Question

If 11.3 mL of 0.110 M HCl is required to neutralize 25.00 mL of a
barium hydroxide solution, what is the molarity of the barium
hydroxide?

2 HCl + Ba(𝑂𝐻)_2→𝐵𝑎〖𝐶𝑙〗_2 + 2 𝐻_2 𝑂

Accepted Answer

Correct option is A) THE TITRATION REACTION IS:BA(OH)2​+2HCL⟶BACL2​,+H2​OACCORDING TO THE REACTION, THE FORMULA FOR A BALANCED EQUATION ISNO.OFMOLECULESOFBA(OH)2​ VOLUMEOFBA(OH)2​×MOLARITY​=NO.OFMOLECULESOFHCL VOLUMEOFHCL×MOLARITY​ =1 25×MOLARITYOFBA(OH)2​​=2 35×0.1​THEREFORE, MOLARITY OF BARIUM HYDROXIDE =0.07

Question #290403

Expert's answer

the titration reaction is:Ba(OH)2+2HCl⟶BaCl2,+H2OAccording to the reaction, the formula for a balanced equation isNo.ofmoleculesofBa(OH)2
VolumeofBa(OH)2×Molarity=No.ofmoleculesofHCl
VolumeofHCl×Molarity
=1
25×MolarityofBa(OH)2=2
35×0.1Therefore, molarity of barium hydroxide =0.07