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- Calculate the pH of 0.750 M pyridinium chloride, C5H5NHCl? Given Kb of C5H5N is 1.70×10-9.4. Calculate the pH of a 0.340 M NaO₂CCO₂H solution. pK₁ = 1.250 and pK2 = 4.266. Please type answer not write by hendCan someone help me with the problem below? CH3NH2 is a weak base (Kb=5.0×10−4), so the salt CH3NH3NO3 acts as a weak acid. What is the pH of a solution that is 0.0490 M in CH3NH3NO3 at 25 ∘C?
- Hydroxylamine, HONH2, readily forms salts such as hydroxylamine hydrochloride which are used as antioxidants in soaps. Hydroxylamine has Kb of 9.1 × 10–9. What is the pH of a 0.054 M HONH2 solution? Please report 2 decimal places.The Kb of (CH3)3N is 6.4x10^-5. What is the pH of a 0.48 M solution of (CH3)3NH+?For a 0.0359 M aqueous solution of cyanic acid, HCNO (Ka = 3.5*10-4), determine the following. What are the major and minor species present? Include phase. What is the major species (other than water)? What is the concentration of the minor species in the solution? What is the concentration of the major species in the solution? What is the concentration of H3O+ in the solution? What is the concentration of OH- in the solution? Find the pH.
- The pH of 8.35 is wrong, but I'm not sure how to get the right answerThe Kb value for ammonia is 1.8 × 10–5 . Determine the pH and the concentration of [OH– ] in a 0.40 M solution of ammonia? pH: [ H+] : pls explain why the answer is this. Pls refer to the picDetermine the pH and the type of solution of a 0.227 g/L C5H5N solution at 25°C. The Kb of C5H5N is 1.7 × 10-9.
- . Morphine is a weak base for which Kb is 8 × 10-7 . Calculate the pH of a solution made by dissolving 0.0400 mol of morphine in water and diluting to 600.0 mL.3)CH3NH2 is a weak base (?b = 5.0×10-4), so the salt CH3NH3NO3 acts as a weak acid. What is the pH of a solution that is 0.0450M CH3NH3NO3 at 25oC?What is the Ph of a 0.23 M triethylamine (C2H5)3N solution? Kb for triethylamine is 5.3 x 10^-4. Report 2 decimal places.