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
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Find the pH of a 0.100 M carbonic acid (H2CO3) solution. Find the equilibrium concentration of...
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...
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.
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...
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 = 5.6 x 10-11. What is the pH of a 0.47 M solution of carbonic acid?
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 0.01 M carbonic acid, H2CO3, solution, given Kal = 4.3 x 10-7, and Ka2 = 5.2 x 10-11. Test your approximation.
Find the pH of a 0.225 M ascorbic acid (H2C6H6O6) solution. Find the equilibrium concentration of C6H6O6 -2. Ka1 = 8.01 x 10-5 Ka2 = 1.59 x 10-12
12. Calculate the pH and the concentration of all species in solution of 0.33 M K2CO3. For carbonic acid Ka1 = 4.3 x 10-7 and Ka2 = 5.6 x 10-11
Use the following chemical reaction a 6.8X1l0^-3 solution of carbonic acid: H2CO3 (aq) +H2O (l) <-> HCO3 (aq) + H3O . Ka1= 4.3x10^-7 . Ka2= 4.7x10^-11 a. if you add NaHCO3 to the solution, would the pH of the solution go up, down, or stay the same? b. Calculate the pH of the solution if you added 3.4 x10^-3 M NaHCO3.