S20 Ch17 Sec5-6 17 Multiple Choice Question 39 Part A Determine the [H3O+] concentration for a 0.200 M solution of HCI. 4.00 x 10-1 M 1.00 x 10-1 M 1.25 x 1014 M 2.50 x 10-14 M 2.00 x 101 M Submit Request Answer Provide Feedback
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- In the laboratory, a general chemistry student measured the pH of a 0.589 M aqueous solution of phenol (a weak acid), C6H5OH to be 4.997. Use the information she obtained to determine the K₂ for this acld. Ka(experiment) = Submit Answer $ 4 R LL F F4 % 5 A T Retry Entire Group 9 more group attempts remaining G Cengage Learning Cengage Technical Support F5 A 6 MacBook Air S Y H & 7 ◄◄ F7 U J * 00 8 ► 11 F8 L ( 9 K F9 O 1 0 L F10 P 4) Previous Next F11 + = Save and F12 8light data and DID NOT round any intermediate calculations. In a 3.8M aqueous solution of benzoic acid (C6H, CO₂H), what is the percentage of benzoic acid that is dissociated? You can find some data that is useful for solving this problem in the ALEKS Data resource. Round your answer to 2 significant digits. 7.0 % GEE olaCHE154-H KCHE154 S20 Ch17 Sec5-6 Chapter 17 Multiple Choice Question 41 Part A Find the percent ionization of a 0.337 M HF solution. The K, for HF is 6.8 x 104. O4.5 % 1.5 % 6.5% 2.3 x 102 % 6.8 x 102 % Submit Request Answer Provide Feedback
- INTRODUCTION LABORATORY SIMULATION 1) Calculate the pH of a solution prepared by dissolving 2.35 g of sodium acetate, CH3COONa, in 78.0 mL of 0.10 Macetic acid, CH;COOH(aq). Assume the volume change upon dissolving the sodium acetate is negligible. Ka of CH3COOH is 1.75 x 10-5. pH E METHODS O RESET P MY NOTES A LAB DATA SHOW LABELSpH Measurement Experiment 1. Objectives: Explore different methods of measuring ph II. Materials: water window cleaner pH meter apple juice 0.1 M NaCl pH paper milk 0.1 M FeCl₂ litmus paper red/blue III. Results and Observations Red litmus paper water apple juice milk window cleaner 0.1 M NaCl 0.1 M FeCl3 IV. Conclusion Blue litmus paper Acidic/basic/neutral PHTrial 1: Initial pH= 3.92mL Mass of KHP and Paper= 0.868g Mass of paper= 0.357g Mass of KHP= 0.511g Trial 2: Initial pH= 4.09ml Mass of KHP and Paper= 0.870g Mass of paper= 0.359g Mass of KHP= 0.511g 1) find Ka and use the value of Ka to calculate the initial pH of each trial 2) calculate Kb for the C8H4O4^-2 anion from the value of Ka that you obtained for KHP.
- nment Score: 77.9% Resources O Hint cion 17 of 28> Each value represents a different aqueous solution at 25 °C. Classify each solution as acidic, basic, or neutral. Acidic Basic Neutral H* = 1.0 x 10-7 pH = 8.39 pOH = 7.00 Answer Bank H|= 5.0 x 10 H| = 35 x 10 POH = 5 34 POH= 10.32 JOH= 89 x 10- JOH = 90 x 10 pH = 5 50 & mWrite the net ionic equation for the acid-base hydrolysis equilibrium that is established when potassium cyanide is dissolved in water. Ac + H20(t) This solution is 16. Submit Answer Retry Entire Group 9 more group attempts remaining red Pred 3rec Visited 2red 2red 2red 2red 5 at (Previous Next Save and Exit nment Cengage Learning | Cengage Technical Support O Focus MacBook Air DII DD 80 888 F8 F9 F6 F7 F3 F4 F5 F1 F2 ! @ 2$ & 4 7 1 Q W E R T Y U. K * 00Based on the results obtained in the following table, which indicator has approximately a pka of 4? Acid-base Color Standards Sample indicator A Y Y Y Y Y Y Y Y Y Y R R R Y Y Y Y Y Y Y C В В В V R R R R Y Y Y C C C C C C C C R R R C pH 3. 4 5 7 8 9 10 11 12 13 14 LEGEND: R-red Y-yellow 0-orange B-blue V-violet C-colorless P-pink A R 1. B.
- 4. The pH of 1.50 mol/L acid is measured to be 5.75. For this acid, the Ka is 10-5.25 = [H₂₂0] A. 2.1 x 10-¹2 B. 1.8 x 10-6 C. 2.4 x 10-6 D. very large Chatz (H30] = 1.77x10-6 = 1,8x10-6 In the following information to answer the next question.5. a) The Kw value that we normally use is for room temperature (25°C). Calculate the equilibrium H+ concentration and pH of pure, neutral water at 0.0°C (Kw= 1.14 x 10-15at 0.0°C) b) Methylamine (CH3NH2) is a derivative of the weak base ammonia. Write the equation for the ionization of methylamine in water, and use the I.C.E. method to find the pH of a 3.75 M CH3NH2 solution.(Kb= 4.37 x 10-4at 25°C)What is the pH of a solution containing 1.053 mol L-1 of a diprotic acid with PKA1 = 3.93 and pKA2 = 7.88 ? H2A + H 20H3O++ HA-pkA1 HA- + H2O H3O++ A2-pkA2 Report your answer to at least 1 decimal place.