Calculate the pH and concentration of CO3^2- in a 0.25 M solution of carbonic acid, H2CO3....

Question

Question

Calculate the pH and concentration of CO3^2- in a 0.25 M solution of carbonic acid, H2CO3. Ka1= 4.4 x 10^-7 Ka2= 4.7 x 10^-11

science chemistry

Answer 1

Answer #1

Answer 2

Similar Homework Help Questions

Find the pH of a 0.100 M carbonic acid (H2CO3) solution. Find the equilibrium concentration of...

Find the pH of a 0.100 M carbonic acid (H2CO3) solution. Find the equilibrium concentration of CO3 -2. Ka1 = 4.30 x 10-7 Ka2 = 5.59 x 10-11
Calculate the pH and the concentrations of all species present (H2CO3, HCO3 – , CO3 2–...

Calculate the pH and the concentrations of all species present (H2CO3, HCO3 – , CO3 2– , H3O + , and OH– ) in a 0.0037 M M carbonic acid solution. Ka1 = 4.3 × 10–7 ; Ka2 = 5.6 × 10–11
Calculate the pH of a 0.30 M carbonic acid solution, H2CO3(aq), that has the stepwise dissociation...

Calculate the pH of a 0.30 M carbonic acid solution, H2CO3(aq), that has the stepwise dissociation constants Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10-11.

You create a 1 L solution of 0.1 M H2CO3. carbonic acid, H2CO3, is a diprotic...

You create a 1 L solution of 0.1 M H2CO3. carbonic acid, H2CO3, is a diprotic acid with Ka1 = 4.5 x 10-7 and Ka2 = 4.7 x 10-11. a) What will the initial pH of the solution be? b) What volume of 0.1 M NaOH will you need to add to reach the second equivalence point( remember carbonic acid deprotonates to bicarbonate HCO3- and then can deprotonate further to CO32-? c) At the second equivalence point, what will the...
What is the pH of a 0.10 M solution of carbonic acid? Carbonic acid, H2CO3 has...

What is the pH of a 0.10 M solution of carbonic acid? Carbonic acid, H2CO3 has two acidic protons: H2CO3 + H2O7 HCO3 + H30+ Ka1 = 4.3x10-7 HCO3 + H202 CO32- + H30+ Ka2 = 5.6x10-11 a) 1.00 b) 0.70 c) 6.37 d) 3.68 e) I still can't figure this out...
For 0.045 M H2CO3, calculate [H30+],[HCO3],[CO3^-2], given Ka1= 4.4 x 10^-7 and Ka2= 4.7 x 10^-11.

For 0.045 M H2CO3, calculate [H30+],[HCO3],[CO3^-2], given Ka1= 4.4 x 10^-7 and Ka2= 4.7 x 10^-11.

Calculate the pH of a 0.01 M carbonic acid, H2CO3, solution, given Kal = 4.3 x...

Calculate the pH of a 0.01 M carbonic acid, H2CO3, solution, given Kal = 4.3 x 10-7, and Ka2 = 5.2 x 10-11. Test your approximation.
Determine the pH of a 0.18 M H2CO3 solution. Carbonic acid is a diprotic acid whose Ka1 = 4.3 ×...

Determine the pH of a 0.18 M H2CO3 solution. Carbonic acid is a diprotic acid whose Ka1 = 4.3 ×10-7 and Ka2 = 5.6 × 10-11.10)A) 10.44 B) 5.50 C) 4.31 D) 11.00 E) 3.56
Carbonic acid, H2CO3 is a diprotic acid with Ka1 = 4.3 x 10-7 and Ka2 =...

Carbonic acid, H2CO3 is a diprotic acid with Ka1 = 4.3 x 10-7 and Ka2 = 5.6 x 10-11. What is the pH of a 0.47 M solution of carbonic acid?

a) Find the concentration of H+, HCO3- and CO32-, in a 0.01M solution of carbonic acid...

a) Find the concentration of H+, HCO3- and CO32-, in a 0.01M solution of carbonic acid if the pH of this is 4.18. Ka1 (H2CO3) =4.45 x 10–7 and Ka2 =4.69 x 10–11 (b) Calculate the pH at the equivalence point of the titration between 0.1M CH3COOH (25 ml) with 0.05 M NaOH. Ka (CH3COOH) = 1.8 x 10–5.