Acid-Base Theory

Open Ended

Why is it important to understand the different definitions of acids and bases, such as the Arrhenius and Brønsted–Lowry models?

Open Ended

What is acid? What is base?

Multiple Choice

Which of the following is NOT a property of acids?

• Taste bitter

• Taste sour

• Corrosive

• React with most metals to produce salt and hydrogen gas

Open Ended

Explain how you can distinguish between an acid and a base using indicators, based on the information provided.

Multiple Select

Which of the following statements about bases is/are correct?

• Bases taste bitter

• Bases feel slippery or soapy

• Bases have a low pH value

• Bases turn red litmus blue

Multiple Choice

According to the Arrhenius theory, what ion does a base produce when dissolved in water?

• H+

• OH-

• Na+

• Cl-

Multiple Choice

What is the chemical formula of the hydronium ion formed when a proton is added to water?

• H2O

• H3O+

• OH-

• H2O2

Open Ended

Explain the difference between the Arrhenius definition of acids and the practical understanding of the hydronium ion in water.

Multiple Choice

Which of the following acids is diprotic?

• HCl

• H2SO4

• H3PO4

• CH3COOH

Multiple Select

Select all statements that correctly describe the dissociation of bases in water.

• A monobasic base produces one OH- ion per formula unit.

• A dibasic base produces two OH- ions per formula unit.

• A tribasic base produces three OH- ions per formula unit.

• All bases are soluble in water.

Open Ended

Compare and contrast the solubility of acids and bases in water, and explain the significance of the term 'alkali'.

Open Ended

Does Arrhenius theory properly define and describe acid-base? Is there any limitation?

Multiple Select

Which of the following are limitations of the Arrhenius acid-base theory?

• It only applies to aqueous solutions.

• It cannot explain the acidity of SO3.

• It explains all acid-base reactions.

• It cannot explain the basicity of NH3.

Multiple Choice

Which of the following reactions can be explained by Arrhenius acid-base theory?

• NH3 + H2O ⇌ NH4+ + OH−

• MgO + H2O → Mg(OH)2

• SO3 + H2O → H2SO4

• NH3 is a base, but does not produce OH− directly

Multiple Choice

Which of the following best describes the Brønsted–Lowry definition of acids and bases?

• Acids produce H+ ions in aqueous solution, bases produce OH- ions

• Acids are proton donors, bases are proton acceptors

• Acids turn litmus paper red, bases turn it blue

• Acids react with metals to produce hydrogen gas

Open Ended

Explain the difference between the Arrhenius and Brønsted-Lowry definitions of acids and bases.

Multiple Select

Which of the following are conjugate acid-base pairs in the reaction NH3(g) + H2O(l) ⇌ NH4+(aq) + OH−(aq)?

• NH3 and NH4+

• H2O and OH−

• NH3 and OH−

• NH4+ and H2O

Open Ended

Explain one limitation of the Brønsted-Lowry acid-base theory using an example from the slides.

Multiple Choice

Which of the following reactions cannot be explained by the Brønsted-Lowry acid-base theory?

• NH3 + BF3 → NH3BF3

• HCl + NaOH → NaCl + H2O

• 2HCl + Mg → MgCl2 + H2

• HCl + CaCO3 → CaCl2 + H2O + CO2

Multiple Choice

Which of the following are products of the reaction between hydrochloric acid and magnesium?

• Magnesium chloride and hydrogen

• Sodium chloride and water

• Calcium chloride and water

• Magnesium sulfate and hydrogen

Open Ended

Compare the products formed when hydrochloric acid reacts with sodium hydroxide and with calcium carbonate. What are the differences in the products?

Multiple Choice

Which ions are considered spectator ions in the reaction between HCl(aq) and NaOH(aq)?

• Cl⁻ and Na⁺

• H⁺ and OH⁻

• Na⁺ and H⁺

• Cl⁻ and OH⁻

Open Ended

Any comment on acid-base reaction?

Open Ended

After learning about acid-base theory, what is one question you still have or something you would like to know more about?

Multiple Choice

What is the main difference between the Arrhenius and Brønsted–Lowry definitions of acids and bases?

• Arrhenius focuses on H+/OH- in aqueous solutions, while Brønsted–Lowry focuses on proton donors and acceptors.

• Arrhenius focuses on proton donors and acceptors, while Brønsted–Lowry focuses on H+/OH- in aqueous solutions.

• Both definitions are exactly the same.

• Arrhenius definition is only for gases.