Chemistry - Ionic Equilibrium Question with Solution | TestHub

ChemistryIonic EquilibriumMiscellaneous/MixedEasy2 minPYQ_2020

ChemistryEasysingle choice

What will be the pH of a solution formed by mixing 40 $c m^{3}$ of 0.1 M HCl with 10 $c m^{3}$ of 0.45 M NaOH?

Options:

Answer:

Solution:

Number of moles of HCl $= \frac{M V}{1000} = \frac{0.1 \times 40}{1000} = 0.004$
Number of moles of NaOH $= \frac{M V}{1000} = \frac{0.45 \times 10}{1000} = 0.0045$
Remaining moles of NaOH after neutralization = 0.0045 – 0.004 = 0.0005
Molarity of $O H^{-}$ $= \frac{0.0005}{50} \times 1000 = 0.01 M$
So pOH $= 2$
So pH = 14 – 2 = 12

Stream:NTA_ABHYASSubject:ChemistryTopic:Ionic EquilibriumSubtopic:Miscellaneous/Mixed

⏱ 2mℹ️ Source: PYQ_2020

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