7) pH = pka + log(ch3coona/ch3cooh)
no of mol of ch3cooH = 40*0.1 = 4 mmol
no of mol of ch3cooNa = 10*0.2 = 2 mmol
pka of ch3cooh = 4.74
pH = 4.74+log(2/4)
= 4.44
8) [H+] = 1.9*10^-3 M
pH = -log(1.9*10^-3)
= 2.72
answer: a.acidic
9) answer: d.all of these.
10. answer: b.bronsted acids.
5. The equilibrium concentrations of the reacting species in the reaction below are CO)-0.50M: [Hs)-0.45M: [CO2]-0.86M...
Consider the following equilibrium process at 686°C: CO2(g) + H2(g) ⇌ CO(g) + H2O(g) The equilibrium concentrations of the reacting species are [CO] = 0.0580 M, [H2] = 0.0430 M, [CO2] = 0.0830 M, and [H2O] = 0.0370 M. (a) Calculate Kc for the reaction at 686°C. (b) If we add CO2 to increase its concentration to 0.460 mol / L, what will the concentrations of all the gases be when equilibrium is reestablished? CO2: M H2: M CO: M...
Consider the following equilibrium process at 686 ° C: CO2(g) + H2(g) ⇌ CO(g) + H2O(g) The equilibrium concentrations of the reacting species are [CO] = 0.0480 M, [H2] = 0.0400 M, [CO2] = 0.0880 M, and [H2O] = 0.0430 M. (a) Calculate Kc for the reaction at 686 ° C. (b) If we add CO2 to increase its concentration to 0.510 mol / L, what will the concentrations of all the gases be when equilibrium is reestablished? CO2: M...
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For the reaction below at a certain temperature, it is found that the equilibrium concentrations in a 5.05-L rigid container are [H2] = 0.0523 M, [F2] = 0.0121 M, and [HF] = 0.450 M. H2(g) + F2(g) 2 HF(g) If 0.203 mol of F2 is added to this equilibrium mixture, calculate the concentrations of all gases once equilibrium is reestablished.
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