An aqueous solution of hydrobromic acid is standardized by titration with a 0.14

Question

An aqueous solution of hydrobromic acid is standardized by titration with a 0.145 M solution of barium hydroxide.

If 21.3 mL of base are required to neutralize 14.6 mL of the acid, what is the molarity of the hydrobromic acid solution?

M hydrobromic acid

2)An aqueous solution of potassium hydroxide is standardized by titration with a 0.136 M solution of hydroiodic acid.

If 18.2 mL of base are required to neutralize 11.7 mL of the acid, what is the molarity of the potassium hydroxide solution?

M potassium hydroxide

Explanation / Answer

The reaction between HBr and Ba(OH)2 is given by

Ba(OH)2 + 2HBr(aq) ---->2HOH + BaBr2

1 mole of Ba(OH)2 requires 2 moles of HBr

moles of Ba(OH)2= molarity* Volume = 0.145*21.3/1000 =0.003089 moles

Moles of HBr= 2*0.003089=0.006177

Molarity =0.006177*1000/14.6=0.423M

2. HI+ KOH---> NaI +H2O

1 mole of HI requires 1 mole of KOH

Moles of acid = 0.136*11.7/1000= 0.001591

Moles of NaOH= 0.001591, Molarity of NaOH= 0.001591*1000/18.2=0.087429

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