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rubyeel224Lv1
28 Sep 2019
Part A
Consider a buffer solution that is 0.50 M in NH3 and 0.20 M in NH4Cl. For ammonia, pKb=4.75.â
Calculate the pH of 1.0 L of the original buffer, upon addition of 0.190 mol of solid NaOH.
Part B
A 1.0-L buffer solution contains 0.100 mol HC2H3O2 and 0.100 mol NaC2H3O2. The value of Ka for HC2H3O2 is 1.8Ã10â5.â
Calculate the pH of the solution, upon addition of 0.030 mol of NaOH to the original buffer.
(I will leave a good rating, thank you)
Part A
Consider a buffer solution that is 0.50 M in NH3 and 0.20 M in NH4Cl. For ammonia, pKb=4.75.â
Calculate the pH of 1.0 L of the original buffer, upon addition of 0.190 mol of solid NaOH.
Part B
A 1.0-L buffer solution contains 0.100 mol HC2H3O2 and 0.100 mol NaC2H3O2. The value of Ka for HC2H3O2 is 1.8Ã10â5.â
Calculate the pH of the solution, upon addition of 0.030 mol of NaOH to the original buffer.
(I will leave a good rating, thank you)
Lelia LubowitzLv2
28 Sep 2019