20 mL of 0.1M H2SO4 solution is added to 30 mL of 0.2 M NH4OH solution. The pH of the resultant mixture is: pkb of NH4OH=4.7

H2SO4+2NH4OH→NH22SO4+2H2O pOH=pKb+log⁡ salt base 4.7+log⁡42=5pH=14−5=9

20 mL of 0.1M H2SO4 solution is added to 30 mL of 0.2 M NH4OH solution. The pH of the resultant mixture is: pkb of NH4OH=4.7

H2SO4+2NH4OH→NH22SO4+2H2O pOH=pKb+log⁡ salt base 4.7+log⁡42=5pH=14−5=9

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20 mL of 0.1M H₂SO₄ solution is added to 30 mL of 0.2 M NH₄OH solution. The pH of the resultant mixture is: $[{pk}_{b} of {NH}_{4} OH = 4 .7]$

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$H_{2} {SO}_{4} + 2 {NH}_{4} OH \to {({NH}_{2})}_{2} {SO}_{4} + 2 H_{2} O$

$p^{OH} = p^{Kb} + \log [\frac{salt}{base}] \begin{array}{l} 4 .7 + \log \frac{4}{2} \\ = 5 \\ p^{H} = 14 - 5 = 9 \end{array}$

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20 mL of 0.1M H2SO4 solution is added to 30 mL of 0.2 M NH4OH solution. The pH of the resultant mixture is: pkb of NH4OH=4.7

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20 mL of 0.1M H₂SO₄ solution is added to 30 mL of 0.2 M NH₄OH solution. The pH of the resultant mixture is: $[{pk}_{b} of {NH}_{4} OH = 4 .7]$