How many moles of Hydrochloric acid are needed to dissolve 39.0 grams of aluminum Hydroxide? I just need to write out the equation but I was out and don't know how PLEASE HELP!
Al(OH)3 + 3HCl ==> AlCl3 + 3H2O
Thank You so MUch, I havee a few more questions Down below, this is just the first THANK YOU!
To determine the number of moles of hydrochloric acid needed to dissolve 39.0 grams of aluminum hydroxide, we first need to write out the balanced chemical equation for the reaction between hydrochloric acid (HCl) and aluminum hydroxide (Al(OH)3).
The balanced equation for the reaction is as follows:
2 Al(OH)3 + 6 HCl → 2 AlCl3 + 6 H2O
Now, we can see that for every 2 moles of aluminum hydroxide (Al(OH)3), we need 6 moles of hydrochloric acid (HCl). This is based on the stoichiometric coefficients in the balanced chemical equation.
To calculate the number of moles of hydrochloric acid needed, we can use the formula:
Moles = Mass / Molar Mass
The molar mass of hydrochloric acid (HCl) is 36.46 g/mol.
Substituting the values into the formula, we have:
Moles of HCl = 39.0 g / 36.46 g/mol
Calculating this, we find:
Moles of HCl = 1.07 mol
Therefore, you would need 1.07 moles of hydrochloric acid to dissolve 39.0 grams of aluminum hydroxide.