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![QUESTION 1
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Calculate the pH of a solution in which 12.5 g of NH4Cl is added to 100 mL of 1.2 M NH3 solution. Kb = 1.8 x 10-5](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fbf1ef2c8-fbe2-49ff-9ab2-e24f07c3cc20%2F5c982af1-fcd1-4b39-b4fa-c0fcb66a9356%2Fuzyh83_processed.jpeg&w=3840&q=75)
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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=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?Calculate the pH of a solution containing 14.68 g of mandelic acid (152 g/mol) and 20.59 g of sodium mandelate (174 g/mol) in 400 mL solution (Ka=3.88x10-4). Please type answer note write by hend.QUESTION 8 Calculate the pH of a solution formed by mixing 0.2128 L of 1.26 M NH4Cl with 0.5737 L of 2.48 M NH3. The Kb for NH3 is 1.8 × 10-5 Please report with 5 signifigant figures
- 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)Please don't use the 'pH of basic salt' formula as I didn't take it in class What is the pH of a 0.500 mol/L solution of sodium cyanide (NaCN) if the cyanide ion has Kb = 1.61 x 10-5?O 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 =
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