d)
*Note: "am" indicates that liquid ammonia is the solvent.
How do you solve for this? Also, how would you write the net ionic equation? Thank you!
12.9 part d
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Michelle_Nguyen_3F
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12.9 part d
Which of the following reactions can be classified as reactions between Bronsted acids and bases? For those that can be so classified, identify the acid and base. (Hint: It may help to write the net ionic equations.)
d) + KNH_{2}(am) \rightarrow KI(am) + 2 NH_{3}(l))
*Note: "am" indicates that liquid ammonia is the solvent.
How do you solve for this? Also, how would you write the net ionic equation? Thank you!
d)
*Note: "am" indicates that liquid ammonia is the solvent.
How do you solve for this? Also, how would you write the net ionic equation? Thank you!
Re: 12.9 part d
Good question. The first thing to note here is that the reaction takes place in liquid ammonia. That is, not in water (no hydronium ions).
Because NH4+ from NH4I is converted into NH3, there is a proton donated to the NH2-.
Because NH4+ from NH4I is converted into NH3, there is a proton donated to the NH2-.
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