# Consider a solution formed by mixing 62.0 mL of 0.100 M H2SO4, 29.0 mL of 0.100 M HOCl, 25.0 mL of 0.200 M NaOH, 25.0 mL of 0.100 M Ca(OH)2, and 10.0…

Consider a solution formed by mixing 62.0 mL of 0.100 M H2SO4, 29.0 mL of 0.100 M HOCl, 25.0 mL of 0.200 M NaOH, 25.0 mL of 0.100 M Ca(OH)2, and 10.0 mL of 0.150 M KOH. Calculate the pH of this solution.Calculate the pH after 0.020 mol NaOH is added to 1.00 L of each of the solutions.(a) 0.200 HONH2 (Kb = 1.1 10-8)(b) 0.200 M HONH3Cl(c) pure H2O(d) a mixture containing 0.200 M HONH2 and 0.200 M HONH3ClCalculate the pH of a solution that is 0.30 M HF and 1.00 M KF.A 25.0 mL sample of 0.100 M lactic acid (HC3H5O3, pKa = 3.86) is titrated with 0.100 M NaOH solution. Calculate the pH after the addition of the following amounts of NaOH.0.0 mL4.0 mL8.0 mL12.5 mLWhich of these solutions is a buffered solution?0.100 M HONH2 (Kb = 1.1 10-8)pure H2Oa mixture containing 0.100 M HONH2 and 0.100 M HONH3Cl0.100 M HONH3Clalculate the pH of each of the following buffered solutions.(a) 0.10 M acetic acid / 0.27 M sodium acetate(b) 0.27 M acetic acid / 0.10 M sodium acetate(c) 0.37 M acetic acid / 0.37 M sodium acetate(d) 0.50 M C2H5NH2 / 0.25 M C2H5NH3Cl(e) 0.57 M C2H5NH2 / 0.57 M C2H5NH3ClCalculate the pH of each of the following solutions.(a) 0.400 M HONH2 (Kb = 1.1 10-8)(b) 0.400 M HONH3Cl(c) pure H2O(d) a mixture containing 0.400 M HONH2 and 0.400 M HONH3ClCalculate the pH after 0.031 mol HCl is added to 1.00 L of each of the four solutions.(a) 0.100 M propanoic acid (HC3H5O2, Ka= 1.3 10-5)(b) 0.100 M sodium propanoate (NaC3H5O2)(c) pure H2O(d) a mixture containing 0.100 M HC3H5O2 and 0.100 M NaC3H5O2Calculate the pH after 0.12 mol of NaOH is added to 1.00 L of the solution that is 0.59 M HF and 1.08 M KF. Calculate the pH after 0.32 mol of HCl is added to 1.00 L of the solution that is 0.59 M HF and 1.08 M KF.