Calculate the pH of a solution made by dissolving 26.5 g potassium acetate in 150 mL solution. (acetic acid, Ka= 1.8 x 10-5)

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 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 = ☐

What is the pH for a weak monoprotic acid if a 0.020 M solution of the acid has a Ka of 3.28 x 10-7 ?

2.  The ionization constant for acetic acid is 1.8 x 10-5. How many grams of NaC2H3O2 must be added to one liter of a 0.20 M solution of HC2H3O2 to maintain a hydrogen ion concentration of 6.5 x 10-5 M?

What is the pH of 0.025 M aqueous acetate ion? (Kb of CH3CO2– = 5.6 ×× 10–10)

Calculate the pH of a solution prepared by dissolving 0.040 moles of sodium nitrite (NaNO2) in 200 mL of a 0.10 M nitrous acid solution (HNO2, Ka = 5.1 x 10-4).

A chemist named Ciara titrates X mL of a 0.7633 M hypochlorous acid (HA) solution with 0.3245 M solution of LiOH at 25 degrees Celsius. Calculate the pH at equivalence. The Ka of hypochlorous acid is 3.16 x 10-8.

A 0.50 M solution of an acid found in milk has a pH of 3.27. What is the percentage ionization of the acid? Percent ionization = i What is the value of K₂ for the acid? K₂= x 10 i %