Chemistry problem: You can dissolve an aluminum soft drink can in an aqueous base of potassium hydroxide.?

Question

Given the following equation:
2Al(s) + 2KOH(aq) +6(H2O)[L] => 2KAl(OH)4[aq] +3(H2)[g]

If you place 2.05 g of aluminum in a beaker with 125-ml of 1.25 M KOH, will any aluminum remain? Show work and justify your answer so I can learn how to do this.

What mass of KAl(OH)4 is produced?

Thank you whoever helps solves this. I don't know how to solve these so show your work please. All the needed information to solve the problems is given.

Answer 1

Work out the moles of Al (mass/Ar) and the moles of KOH (volume x molarity/1000). See which is bigger.

Work out the Mr of potassium aluminate and multiply it by whichever of the moles you worked out earlier was the smaller.