Where\[K_{a1} = 4.20 \times 10^{-7} \\K_{a2} = 4.69 \times 10^{-11}\](a) **Calculate the fraction \(H_2CO_3, HCO_3^-, CO_3^{2-}\)** - use the following table as your template.(b) **Plot \(pH\) vs. fraction of \(H_2CO_3, HCO_3^-, CO_3^{2-}\)** using the plotting guidelines all on the same chart.\[\begin{array}{ccccc}\text{pH} & [H^+] & \alpha_{H_2CO_3} & \alpha_{HCO_3^-} & \alpha_{CO_3^{2-}} \\\hline1.806 & 6.739 \\2.020 & 6.954 \\2.235 & 7.168 \\2.449 & 7.383 \\2.664 & 7.598 \\2.878 & 7.812 \\3.093 & 8.027 \\3.307 & 8.241 \\3.522 & 8.456 \\3.736 & 8.670 \\3.951 & 8.885 \\4.165 & 9.099 \\4.380 & 9.314 \\4.594 & 9.528 \\4.809 & 9.743 \\5.023 & 9.957 \\5.238 & 10.172 \\5.452 & 10.386 \\5.667 & 10.601 \\5.881 & 10.815 \\6.096 & 11.030 \\6.310 & 11.244 \\6.525 & 11.459 \\5.881 & 11.673 \\6.096 & 11.888 \\6.310 & 12.102 \\6.525 & 12.317 \\\end{array}\]

Answered: Image /qna-images/answer/0c71a5fe-4586-472b-89e1-884406cbdd1c.jpg

Where (a) Calculate the fraction H₂CO3, HCO3, CO3², use the following table as your template. (b) Plot_p¹ vs. fraction of H₂CO3, HCO³, CO² using the plotting guidelines all on same chart. pH [H] “H,co, Kal = 4.20 x 10-7 Ka24.69 x 10-¹1 1.806 2.020 2.235 2.449 2.664 2.878 3.093 3.307 3.522 3.736 3.951 4.165 4.380 4.594 4.809 5.023 5.238 5.452 5.667 5.881 6.096 6.310 6.525 α an,co, ancoraco α 6.739 6.954 7.168 7.383 7.598 7.812 8.027 8.241 8.456 8.670 8.885 9.099 9.314 9.528 9.743 9.957 10.172 10.386 10.601 10.815 11.030 11.244 11.459 11.673 11.888 12.102 12.317 12.531

Where (a) Calculate the fraction H₂CO3, HCO3, CO3², use the following table as your template. (b) Plot_p¹ vs. fraction of H₂CO3, HCO³, CO² using the plotting guidelines all on same chart. pH [H] “H,co, Kal = 4.20 x 10-7 Ka24.69 x 10-¹1 1.806 2.020 2.235 2.449 2.664 2.878 3.093 3.307 3.522 3.736 3.951 4.165 4.380 4.594 4.809 5.023 5.238 5.452 5.667 5.881 6.096 6.310 6.525 α an,co, ancoraco α 6.739 6.954 7.168 7.383 7.598 7.812 8.027 8.241 8.456 8.670 8.885 9.099 9.314 9.528 9.743 9.957 10.172 10.386 10.601 10.815 11.030 11.244 11.459 11.673 11.888 12.102 12.317 12.531

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

In order to determine the Ka of HXO₂, a scientist prepared a HXO₂ solution with a pH=3. If the scientist determined the Ka to be 1.2 X 10⁻⁵, what was the molarity of the acid he started with? (If you use any assumptions, be sure to check that they are valid!) Round the final answer to the three decimal places.
can you help me on the second problem please
Morphine (C17H1903N) is very effective at relieving intense pain. Calculate the pH of a 0.00115 M solution of morphine. Kp = 8.0 x 10- (the answer should be entered with 3 significant figures; do not enter units; give answer in normal notation--examples include 1.23 and 120. and -123 and 123. and 12.3) MacBook Pro >) esc @ # & 1 3 4 7 8 Q W E R T. Y A S H J K C V option cоmmand command option .. .. V * 00
Construct the expression for Ka for the weak acid, NH4+. 1 Based on the definition of Ka, drag the tiles into the numerator or denominator to construct the expression for the given acid. [H₂O] 2[OH-] [NH3]² NH.(aq) + H2O(I) = HO-(aq) + NH3(aq) [H3O+] 2[NH] [NH₂-]² Ka = [OH-] 2[NHs] [NH] 2[NH₂] [NH3] [H₂O]² [NH₂-] [H3O+]² 2[H₂O] [OH-]² ✓ RESET 2[H3O+] [NH
Consider the following data on some weak acids and weak bases: acid base Ka name formula name formula HNO, 4.5 x 10 CgH;NH2|4.3 × 10 - 10 -4 nitrous acid aniline 4 -8 hydrofluoric acid HF 6.8 × 10 hydroxylamine HONH, 1.1 x 10 Use this data to rank the following solutions in order of increasing pH. In other words, select a '1' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. solution pH 0.1 M HONH3CI choose one v 0.1 M Nal choose one v 0.1 M KNO2 choose onev 0.1 M NaF choose one v
< 10:14 1 4 7 A diprotic acid, H₂A, has Ka1 = 3.4 x 10-4 and Ka2 = 6.7 x 10-⁹. What is the pH of a 0.27 M solution of H₂A? +/- 2 Question 16 of 20 5 8 3 6 9 O Tap here or pull up for additional resources Submit 97 X с x 100
Calculate the pH of the mixture of 105 mL of 0.195 mol/L hydrazine (H2NNH2) with 95 mL of a 0.215 mol/L H2NNH3Br solutionGive an answer to at least 3 decimal places. Next, calculate the pH of this same solution if 12.00 mL of 0.300 mol/L HNO3 is added.Give an answer with at least 3 decimal places.
What is the concentration of H3O+ in a solution that is 0.0600 M Hypochlorous acid (HClO)? What is the pH? To solve this problem: Write the acid dissociation equilibrium for HClO Set up an ICE chart ( with x = the concentration of H3O+ at equilibrium) Write the expression for Ka. Fill this in with the concentrations of H3O+, ClO- and HClO at equilibrium, in terms of x. Decide if x can be neglected. You may neglect x if the initial concentration of the HClO is greater than 100 times the Ka. You will need the value of Ka. Look it up on the chart (p 4 of packet) Solve for x Find the pH The pH of a 0.0200 M solution of an unknown acid is 2.56. What is the Ka of this acid? To solve this problem: Write the acid dissociation equilibrium for the generic aicd “HA” Set up an ICE chart ( with x = the concentration of H3O+ at equilibrium) Write the expression for Ka. Fill this in with the concentrations of H3O+, A- and HA at equilibrium, in terms of x. What is x? Can you find it…
Complete the following table. Be sure to show each calculation in detail.
Find the H3O+H3O+ concentration of a 0.220 MM hypochlorous acid solution (whose acid dissociation constant is Ka=2.9×10−8Ka=2.9×10−8). Express the concentration to two significant figures.
Please help me
G The pH of a 0.66M solution of hydrocyanic acid (HCN) is measured to be 4.69. Calculate the acid dissociation constant K of hydrocyanic acid. Round your answer to 2 significant digits. K₁ = [] a x10