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- The pH of an aqueous solution of 0.532 M hydrofluoric acid, ( K₂ (HF) = 7.20 × 10-4) isThe active ingredient of bleach such as Clorox is sodium hypochlorite (NaClO). Its conjugate acid, hypochlorous acid (HClO), has a Ka of 3.0 × 10^–8. (a) The undiluted bleach contains roughly 1 M NaClO. Calculate the pH of 1 M NaClO solution. (b) Some applications require extremely diluted bleach solution, such as swimming pools. Suppose the solution in (a) is diluted by 10,000 -fold. Calculate the pH of the diluted solution, and demonstrate that you can still neglect the autoionization of water in your calculation. (c) Suppose the solution in (a) is diluted by 1 million-fold, briefly explain how your approach will be different. Write the equation with [H3O+] as the unknown, but you do not need to solve it.The hydroxide ion concentration of an aqueous solution of 0.532 M phenol (a weak acid), C,H;OH, is [OH] = M.
- The amino acid asparagine has ionization constants Kal = 6.92 x 10-3 and K ₁2 = 6.92 x 10-3 and K₁2 = 1.86 x 10-9, which correspond to the carboxylic acid group and the amino group respectively. Calculate the pH of a 0.170 M asparagine (HN) solution. pH =The value of K₂ for nitrous acid is 4.50×10-4. What is the value of K₁, for its conjugate base, NO₂? ||Estimate the pH of 0.05 M NaCN(aq) at 25°C. Ka(HCN) = 3.4 × 10−9. Write your answer with two decimal places
- The pH of an aqueous solution of 0.522 M benzoic acid, C6H5COOH isThe pH of an aqueous solution of acetic acid (CH3COOH) is 2.0. What is the initial molar concentration of CH3COOH, if its acid ionization constant is Ka = 1.8×10–5?Determine the pH of a 1.497 M solution of potassium cyanide (KCN) in water. Ka for HCN is 6.17 × 10–10. Enter your response in pH units to the nearest 0.01.