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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 that is 0.28 M inNa2CO3?


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Deanna Hettinger
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Related questions

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:-)

Carbonic acid is a diprotic acid, H2CO3, with Ka1 = 4.2 × 10^-7 and Ka2 = 4.8 × 10^-11 at 25°C. The ion product for water is Kw = 1.0 × 10^-14 at 25°C. What is the OH– concentration of a solution that is 0.20 M in Na2CO3?

Can i please get all questions answered

1. Add 20.0 mL of .120 M HNO3 to 20.0 mL of .120 M sodium benzoate. What is the pH?

KA of benzoic acid is 6.31 x 10-5

2. Which system would you use to construct a buffer with a pH of 6.50?

(you will need a KA table for this)

I C6H5OH / C6H5O- (phenol / phenolate)

II H2CO3 / HCO3- (carbonic acid / hydrogen carbonate)

III HC2H2O2Cl / C2H2O2Cl- (chloroacetic acid / chloroacetate)

IV H2PO4- / HPO42- (dihydrogen phosphate / hydrogen phosphate)

3. Titrate 26.0 mL .147 M H3C6H5O7 with .0664 M Mg(OH)2. How many mL of titrant are needed to completely neutralize the acid?

4. A titration of 20.0 mL 0.111 M propionic acid (KA = 1.34 x 10-5) requires 31.7 mL to reach the equivalence point. What is the pH of the solution when 22.9 mL of titrant have been added?

5. A titration of 20.0 mL 0.111 M propionic acid (KA = 1.34 x 10-5) requires 31.7 mL to reach the equivalence point. What is the pH exactly 2.00 mL beyond the equivalence point? hint: you will need the concentration of the titrant to do this

6. A sample of 15.0 mL of .100 M oxalic acid (H2C2O4) requires exactly 30.0 mL of NaOH to completely neutralize it. What is the pH of the solution if you only add 15.0 mL of NaOH instead?

7. The value of KW at 20oC is 1.00 x 10-14, but at 50oC it is 5.48 x 10-14. What is the pH of neutral water at 50oC?

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