Chemistry - Ionic Equilibrium Question with Solution | TestHub

ChemistryIonic EquilibriumpH of Strong and Weak Acids and BasesEasy2 minPYQ_2018

ChemistryEasysingle choice

When $50 mL$ of $0.1 M NH_{3}$ is mixed with $10 mL$ of $0.1 M HCl$ then what is the $pH$ of resultant solution? $(p K_{b} = 4.75)$

Options:

Answer:

Solution:

$NH_{3} + HCl ⟶ NH_{4} Cl Initial 50 \times 0.1 10 \times 0.1 = 5 mmol = 1 mmol After 4 mmol 0 mmol 1 mmol reaction pOH = p K_{b} + lo g \frac{[ salt ]}{[ base ]} = 4.75 + lo g (\frac{1}{4}) = 4.15 pH = 14 - pOH = 14 - 4.15 = 9.85$

Stream:AIIMSSubject:ChemistryTopic:Ionic EquilibriumSubtopic:pH of Strong and Weak Acids and Bases

⏱ 2mℹ️ Source: PYQ_2018

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