When 1 mol of #NaBH_4# is used to reduce a ketone, how many moles of Hydride is used? How do you determine this?
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Theoretically, 1 mol of
The first step's equation is as follows:
However, because some of the reducing reagent may react with the solvent, an excess of it is frequently used.
Water is added and heated in the second step.
In doing so, the boron complex is hydrolyzed and alcohol is produced:
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When 1 mol of NaBH4 is used to reduce a ketone, 4 moles of hydride (H-) ions are used. This is because NaBH4 donates four hydride ions (H-) per molecule in the reduction reaction. The stoichiometry of the reaction between NaBH4 and the ketone dictates the number of hydride ions required for the reduction process.
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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
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