Which of the following reactions is most consistent with that of a base? a) NH 4 + → NH 3 + H + b) H 2 CO 3 → HCO 3 - + H + c) NaOH → Na + + OH - d) HCl → H + + Cl -

Okay, everyone, which of the following reactions is most consistent with that of a base? Okay. So what technically is a base? Remember, in acids and bases, a base is a substance that decreases the hydrogen ion concentration. Now, if you look at our answer choices here, there's only actually one that doesn't make more hydrogen ions. If you look at our answer choices, answer choice a creates a hydrogen ion, b also creates a hydrogen ion, d also creates a hydrogen ion. In fact, these are acids because they are increasing the hydrogen ion concentration, but a base is the exact opposite. It decreases the hydrogen ion concentration. So by process of elimination, we are left with answer choice C, which in fact is the correct answer. But why is it going to decrease the hydrogen ion concentration? Because it creates this hydroxide ion here. And remember that hydroxide ions plus hydrogen ions make what? Remember that together, they are going to create water, which is going to remove many of the hydrogen ions from that solution, decreasing their concentration. So, in fact, the only substance here that is going to react like a base is going to be answer choice c, which is sodium hydroxide. Okay, everyone. Let's move on to our next video.

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2. Cell Chemistry & Cell Components

Acids and Bases

Anatomy & Physiology

2. Cell Chemistry & Cell Components

Acids and Bases

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Multiple Choice

Which of the following reactions is most consistent with that of a base?
a) NH₄⁺ → NH₃ + H⁺
b) H₂CO₃ → HCO₃^- + H⁺
c) NaOH → Na⁺ + OH^-
d) HCl → H⁺ + Cl^-

a) NH₄⁺ → NH₃ + H⁺

b) H₂CO₃ → HCO₃^- + H⁺

c) NaOH → Na⁺ + OH^-

d) HCl → H⁺ + Cl^-

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Verified step by step guidance

Identify the definition of a base in chemistry: A base is a substance that can accept hydrogen ions (H+) or release hydroxide ions (OH-) in solution.

Examine each reaction to determine if it involves the release of hydroxide ions (OH-) or the acceptance of hydrogen ions (H+).

Analyze the first reaction: NH4+ → NH3 + H+. This reaction involves the release of a hydrogen ion (H+), which is characteristic of an acid, not a base.

Analyze the second reaction: H2CO3 → HCO3- + H+. This reaction also involves the release of a hydrogen ion (H+), indicating acidic behavior.

Analyze the third reaction: NaOH → Na+ + OH-. This reaction involves the release of hydroxide ions (OH-), which is consistent with the behavior of a base.