NCERT Class XI Chemistry Equilibrium Solutions
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Question : 48
Total: 73
Assuming complete dissociation, calculate the pH of the following solutions:
(a) 0.003 M HCl
(b) 0.005 M NaOH
(c) 0.002 M HBr
(d) 0.002 M KOH
(a) 0.003 M HCl
(b) 0.005 M NaOH
(c) 0.002 M HBr
(d) 0.002 M KOH
Solution:
(a) HCl + aq → H + + C l –
∴[ H + ] = [HCl] = 3 × 10 − 3 M, pH = - log ( 3 × 10 − 3 ) = 2.52
(b) NaOH + aq →N a + + O H −
∴[ O H − ] = 5 × 10 − 3 M
∴[ H + ] =
= 2 × 10 − 12 M , pH = - log (2 × 10 − 12 ) = 11.70
(c) HBr + aq →H + + B r −
∴[ H + ] = 2 × 10 − 3 M, pH = - log ( 2 × 10 − 3 ) = 2.70
(d) KOH + aq →K + + O H −
∴[ O H − ] = 2 × 10 − 3 M , [ H + ] =
= 5 × 10 − 12
pH = - log( 5 × 10 − 12 ) = 11.30
∴
(b) NaOH + aq →
∴
∴
(c) HBr + aq →
∴
(d) KOH + aq →
∴
pH = - log
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