When 22.6 mL of 0.229 M hydrochloric acid (HCI) and 22.6 mL of 0.229 M ammonia (NH3) are combined, what will be the pH value of the mixture? (Kp of NH3 = 1.8 x 10, Ka x Kh = Kw for conjugate acid-base); Please keep your answer to two decimal place X.Xx.

What mass of aluminum hydroxide can be dissolved in a solution whose pH is held at 11.20? (Ksp of aluminum hydroxide = 1.9x10^-33)

What is the pH of a solution prepared by adding 60.4 g ethylammonium chloride (C2H5NH3CI, 81.55 g/mol) to 1.00L of a 0.300 M aqueous solution of ethylamine (C2H5NH2, 45.08 g/mol, Kp = 4.3 x 104 at 25°C)? Enter your answer in decimal format with two decimal places (value + 0.02).

Propanoic acid (CH3CH2COOH) has a Ka of 1.3×10–5.FW(propanoic acid) = 74.08 g/mol; FW(calcium propanoate) = 186.22 g/mol a) At what pH will a solution of propanoic acid and sodium propanoate best resist changes to its pH? How do you know? b) 75 g calcium propanoate Ca(CH3CH2COO)2 is diluted to 150.0 mL with deionized water. 50.0 mL of a 3.0 M propanoic acid solution is added. Determine the equilibrium concentrations of each species and the pH of the resulting solution.

A 0.500 L solution is composed of 0.200 M (CH3)2NH and 0.200 M (CH3)2NH₂Cl at 25 °C. What is the pH of the solution after 0.040 moles of HBr are added to the solution at the same temperature? You may assume no change in volume for the system. Enter your answer with two decimal places. At 25 °C: Kb for (CH3)₂NH = 5.9 x 10-4 Kb for KOH= 3.2 x 10¹

A solution is made by mixing 185 mL of 0.100 M formic acid (Ka = 1.7 x 10-4 ) with 190. mL of 0.100 M sodium formate. What is the pH of the solution? Express your answer in decimal notation rounded to three significant figures.

A solution is prepared at 25 °C that is initially 0.69M in dimethylamine ((CH3)2NH), a weak base with K = 5.4 × 10-4, and 2.4M in dimethylammonium ((CH3)2NH₂CI). Calculate the pH of the solution. Round your answer to 2 decimal places. chloride pH = ☐

A solution is prepared at 25 °C that is initially 0.15M in propanoic acid (HC₂H-CO₂), a weak acid with K=1.3 × 105, and 0.18M in potassium propanoate (KC₂H,CO₂). Calculate the pH of the solution. Round your answer to 2 decimal places. pH = 0 X S

8. You will perform some calculations to see the difference between a pH buffer solution and a weak acid solution of the same pH when a small amount of strong base is added. Chlorous acid, HC1O₂, is a moderately strong acid with a Ka = 1.110×10-². Please answer the following questions. A. B. What is the molarity of the HClO₂ solution whose pH is 2.21? Please provider your answer below. 미ㄷ → Please provider your answer below. f A $ To prepare a buffer solution of the same pH, what is the molarity of the NaClO₂ if the molarity of the HC1O₂ is 0.6771 M? M → M → $

What is the pH of a solution that is 0.21 M CH3NH2 (methylamine) and 0.31 M CH3NH3Cl (methylammonium chloride)? (Assume Kw is 1.0 ✕ 10−14.)