We’re being asked to determine whether HI can dissolve the given metal sample, write a balanced reaction, and the volume of 3.5 M HI required to completely dissolve the sample.
We’re going to dissolve metals meaning the metals will undergo oxidation. HI will break up in the solution:
• HI(aq) → H+(aq) + I-(aq)
▪ if we’re going to oxidize the metals, it means that something is also reduced in the solution
▪ I-(aq) → with negative charge and it is the most reduced form of I X
▪ H+(aq) → has a positive charge → can gain e- and can be reduced ü
Determine whether HI can dissolve each metal sample. If it can, write a balanced chemical reaction showing how the metal dissolves in HI and determine the minimum volume of 3.5 M HI required to completely dissolve the sample.
a. 2.15 g Al
b. 4.85 g Cu
c. 2.42 g Ag
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Our tutors have indicated that to solve this problem you will need to apply the Standard Hydrogen Electrode concept. If you need more Standard Hydrogen Electrode practice, you can also practice Standard Hydrogen Electrode practice problems.
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Based on our data, we think this problem is relevant for Professor Petit's class at CSUF.
What textbook is this problem found in?
Our data indicates that this problem or a close variation was asked in Chemistry: A Molecular Approach - Tro 3rd Edition. You can also practice Chemistry: A Molecular Approach - Tro 3rd Edition practice problems.