The Ka for formic acid (HCO2H) is 1.8x10-4, What is the pH of a 0.20M aqueous solution of sodium formate (NaHCO2)?

The pH of a 0.16 M solution of a weak acid, HA, is 2.85. What is the value of Ka for the weak acid?

The ka of an unknown acid, HYO₂,  is determined to be 5 x 10⁻² empirically. What is the pH of a 0.1 M solution of HYO₂?

The pH of an aqueous solution of 0.506 M benzoic acid , C6H5COOH is

The pH of an aqueous solution of 0.149 M potassium acetate, (Assume that KCH3COO, is K. (HCH3COO) = 1.80 × 10-5.) This solution is

Over the past 250 years, the average upper-ocean pH near the Pacific Northwest has decreased by about 0.1 units, from about 8.2 to 8.1. This drop in pH corresponds to an increase in acidity of about 30%. When CO2 levels in seawater rise, the availability of carbonate ion, CO32−, makes it more difficult for marine organisms to build and maintain shells and other body parts from calcium carbonate. Calculate H3O+ and OH− concentrations at pH levels of 8.2 and 8.1. Demonstrate by calculations that this decrease in pH corresponds to an increase in acidity of about 30%. Explain the relationship between the pH of seawater and the availability of carbonate ions. Does the change in pH from 8.2 to 8.1 result in an increase or decrease in the availability of carbonate ions?

Calculate the pH of a weak base solution ([B] > 100 K₂). Calculate the pH of a 0.247 M aqueous solution of hydroxylamine (NH₂OH, K₂ = 9.1×109) and the equilibrium concentrations of the weak base and its conjugate acid. pH [NH₂OH] equilibrium (NH3OH*]equilibrium ΣΣ