![5. The equilibrium concentrations of the reacting species in the reaction below are CO)-0.50M: [Hs)-0.45M: [CO2]-0.86M and (H20] 0.40 M a calculate Ka for the reaction at 5000 b, if we decrease the CO, concentration to 0.5M; what will the concentrations of all the gases be when equilibrium is reestablished? c. what is the Kp of this system? CO2 (g) + H2 (g) ←→CO (g) + H,O(g) 6. You are conducting a titration of 22 ml ofo.1 M HCI with 0 1 M NaOH How many mi will it take to reach the equivalence point?](http://img.homeworklib.com/questions/50954340-d205-11ea-865c-439827d21f10.png?x-oss-process=image/resize,w_560)
Homework Answers
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.
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5. The equilibrium concentrations of the reacting species in the reaction below are CO)-0.50M: [Hs)-0.45M: [CO2]-0.86M...
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If 0.203 mol of F2 is added to this equilibrium
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5-3 Write the equilibrium constant expression of this reaction and calculate the concentration of all the...
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For the reaction below at a certain temperature, it is found
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If 0.203 mol of F2 is added to this equilibrium
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5-3 Write the equilibrium constant expression of this reaction and calculate the concentration of all the gases at equilibrium for the reaction: CO(g) + H20 (g) = CO2(g) + H2 (g) Given that the initial concentrations of all the gases are 0.05 M and that Kc = 5.1 at 700 K.
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