12.8 ml of 4.65 M phosphoric acid was accidentally spilled on a laboratory bench

Question

12.8 ml of 4.65 M phosphoric acid was accidentally spilled on a laboratory bench top, Pulverized barium hydroxide anhydride (a base) was handy and quickly used to neutralize the aci 8.85 g of this base was distributed over the acid spill. Was sufficient base used or do ene. more? What amount (in grams) do your calculations show was the excess or the amount 1, still needed? The neutralization reaction described above yields water as one of the products. Calculate the maximum yield of water (in grams).

Explanation / Answer

Ans 1 :

The balanced reaction is given as :

3Ba(OH)2 + 2H3PO4 = Ba3(PO4)2 + 6H2O

Number of moles of acid = 4.65 x 0.0128 = 0.05952 mol

Number of moles of Ba(OH)2 = 8.85 / 171.3 = 0.05165 mol

2 moles of acid in the reaction requires 3 moles of base

Then 0.05952 mol of acid will require : ( 0.05952 x 3) / 2 = 0.08928 mol of base

So the base was insufficient , and we need to apply more of it to neutralise the complete acid spillage.

Number of moles of base needed = 0.08928 - 0.05165 = 0.0376

So more Ba(OH)2 needed = 0.0376 x 171.3

= 6.44 grams

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