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parwana
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Calculate [H+]?
Calculate [ H + ] of a 0.220 M solution of Aniline C6H5NH2 Kb = 7.4e-10
Calculate [ H + ] of a 0.220 M solution of Aniline C6H5NH2 Kb = 7.4e-10
chem_tr said:Sirus is right; an alternative point of view may be using dissociative approach. In this, you start with 0.220 M of aniline, but only [itex]\displaystyle x[/itex] of it is ionized to give some [itex]\displaystyle H^+[/itex]. We know the equilibrium constant of this reaction, i.e., [tex]\displaystyle \frac {10^{-14}}{K_b}[/tex].
[tex]\displaystyle \underbrace{C_6H_5NH_2_{(aq)}}_{0.220-x} \leftrightharpoons \underbrace{C_6H_5NH^-_{(aq)}}_{x}+\underbrace{H^+_{(aq)}}_{x}[/tex]
The formula for calculating [H+] is pH = -log[H+].
To calculate [H+] from pH, use the formula [H+] = 10^-pH.
The relationship between [H+] and pH is inverse. As the concentration of [H+] increases, pH decreases and vice versa.
No, you cannot calculate [H+] without knowing the pH. The pH is necessary for the calculation of [H+] using the formula [H+] = 10^-pH.
Calculating [H+] is important for understanding the acidity or basicity of a solution. It is also essential in various scientific fields such as chemistry, biology, and environmental science.