Question

1.) a buffer solution is 0.453 M im HNO2 and 0.339 M in NaNO2. If Ka for HNO2 is 4.5x10^-4, what is the pH of this buffer solution?

pH = ????

2.) A buffer solution is 0.373 M in H2C2O4 and 0.303 M in KHC2O4. If Ka1 for H2C2O4 is 5.9x10^-2, what is the pH of this buffer solution?

pH = ????

3.) a buffer solution is 0.333 M in KH2PO4 and 0.248 M in K2HPO4. If Ka for H2PO4^- is 6.2x10^-8, what is the pH of this buffer solution?

pH = ????

Answer 1

Answer :- Given that for one more of O2 (gy, il ne 1 mole, Cum = 2,5R, where R = Rydberg Constant = 8.314 T. ki mor 02 is expand adiabatically from 301 k and 4.00 bar to 1.60 bar, le, Ti = 3014, P = 4 bour, If = 1.60 bar. (ep, m = Com tR/ As, I Cp - Cv = R7 for ideal Cam = 2.58 +2 = 3:58] gas We know that for adiabatic process for an ideal gas,

We know that, [pka = -logra = - log (4.5 x 10-4) > lpka = 3.3 According to the Honderso-Hasseche pH = pka [salt] log a Tared pH = 3.3 + log(0359m => /pH = 3.3 -0.1 = 3.2
So, the PH of the buffer solution is 3.2 .