A buffer solution is prepared in which the concentration of NH_(3) is 0.30 M and the concentrationof NH_(4)^(+) is 0.20 M. If the equilibrium constant, K_(b) for NH_(3) equals 1.8xx10^(-5), what is the pH of this solution ?

A buffer solution is prepared in which the concentration of NH_(3) is

1.	A buffer solution is prepared in which the concentration of NH_(3) is 0.30 M and the concentrationof NH_(4)^(+) is 0.20 M. If the equilibrium constant, K_(b) for NH_(3) equals 1.8xx10^(-5), what is the pH of this solution ?
Answer» <html><body><p><<a href="https://interviewquestions.tuteehub.com/tag/p-588962" style="font-weight:bold;" target="_blank" title="Click to know more about P">P</a>>8.73<br/>9.08<br/>9.43<br/>11.72</p>Solution :`p_(<a href="https://interviewquestions.tuteehub.com/tag/oh-585115" style="font-weight:bold;" target="_blank" title="Click to know more about OH">OH</a>)=pK_(<a href="https://interviewquestions.tuteehub.com/tag/b-387190" style="font-weight:bold;" target="_blank" title="Click to know more about B">B</a>)+log.(["Salt"])/(["<a href="https://interviewquestions.tuteehub.com/tag/base-892693" style="font-weight:bold;" target="_blank" title="Click to know more about BASE">BASE</a>"])=4.74+log.(0.20)/(0.30)` <br/> `=4.74+(0.301-0.4.74)=4.74-0.176` <br/> `=4.56` <br/> `:. pH = 14 - 4.56 = 9.44`</body></html>