Calculate pH of the following solutions:
(i) $0.001 M H N O_{3}$
(ii) $0.005 M H_{2} S O_{4}$
(iii) $0.01 M K O H$
(iv) $10^{- 8} M N a O H$
(v) $0.0008 M B a {(O H)}_{2}$

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Solution

Formula for $p H = - l o g [H^{+}]$
$(i) 0.001 M H {N O}_{3} ⇌ 0.001 M H^{+} p H = - l o g [0.001] p H = 3 (i i) 0.005 M H_{2} {S O}_{4} ⇌ 0.005 \times 2 M H^{+} p H = - l o g [0.01] p H = 2 (i i i) 0.01 M K O H ⇌ 0.01 M {O H}^{-} p [{O H}^{-}] = - l o g [0.01] p O H = 2 p H = 14 - p O H = 14 - 2 = 12 (i v) 10^{- 8} M N a O H ⇌ 10^{- 8} M {O H}^{-} p O H = - l o g [10^{- 8}] = 8 p H = 14 - 8 = 6 (v) 0.0008 M B a {(O H)}_{2} ⇌ 2 \times 0.0008 M {O H}^{-} p O H = - l o g [0.0016] = 2.7959 p H = 14 - 2.7959 = 11.2041$

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Calculate pH of the following solutions: (i) 0.001MHNO3 (ii) 0.005MH2SO4(iii) 0.01MKOH(iv) 10−8MNaOH (v) 0.0008MBa(OH)2

Calculate pH of the following solutions:
(i) $0.001 M H N O_{3}$
(ii) $0.005 M H_{2} S O_{4}$
(iii) $0.01 M K O H$
(iv) $10^{- 8} M N a O H$
(v) $0.0008 M B a {(O H)}_{2}$