You have a solution of the three molecules below in a suitable organic solvent. NH₂ OH In addition to the organic solvent and the three molecules, you have access to the following solutions: 1 M NaOH 1 M HCI 1 M CH3COOH 1 M Na2HPO4 Outline a method for how you would separate this solution into its component parts and briefly explain your rationale. You do not need to provide the level of detail shown in the Experimental; just the basics will be sufficient (e.g. wash with ______ to separate component_____, then wash with to separate component Y, etc.). Hint: you might need to search their pką values! You can write in paragraph style or organize your steps in a numbered list.

Suppose a 0.023M aqueous solution of oxalic acid (H₂C₂04) is prepared. Calculate the equilibrium molarity of C₂0. You'll find information on the properties of oxalic acid in the ALEKS Data resource. Round your answer to 2 significant digits. M 0.9 C C 0 E C

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the References to access Important values if needed for this question. What concentration of barlum hydroxide is needed to give an aqueous solution with a pOH of 1.220? Molarity of barlum hydroxide = M Submit Answer 288 R F4 % 5 Show Hint .:: T Retry Entire Group G F5 Cengage Learning Cengage Technical Support ^ 6 9 more group attempts remaining MacBook Air Y H & 881 7 ◄◄ F7 U 8 F8 1 9 F9 O 0 F10 P 4) .. Previous F11 Next 11 Save and Ex 10

What is the pOH of a solution prepared by diluting 208.4 mL of 1.059 M HNO3 (ka>>1) to a total volume of 14.248L? Please report your answer to 3 decimal places.

Q3. This question is about the pH of several solutions. Give all values of pH to 2 decimal places. (a) (i) Write an expression for pH. (b) (ii) Calculate the pH of the solution formed when 10.0 cm³ of 0.154 mol dm-³ hydrochloric acid are added to 990 cm³ of water. The acid dissociation constant, Ka, for the weak acid HX has the value 4.83 x 10-5 mol dm-³ at 25 °C. A solution of HX has a pH of 2.48 Calculate the concentration of HX in the solution. Page 4 of 14

What amount of solid NaOH must be added to 1.0 L of a 0.10 M H2CO3 solution to produce a solution with [H+] = 3.2 * 10 - 11 M? There is no significant volume change as the result of the addition of the solid.

A Dashboard 101 Chem101 + а ap.101edu.co Question 10 of 16 Submit Complete the balanced chemical reaction for the following weak base with a strong acid. In this case, write the resulting acid and base as its own species in the reaction. NH:(aq) + HCI(aq) - 14- O3- |2+ 3+ 14+ 1 2 3 4 7 9. 1 I5 16 (s) (g) (aq) H3O+ H2O OH- CI Reset • x H2O Delete + 10:24 PM P Type here to search 65°F Mostly sunny 10/31/2021 1L

Calculate the concentrations of all species in a 1.01 M Na₂SO3 (sodium sulfite) solution. The ionization constants for sulfurous acid are Kal = 1.4 x 10-2 M and K₁2 = 6.3 x 10-8M. [Na+] = [HSO3] = [OH-] = M [so-] = M [H₂SO3] = M [H+] = M M M

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