How do I calutatle the Kb and Ka values from a measured pH for the following:
1.0 M solution of NH4C2H3O2 with the pH of 7.05
1.0 M solution of Na2CO3 with the pH of 11.66
Please show work, thank you.
How do I calutatle the Kb and Ka values from a measured pH for the following: 1.0 M solution of N...
Consider 1.0 L of a solution which is 0.45 M HF and 0.2 M NaF (Ka for HF = 7.2 x 10-4). Assume 2 significant figures in all of the given concentrations so that you should calculate all of the following pH values to two decimal places. Calculate the pH after 0.10 mol of HCl has been added to the original solution. Assume no volume change on addition of HCl. Why do we need to convert to Kb? I know...
Calculate ka or kb from experimental data. The pH of a 8.7x10-2-M solution of maleic acid (H,C H204) is measured to be 1.52. Use this information to determine a value of K, for maleic acid. H2C4H204(aq) + H2O(1) P HC4H204 (aq) +H30*(aq) Ka=
What is the pH of a 0.10M solution of methylamine (:NH2CH3) From Table 15.8, Kb = 4.4 x 10-4. Please show me how to work it out, thank you!
QUESTION 3 2 pointsSave Answer Calculate the pH of the following solution, using Ka and/or Kb values: 0.100 M CH3 NH3CI
Calculate the PH of a 0.36 M aqueous solution of NH4NO3. Kb of NH3= 1.8 x10^-5. Please show your work; I know how to do a normal problem but I am confused because the Kb is only for NH3, not the whole thing. Thanks!
I need help with number 14, 15 , and 16 please! I also provided information in order to solve the problem, but I dont know how to do that. thank you! We were unable to transcribe this imageJ. Uly the experimental data for pH and the concentration of the solutions, calculate the k WORK.) Solution Value of K, or kb 0.1 ZnCl2 Ko= 9.0x10-17 0.1 KAI(SO4)2 Kb = 1.44x10-20 0.1 NH4Cl Ka = 3.80 x 10-9 0.1 NaC H302 Ko=...
Using tabulated Ka and Kb values, calculate the pH of the following solutions. Answer to 2 decimal places. A solution containing 3.1x101 M HF and 4.6x101 M NaF. For HF, Ka 7.2x10-4 Submit Answer Tries o/s 1000.0 mL of solution containing 23.0 g of HOCI and 45.0 g of NaoCI For Hoci, Ka-3.5x10-8 Submit Answer Tries o/s A solution made by mixing 135.00 mL of 1.100 M HOBr with 50.00 mL of 1.000 M NaOH. For HOBr, Ka-2.0×10-9. Submit Answer...
Calculate the pH of each of the following solutions (Ka and Kb values are given in Appendix D in the textbook). 9.0×10−2 M propionic acid (C2H5COOH). 0.100 M hydrogen chromate ion (HCrO−4). 0.119 M pyridine (C5H5N).
11. a) The pH of 0.015 M HNO2(aq) was measured as 2.63. What are the values of Ka and pKa of nitrous acid? b) The pH of 0.10 M butylamine, CaH,NH2(aq) was measured as 12.04. What are the percentage protonation and the values of Kb and pkb of butylamine?
How do I do this without being give Kb or Ka? Please walk me through the steps Question 8 O out of 1 points Calculate the pH during the titration of 24 mL of 0.22 M HCl with 0.17 M KOH after 11 ml of the base have been added Selected Answer: Correct Answer: [None Given) 1.01 +0.02