Neutralization Reactions
Chemistry ⇒ Acids, Bases, and Salts
Neutralization Reactions starts at 7 and continues till grade 12.
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See sample questions for grade 12
A 100 mL solution of 0.5 M H2SO4 is neutralized by NaOH. Calculate the moles of NaOH required.
A 25 mL sample of 0.2 M HNO3 is neutralized by 0.1 M KOH. Calculate the volume of KOH required.
A solution contains 0.05 mol of HCl. How many moles of NaOH are needed to neutralize it completely?
A solution of 0.1 M HCl is titrated with 0.1 M NaOH. If 30 mL of NaOH is required to reach the endpoint, what was the initial volume of HCl?
A student mixes 50 mL of 0.1 M HCl with 50 mL of 0.1 M NaOH. What is the pH of the resulting solution?
Calculate the volume of 0.2 M NaOH required to completely neutralize 25 mL of 0.1 M H2SO4.
Describe the difference between the neutralization of a monoprotic acid and a diprotic acid.
Describe the role of titration in studying neutralization reactions.
Describe what happens to the pH of a solution as a strong acid is gradually neutralized by a strong base.
Explain why the neutralization of a polyprotic acid requires more than one equivalent of base.
Explain why the neutralization of a weak acid with a strong base is not as exothermic as that of a strong acid with a strong base.
Explain why the pH at the equivalence point in the titration of a weak acid with a strong base is greater than 7.
Explain why the salt formed in a neutralization reaction may not always result in a neutral solution.
What is a neutralization reaction?
Write the balanced chemical equation for the neutralization of sulfuric acid (H2SO4) with potassium hydroxide (KOH).
A 0.2 M solution of H2SO4 is titrated with 0.1 M Ba(OH)2. Calculate the volume of Ba(OH)2 required to neutralize 50 mL of the acid.
A 50 mL solution of 0.1 M CH3COOH (acetic acid) is titrated with 0.1 M NaOH. Calculate the pH at the equivalence point. (Given: Ka for acetic acid = 1.8 × 10-5)
A laboratory technician accidentally adds excess NaOH to a solution of HCl during a titration. Describe the chemical species present in the final solution and explain the resulting pH.
Describe how a buffer solution can be formed during a neutralization reaction, and provide a specific example with chemical equations.
Explain, with reference to chemical equations, why the pH at the equivalence point in the titration of a weak base with a strong acid is less than 7.
