acid in aqueous solutions.
The solution at the endpoint of an acid-base titration involving a weak acid and a strong base will be alkaline. This is because the weak acid will have been neutralized by the strong base, resulting in excess hydroxide ions in the solution causing it to be alkaline.