What concentration of acetic acid is needed to give a hydrogen ion concentration of $$3.5$$ × $$10-4$$ M ? $$Ka=$$ $$1.8$$ × $$10-5$$ ?

Question

What concentration of acetic acid is needed to give a hydrogen ion concentration of $$3.5$$ × $$10-4$$ M ?     $$Ka=$$ $$1.8$$ × $$10-5$$ ?

Infinity Learn · Accepted Answer

$$CH3COOHC$$ $$-$$ Cα  ⇌  $$CH3COO-C$$α    $$+$$  $$H+C$$αLet the concentration of acetic acid be ‘C’.$$Ka=$$ $$1.8$$ × $$10-5$$ $$=$$ Cα.Cα$$C1-$$α $$=$$ Cα$$2Now$$  α$$2$$ $$=$$ KaC  or  α $$=KaC$$ or  Cα $$=$$ Ka.CCα $$=$$ $$H+$$ $$=$$ $$3.5$$ × $$10-4M$$∴       $$3.5$$ × $$10-4=$$ $$1.8$$ × $$10-5COr$$      C $$=$$ $$3.5$$ × $$10-41.8$$ × $$10-5C$$ $$=$$ $$3.5$$ × $$10-421.8$$ × $$10-5$$   $$=$$ $$12.25$$ × $$10-81.8$$ × $$10-5$$ $$=$$ $$6.80$$ × $$10-3M$$

What concentration of acetic acid is needed to give a hydrogen ion concentration of $3.5 \times 10^{- 4} M$ ? $(K_{a} = 1.8 \times 10^{- 5})$ ?

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What concentration of acetic acid is needed to give a hydrogen ion concentration of 3.5 × 10-4 M ? Ka= 1.8 × 10-5 ?

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What concentration of acetic acid is needed to give a hydrogen ion concentration of $3.5 \times 10^{- 4} M$ ? $(K_{a} = 1.8 \times 10^{- 5})$ ?