In the following balanced neutralization reaction equation, how many moles of Ca(OH)2 are required to completely neutralize 1.2
1 answer:
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Data Given:
Molarity = 0.085 M
Ka = 4.5 × 10⁻⁴
To Find:
pH = ?
Solution:
First find out the concentration of [H⁺] Ions using following formula,
[H⁺] =
Puting values,
[H⁺] =
[H⁺] =
[H⁺] = <span>0.00618465843
</span>Or,
[H⁺] = 6.18 × 10⁻³
Calculate pH as,
pH = -log [H⁺]
pH = -log (6.18 × 10⁻³)
pH = 2.20
Molarity = 0.085 M
Ka = 4.5 × 10⁻⁴
To Find:
pH = ?
Solution:
First find out the concentration of [H⁺] Ions using following formula,
[H⁺] =
Puting values,
[H⁺] =
[H⁺] =
[H⁺] = <span>0.00618465843
</span>Or,
[H⁺] = 6.18 × 10⁻³
Calculate pH as,
pH = -log [H⁺]
pH = -log (6.18 × 10⁻³)
pH = 2.20