Strong acid vs Strong base

What is the pH at the equivalence point in a strong acid–strong base titration?

What options below are strong acid?

• HF

• HCl

• H₂SO₄

• HCN

Which acid base pair represents this titration curve?

• HF + NaOH

• HCl + CH₃COOH

• HCl + NaOH

• HCN + HCOOH

Which titration curve is strong acid vs strong base?

• A

• B

• C

• D

Why pH value at point 1 is so low?

• The strong acid is only partially ionized, producing few H⁺ ions.

• No base has been added yet, so the solution contains a high concentration of H⁺ ions from the fully ionized strong acid.

• The base neutralizes all the acid instantly, lowering the pH.

• The acid has reacted with water to form a weak acidic solution.

From point 1 to point 2, why the graph gradually curve upward?

• The strong acid becomes weaker over time, raising the pH.

• The acid is forming a buffer solution with the base, which causes a steep pH rise.

• The acid is gradually neutralized by the added base

• The indicator added increases the pH before neutralization begins.

Point 3 is known as equivalance point which result in pH7. Why?

• The salt formed is acidic and lowers the pH.

• Both the acid and base are strong, the resulting solution contains only neutral water and a neutral salt.

• The acid and base are only partially ionized, so pH stabilizes at 7.

• The solution at point 3 now contains a buffer of weak acid and its conjugate base. Thus, the pH is balanced at 7.

Why does the rise sharply and remain high after the equivalence point (Point 4) in a strong acid–strong base titration?

• The acid becomes a weak acid, so it no longer neutralizes the base effectively.

• The indicator reacts with water to produce hydroxide ions.

• The solution forms a buffer, keeping the pH high and stable.

• Excess OH⁻ ions from the added strong base raise the pH significantly.