For the titration of 25.0 ml of a 0.10 m solution of acetic acid, ch3cooh, with 0.10 m sodium hydroxide solution (ka of acetic acid is 1.8*10^-5):

if this weak acid is effective as a buffer between the concentration ratios for the conjugate acid-base pair of 10: 1 and 1: 10, what ph range does this cover?

17.1 Acid–Base Reactions 17.1a Strong Acid/Strong Base Reactions In Chemical Reactions and Solution Stoichiometry (Unit 4) you learned that acids and bases react to form water and a salt and that these reactions are called neutralization reactions because, on completion of the reaction, the solution is neutral. However, acid–base reactions do not always result in the formation of a solution with a neutral pH, and not all acid-base reactions proceed to 100% completion (Interactive Figure 17.1.1). Interactive Figure 17.1.1 Investigate the extent of acid-base reactions. HCl(aq) 1 NaOH(aq) 0% 100% H2O(,) 1 NaCl(aq) HCl(aq) 1 NH3(aq) 0% 100% NH4+(aq) 1 Cl–(aq) HF(aq) 1 CH3CO2–(aq) 0% 100% CH3CO2H(aq) 1 F–(aq) HCN(aq) 1 NH3(aq) 0% 100% NH4+(aq) 1 CN–(aq) © 2013 Cengage Learning Figure 17.1.1 Not all acid-base reactions go to 100% completion There are four classes of acid–base reactions: strong acid + strong base, strong acid + weak base, weak acid + strong base, and weak acid + weak base. For each, we will investigate the extent of the reaction and the pH of the resulting solution when equimolar amounts of reactants are combined