Acid/base equilibria (2011 VCE) 1) Which 0.1 M solution of the following acids has the highest pH a) nitrous acid b) ethanoic acid c) methanoic acid d) hypobromous acid Solution . 2) Write an equation for the reaction of methanoic acid and water Solution 3) Write an equilibrium expression for the acidity constant, Ka for the reaction in 2) above Solution 4) A solution is prepared by adding 0.500 mol of methanoic acid, HCOOH, and 0.100 mol of sodium methanoate, HCOONa, to 2.00 L of water. Determine the concentration of H3O+ ions in this solution. In your calculations assume that - the equilibrium concentration of HCOOH is approximately equal to the initial concentration of HCOOH. - the equilibrium concentration of HCOO- is approximately equal to the initial concentration of HCOO- Solution Click for the examiners report 5) Calculate the pH of this solution Solution 6) The following two solutions are prepared - Solution A: 1.00 L solution contains 0.500 mole of methanoic acid. - Solution B: 1.00 L solution contains 0.500 mole of methanoic acid and 0.100 mole of sodium methanoate. Which solution has the higher pH? Justify your answer in terms of the equilibria involved. Solution 