Part A: Watch the animation and observe the titration process of a standard 0.100 M sodium hydroxide solution with 50.0 \rm ml of a 0.100 M hydrochloric acid solution. Identify which of the following statements regarding acid-base titration are correct. Check all that apply. a - The titration process is based on a chemical reaction. b - The \rm pH of the solution at the equivalence point is 7. c - At the endpoint, the \rm pH of solution is 10 and the color of solution is pink. d - At the beginning of the titration process, the \rm pH of the solution increases rapidly. e - The chemical reaction involved in an acid-base titration is a neutralization reaction. f - Before any base is added to the solution, the \rm pH of the solution is high. g - In a titration process, the endpoint is reached before the equivalence point. h - The \rm pH of the solution changes very slowly at the equivalence point. Part B: 100 \rm mL of 1.00 M HCl solution is titrated with 1.00 M~ \rm NaOH solution. You added the following quantities of 1.00 M NaOH to the reaction flask. Classify the following conditions based on whether they are before the equivalence point, at the equivalence point, or after the equivalence point/endpoint. Drag the appropriate items to their respective bins 10.0mL of 1.00 M NaOH 150 mL of 1.00 M NaOH 5.00 mL of 1.00 M NaOH 50.0 mL of 1.00 M NaOH 200 mL of 1.00 M NaOH BINS: Before equivalent point At equivalent point After equivalent point Part C: A volume of 90.0 mL of a 0.400 M HNO3 solution is titrated with 0.470 M KOH. Calculate the volume of KOH required to reach the equivalence point.
Part A: Watch the animation and observe the titration process of a standard 0.100 M sodium hydroxide solution with 50.0 \rm ml of a 0.100 M hydrochloric acid solution. Identify which of the following statements regarding acid-base titration are correct. Check all that apply. a - The titration process is based on a chemical reaction. b - The \rm pH of the solution at the equivalence point is 7. c - At the endpoint, the \rm pH of solution is 10 and the color of solution is pink. d - At the beginning of the titration process, the \rm pH of the solution increases rapidly. e - The chemical reaction involved in an acid-base titration is a neutralization reaction. f - Before any base is added to the solution, the \rm pH of the solution is high. g - In a titration process, the endpoint is reached before the equivalence point. h - The \rm pH of the solution changes very slowly at the equivalence point. Part B: 100 \rm mL of 1.00 M HCl solution is titrated with 1.00 M~ \rm NaOH solution. You added the following quantities of 1.00 M NaOH to the reaction flask. Classify the following conditions based on whether they are before the equivalence point, at the equivalence point, or after the equivalence point/endpoint. Drag the appropriate items to their respective bins 10.0mL of 1.00 M NaOH 150 mL of 1.00 M NaOH 5.00 mL of 1.00 M NaOH 50.0 mL of 1.00 M NaOH 200 mL of 1.00 M NaOH BINS: Before equivalent point At equivalent point After equivalent point Part C: A volume of 90.0 mL of a 0.400 M HNO3 solution is titrated with 0.470 M KOH. Calculate the volume of KOH required to reach the equivalence point.
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