The pH of a 0-1 M NH4OH solution0-1 M is equal to-Given that - Kb - 10-5-

The correct option is B 11 NH_4OH → NH_4^+ +OH^ For a weak base,Concentration of [OH^ ] = Cα = √(C× K_b ) = √(0.1×10^ 5) = 10^ 3M So, #160; ...

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Allotropes of Phosphorus

The pH of a ...

Question

The pH of a $0.1 M N H_{4} O H$ solution is equal to:
[Given that : $K_{b} = 10^{- 5}$ ]

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N H_{4} O H

K_{b}

= 1.0 \times 10^{- 5}

K_{b}

0.2 M

p H

9.50

p H

0.2 M

K_{b} = 1.76 \times 10^{- 5}

∣ ∣ ∣ ∣ ∣ \begin{matrix} ^{10} C_{4} & ^{10} C_{5} & ^{11} C_{m}^{11} C_{6} & ^{11} C_{7} & ^{12} C_{m + 2}^{12} C_{8} & ^{12} C_{9} & ^{13} C_{m + 4} \end{matrix} ∣ ∣ ∣ ∣ ∣

m

p H

N H_{4} C l

N H_{4} O H

p K_{b}

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