1. Youhave a 250 mL sample of 1.62 M acetic acid (Ka= 1.8x10^-5).Calculate the pH of the best buffer. Determine the concentrationsof components needed to make a solution that could resist (<0.5pH change) the addition of 0.15 mol of a strong acid orbase.
2.Carbonic acid is a diprotic acid, H2CO3, with Ka1=4.2x10^-7 and Ka2= 4.8x10^-11 at 25 degrees. The ion product forwater is Kw= 1.0x10^-14 at 25 degrees. What is the OH-concentration of a solution tha tis 0.28 M inNa2CO3?
3. A titration of 200 mL of 1.00 MH2A was done with 1.16 M NaOH. For the diprotic acid H2A, Ka1=2.50x10^-5, Ka2= 3.10x10^-9. Calculate the pH after 600 mL of 1.16M NaOH have been added.
4. 15.0 mL of 0.50 M NaOH is addedto a 100 mL sample of 0.430 M NH3 (Kb for NH3= 1.8x10^-5). What isthe equilibrium concentration of NH4+ ions?.....and NH4?.....andpH?
Step bystep to get full answer....I want to make sure I am working theseproblems correctly...best, most clear and concise answer gets fullpoints... feel free to dumb it down:-)
1. Youhave a 250 mL sample of 1.62 M acetic acid (Ka= 1.8x10^-5).Calculate the pH of the best buffer. Determine the concentrationsof components needed to make a solution that could resist (<0.5pH change) the addition of 0.15 mol of a strong acid orbase.
2.Carbonic acid is a diprotic acid, H2CO3, with Ka1=4.2x10^-7 and Ka2= 4.8x10^-11 at 25 degrees. The ion product forwater is Kw= 1.0x10^-14 at 25 degrees. What is the OH-concentration of a solution tha tis 0.28 M inNa2CO3?
3. A titration of 200 mL of 1.00 MH2A was done with 1.16 M NaOH. For the diprotic acid H2A, Ka1=2.50x10^-5, Ka2= 3.10x10^-9. Calculate the pH after 600 mL of 1.16M NaOH have been added.
4. 15.0 mL of 0.50 M NaOH is addedto a 100 mL sample of 0.430 M NH3 (Kb for NH3= 1.8x10^-5). What isthe equilibrium concentration of NH4+ ions?.....and NH4?.....andpH?
Step bystep to get full answer....I want to make sure I am working theseproblems correctly...best, most clear and concise answer gets fullpoints... feel free to dumb it down:-)
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