A research student titrates 100 mL of a 0.2 M solution of hypobromous acid (HBrO) with 0.1 M NaOH....

Question

A research student titrates 100 mL of a 0.2 M solution of hypobromous acid (HBrO) with 0.1 M NaOH. What is the pH of the solution after 400 mL of NaOH is added at 25o C?  Ka (HBrO) = 2.5 × 10-9

Robert · Accepted Answer

According to the reaction: 
HOBr (aq) + NaOH (aq) ======= NaOBr (aq)  + H2O (l) 
Concentration of HOBr = 0.2 M 
Volume of HOBr = 100 mL 
No. of Moles of HOBr = 0.2 M x 0.1 L = 0.02 Moles 
Concentration of NaOH = 0.1 M 
Volume of NaOH = 400 mL 
No. of Moles of NaoH used = 0.1 M x 0.4 L = 0.

A research student titrates 100 mL of a 0.2 M solution of hypobromous acid (HBrO) with 0.1 M NaOH. What is the pH of the solution after 400 mL of NaOH is added at 25o C? Ka (HBrO) = 2.5 × 10-9

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