ࡱ> 796{ Ybjbjzz 0$Y 44,$@ .$n! $|{t" I[ 0@ !Z$=B$${${0B@ $4 T: Acids and Bases Worksheet At the equivalence point in a titration, what is true of moles of acid vs. moles of base? Label the following substances as strong electrolyte, weak electrolyte or non-electrolyte: BaCl2 (aq) b. HF (aq) c. KOH (aq) d. C6H12O6 (aq) e. HNO3 (aq) f. PbCl2 (s) In each of the following chemical equations, identify the conjugate acid-base pairs. a. HSO4- + H2O ( SO42- + H3O+ b. CH3NH2 + HCl ( CH3NH3+ + Cl- c. CH3COO- + H2O ( CH3COOH + OH- Complete the equation for each of the following conjugate acid-conjugate base reactions. HNO2 + H2O ( H3O+ + NO2- HBrO4 + H2O ( H3O+ + BrO4- Write the conjugate acid for each of the following: a. HPO42- _________ c. HS- _________ b. NO2- _________ d. S2- _________ Write the conjugate base for each of the following: a. HNO3 _________ c. H3O+ _________ b. HPO42- _________ d. H2CO3 _________ Calculate the [H+] in each of the following solutions, and indicate whether the solution is acidic, basic, or neutral. a. [OH-] = 3.99 x 10-5 M b. [OH-] = 7.23 x 10-2 M Calculate the [OH-] in each of the following solutions, and indicate whether the solution is acidic, basic, or neutral. a. [H+] = 1.27 x 10-3 M b. [H+] = 3.87 x 10-5 M For each pair of concentrations, tell which represents the more basic solution. [H+] = 1.21 x 10-8 M or [OH-] = 0.10 M [H+] = 0.00100 M or [OH-] = 1.78 x 10-13 M [H+] = 4.23 x 10-6 M or [OH-] = 1.15 x 10-7 M Calculate the pH corresponding to each of the hydrogen ion concentrations given below. Tell whether each solution is acidic, basic, or neutral. a. [H+] = 0.00100 M b. [H+] = 9.18 x 10-11 M Calculate the pH corresponding to each of the hydroxide ion concentrations given below. Tell whether each solution is acidic, basic, or neutral. a. [OH-] = 4.22 x 10-3 M b. 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