What is the pH of 0.005 M Ba(OH)2 solution? a) 12 b) 2 c) 0.005 d)...

What is the pH of 0.005 M Ba(OH)2 solution?
a) 12
b) 2
c) 0.005
d) -2

Expert Solution

Given concentration of Ba(OH)₂ is = 0.005 M

= 5x10^-3 M

Ba(OH)₂ Ba²⁺ + 2OH^-

1 mole of Ba(OH)₂ produces 2 moles of OH^-

So [OH^-] = 2x concentration of Ba(OH)₂

= 2 x 5x10^-3 M

= 10 x 10 ^-3 M

= 10 ^-2 M

So pOH = - log[OH^-]

= - log 10 ^-2

= 2

pH = 14 - pOH

= 14 - 2

= 12

Therefore pH of the solution is 12

So option (a) is correct.

queen_honey_blossom answered 1 year ago

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