Write the first and second dissociation reactions and the Ka equations of each for carbonic acid, H2CO3. Ka1 = 4.4 × 10^–7 Ka2 = 4.7 × 10^–11
1)
H2CO3(aq) + H2O(l) <->
HCO3-(aq) +
H3O+(aq)
Ka1 = [HCO3-][H3O+]/[H2CO3]
2)
HCO3-(aq) + H2O(l) <->
CO32-(aq) +
H3O+(aq)
Ka2 = [CO32-][H3O+]/[HCO3-]
Write the first and second dissociation reactions and the Ka equations of each for carbonic acid,...
Calculate the pH and percent dissociation of 0,25 M NH3, Ks- 1.8*10 8. Write the first and second dissociation reactions and the K, equations of each for carbonic acid, H2CO3. Kai -4.4 x 10- Ka) = 4.7 x 10-" 9. Classify the following salts as acidic, basic or neutral: (a) NaNO2 (b) NHACI (c) KF (d) KNO3 (e) NHC2H302 10. What is the pH of 0.35 M NH4Cl (salt solution)? Ks for ammonia (NH3) - 1.8 x 10-
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...
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?
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.
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
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
Hydrosulfuric acid, H2S, has two acid ionization constants. Write equations that correspond to each Ka value. Include states of matter in your answer. Click in the answer box to open the symbol palette. Ka1 = 8.9 × 10−8 Ka2 = 1.0 × 10−19
Given the set of reactions below, combine the first two equations and then model the system resulting from the resulting two reactions as if it were a diprotic acid system. Include a fractional composition plot of the α of species CO2 (aq), HCO3 – (aq) and CO3 2– (aq) as a function of pH. CO2 (aq) + H2O ⇄ H2CO3(aq) H2CO3(aq) + H2O ⇄ HCO3 – (aq) + H3O+ HCO3 – (aq) + H2O ⇄ CO3 2– (aq) + H3O+...
Write the balanced chemical equilibrium equations for both ionizations of 0.150M carbonic acid 1st ionization (Ka,1 = 4.3 x 10^-7): 2nd ionization (Ka,2 = 4.8 x 10^-11):