The pH of 300 mL solution made of 0.96 M acetic acid and 0.86 M potassium acetate is (K₂ = 1.8 x 10-5) after the addition of 0.80 moles NaOH Your Answer:

Determine the resulting pH when 0.003 mol of solid NaOH is added to a 100.0 mL buffer containing 0.13 M HClO and 0.37 M NaClO. The value of Ka for HClO is 2.9 × 10⁻⁸. Determine the moles of the ractant and product after the reaction of the acid and base. (Similar to ICE format but is instead Before (mol), Change (mol), and After (mol) Determine the ICE table for HClO (aq) + H2O - H3O+ + ClO- (aq) Fill in Ka= ? = 2.9 * 10-8 Calculate pH

Solution A contains 0.100 mol L−1 sodium methanoate and 0.126 mol L−1 methanoic acid. What is the concentration of methanoate ions (in mol L−1) after the addition of 5.0 mL of 0.010 mol L−1 HCl to 25.0 mL of solution A?

25.00mL of a 0.100 M sodium hydroxide is added to 45.00 mL of a 0.100 M acetic acid solution. The Ka of acetic acid is 1.8x10-5. What is the pH of the solution after adding NaOH?