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2 years ago

Calculate the pH when 60.0 mL of 0.200 M HBr is mixed with 30.0 mL of 0.400 M CH₃NH₂ (Kb = 4.4 × 10⁻⁴).

1 answer:

8 0

When a volume of 60.0 mL of 0.200 M HBr is mixed with a volume of 30.0 mL of 0.400 M CH3NH2, The pH value is mathematically given as

pH=10.64

<h3>What is the pH value when 60.0 mL of 0.200 M HBr is mixed with 30.0 mL of 0.400 M CH₃NH₂?</h3>

Question Parameters:

The pH when 60.0 mL of 0.200 M HBr

30.0 mL of 0.400 M CH₃NH₂ (Kb = 4.4 × 10^{-4}).

Generally, the equation for the Chemical Reaction is mathematically given as

H Br + H_3C NH_2----- > CH_3 NH_3 Br

Therefore

oH=p^{kb}+-log $\frac{salt}{base}$

OH=-log(4.4*10^{-4})+ $\frac{0.1}{0.1}$

OH=3.36

In conclusion, The equation pH value

pH+OH=14

Therefore

pH+=14-3.36

pH=10.64

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3 years ago

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