Find the volume of 0.110 M hydrochloric acid necessary to react completely with 1.54 Al(OH)3.
Please explain how to do this.
Indicate your subject in the "School Subject" box, so those with expertise in the area will respond to the question.
To find the volume of hydrochloric acid necessary to react completely with Al(OH)3, we need to determine the balanced chemical equation for the reaction between hydrochloric acid (HCl) and aluminum hydroxide (Al(OH)3).
The balanced chemical equation for this reaction is:
3HCl + Al(OH)3 -> AlCl3 + 3H2O
From the balanced equation, we can see that the ratio between HCl and Al(OH)3 is 3:1. This means that for every 3 moles of HCl, we need 1 mole of Al(OH)3 to react completely.
Now, we need to calculate the moles of Al(OH)3 we have. The molar mass of Al(OH)3 can be calculated as follows:
Al: 1 * atomic mass of Al
O: 3 * atomic mass of O
H: 3 * atomic mass of H
So the molar mass of Al(OH)3 is:
1 * (atomic mass of Al) + 3 * (atomic mass of O) + 3 * (atomic mass of H)
Now, we can calculate the moles of Al(OH)3 we have by dividing its mass by its molar mass.
Next, we need to determine the amount of HCl in moles required for the reaction to occur completely. Since the ratio of HCl to Al(OH)3 is 3:1, we can multiply the moles of Al(OH)3 by 3 to find the moles of HCl required.
Finally, we need to find the volume of 0.110 M HCl solution that contains the calculated moles of HCl. We can use the equation:
moles = molarity * volume
Rearranging the equation to solve for volume, we have:
volume = moles / molarity
Substituting the moles of HCl and the molarity into the equation will give us the volume of hydrochloric acid solution required to react completely with the given amount of Al(OH)3.