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- Question 3 :We have 500.0 mL of a buffer solution that is 0.633 M in NH3 and 0.332 M in NH4Cl. We add 500.0 mL of a solution 0.234 M in HCl. The final volume is 1.0000 L. The Kb value for NH3 is 1.8 x 10-5. What is the pH of the final solution?Question 20 Calculate the pH of a buffered aqueous solution consisting of 0.07 M Li₂HPO4 and 0.085 M Li3PO4. The K₂ for HPO42- is 4.84 x 10-13. Enter your answer with 1 digit after the decimal. pH=b My Questions | bartleby X اساسيات كيمياء تحليلية + What is the pH of a solution prepared by dissolving 1.00 g of the weak acid HA (molar mass = 138.95 g/mol, ka = 2.05 X 10-3) in 50.0 mL of 0.113 M NAOH and diluting the mixture to 500 mL? 1. 03.25 2. O2.04 3. 05.58 4. 06.41 5. 02,52
- a) What is the pH of a solution prepared by adding 11.1 mL of 0.50 M NaOH solution to 200. mL of a solution which is 0.40 M in NH4+ and 0.40 M in NH3? The Kb of NH3 is 1.8 x 10-5. The correct answer should be reported to two places past the decimal. b) Caculate the pH of a solution prepared by mixing 84.7 mL of a 0.25 M aqueous aniline solution (C6H5NH2, Kb = 4.3 x 10-10) with 100. mL of a 0.11 M aqueous nitric acid solution. Your pH should be reported to two places past the decimal point.Question 3:We have 500.0 mL of a buffer solution which is 0.663 M NH3 and 0.328 M NH4Cl. Add 500.0 mL of a 0.250 M HCl solution. The final volume is 1.0000 L. The Kb value for NH3 is 1.8 x 10-5. What is the final pH of this solution?0.185 M in HCHO2 (Ka = 1.8 ×x 10-4) and 0.230 M in HC2H3O2 (Ka = 1.8 × 10-5) Express your answer to two decimal places. ? Find the pH of each mixture of acids. pH = 2.11 Submit Previous Answers Request Answer X Incorrect; Try Again; 3 attempts remaining In a mixture of two acids that have similar K, values, the dissociation of one acid affects the dissociation of the other acid, and vice versa. Prepare two ICE tables (where I means initial, C means change, and E means equilibrium), one for the dissociation of HCHO2 and one for the dissociation of HC2H3O2. Use the given acid-dissociation constants to calculate the amount of H3O+ produced by each acid in the pair. Part D 6.00x10-2 M in acetic acid (Ka = 1.8 × 10-5) and 6.00×102 M in hydrocyanic acid (Ka = 4.9 × 10-10) Express your answer to two decimal places. ? pH =
- Please chose one of the following two questions and answer 5) What are the [H.0] and pH of 0.085M weak base C:H&NH2? 6) What is the pH of an aqueous solution that is 0.1M NH.CI? The Kb value for NH3 is 1.8 x 10 (Hint: Decide which ion can hydrolyze)What is the pH of the solution 0.12M NH4OH with Kb = 1.8 × 10-⁵ How much will the pH of the solution become when we add 2.2 grams of NH4Cl to 250 ml of solution?1. Calculate the pH of 2.8 x 10^-4 M Ba(OH)2. 2. Calculate the pH of a 0.26 M methylamine solution. Kb = 4.4 x 10^-4 3.Calculate the pH of an aqueous solution containing the following: (a). 0.80 M lactic acid and 0.40 M lactate ion (Ka of lactic acid = 1.38 x 10^-4) (b). 0.30 M NH3 and 1.50 M NH4+ (Kb of NH3 = 1.8 x 10^-5)
- Question 3 Calculate the pH of a solution that is 0.350 M in the weak acid HA (K = 3.88×106) and 0.150 M in A. Type m 10 po pHO ADVANCED MATERIAL 0/5 Calculating the pH of a buffer A solution is prepared at 25 °C that is initially 0.49 M in diethylamine ((C,H5),NH), a weak base with K = 1.3 × 10 °, and 0.36M in diethylammonium bromide ((C,H5), NH,Br). Calculate the pH of the solution. Round your answer to 2 decimal places. pH =Question 9 What is the pH when 24.8 mL of 0.10 M NaOH is added to 25 0 mL of 0.35 M HNO2? (Ka = 4 0 10-4) Report your answer to two decimal places A Moving to another question will save this response.