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1.122 g of an unknown monoprotic base dissolved in 50.0 ml of water is titrated to endpoint with 20.0 ml of a 1.00 m hcl solution what is the unknown base?
Wiki User
∙ 14y ago
Assuming the base is a strong base (you don't have enough info if it isn't), and that the end point is neutralization...
You have 0.02 mol of acid (HCl is a strong acid, to get this multiply 0.020 L (20 mL) times 1 mol per liter (the molarity given as 1 M HCl). Therefore you must neutralize with 0.02 mol of base.
You know you have 1.122 g of the base, so you have to find the appropriate molecular weight of the base to give 0.02 mol
Set up the equation:
1.122 g of base divided by x g/mol (the molecular weight) = 0.02 mol
Make sure your units cancel, since you a dividing by g/mol the grams cancel and you are left with mol = mol, therefore units cancel. I cannot illustrate this more clearly, I apologize.
The equation to solve is therefore 1.122/x = 0.02, x=56.1 g/mol, therefore the base most is probably KOH (39 +17).
Wiki User
∙ 14y ago
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So... what's the question?
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