Consider the titration of a 25.0-mL sample of 0.175 M CH;NH2 with 0.150 M HBr. Determine each quantity. a. the initial pH b. the volume of added acid required to reach the equivalence point c. the pH at 5.0 mL of added acid d. the pH at one-half of the equivalence point e. the pH at the equivalence point f. the pH after adding 5.0 mL of acid beyond the equivalence point
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- Consider the titration of butyric acid (HBut) with sodium hydroxide. In an experiment, 50.00 mL of 0.350 M butyric acid is titrated with 0.225 M NaOH. Ka HBut=1.5105. (a) Write a balanced net ionic equation for the reaction that takes place during titration. (b) What are the species present at the equivalence point? (c) What volume of sodium hydroxide is required to reach the equivalence point? (d) What is the pH of the solution before any NaOH is added? (e) What is the pH of the solution halfway to the equivalence point? (f) What is the pH of the solution at the equivalence point?A 0.2481 M solution of KOH is used to titrate 30.00 mL of 0.269 M hydrobromic acid. Assume that volumes are additive. (a) Write a balanced net ionic equation for the reaction that takes place during the titration. (b) What are the species present at the equivalence point? (c) What volume of KOH is required to reach the equivalence point? (d) What is the pH of the solution 1. before any KOH is added? 2. halfway to the equivalence point? 3. at the equivalence point?Consider the titration of a 25.0-mL sample of 0.115 M RbOH with 0.100 M HCl. Determine each quantity.a. the initial pHb. the volume of added acid required to reach the equivalence pointc. the pH at 5.0 mL of added acidd. the pH at the equivalence pointe. the pH after adding 5.0 mL of acid beyond the equivalence point
- Consider the titration of a 20.0-mL sample of 0.105 M HC2H3O2 with 0.125 M NaOH. Determine each quantity.a. the initial pHb. the volume of added base required to reach the equivalence pointc. the pH at 5.0 mL of added based. the pH at one-half of the equivalence pointe. the pH at the equivalence pointf. the pH after adding 5.0 mL of base beyond the equivalence pointConsider the titration of a 21.0-mL sample of 0.110 M HC2H3O3 (Ka=1.8×10−5) with 0.120 M NaOH... 1. Determine the initial pH and the volume of added base required to reach the equivalence point. 2. Determine the pH at 5.00 mL of the added base, the pH at one-half of the equivalence point, and the pH after adding 6.00 mL of base beyond the equivalence point..Consider the titration of a 25.0-mL sample of 0.175 M CH3NH2 with 0.150 M HBr. Determine each quantity.a. the initial pHb. the volume of added acid required to reach the equivalence pointc. the pH at 5.0 mL of added acidd. the pH at one-half of the equivalence pointe. the pH at the equivalence pointf. the pH after adding 5.0 mL of acid beyond the equivalence
- Consider the titration of a 35.0-mL sample of 0.175 M HBr with 0.200 M KOH. Determine each quantity.a. the initial pHb. the volume of added base required to reach the equivalence pointc. the pH at 10.0 mL of added based. the pH at the equivalence pointe. the pH after adding 5.0 mL of base beyond the equivalence pointA 51 mL sample of 0.13 M CH3COOH is titrated with 0.045 M LiOH. Calculate the pH of the solution after the addition of 41.99 mL LiOH.Consider the titration of 50.00 mL of 0.100 M benzoic acid (HC7H5O2, Ka = 6.3 × 10−5) (aq) with 0.130 M LiOH(aq). What is the pH of the titration solution... a) before any LiOH is added? b) after 20.00 mL of LiOH is added? c) at the equivalence point? Also, what volume of LiOH is required to reach this? d) For this titration, which is the best indicator to use: phenolphthalein, bromothymol blue, or methyl orange? Justify your answer.
- Consider the titration of a 27.6 mL sample of 0.120 M RbOHwith 0.100 MM HCl. Determine the pH after adding 6.0 mL of acid beyond the equivalence point.A student needs to determine by titration with NaOH the precise %KHP in an unknown sample that is thought to contain approximately 50%KHP. Approximately what mass of sample should the student use in order to use about 20mL of 0.1005 M NaOH to reach the endpoint of the titration?A 30.0 mL sample of 0.135 M aqueous benzoic acid is titrated with 0.115 M aqueous potassium hydroxide. (a) What is the initial pH of the benzoic acid solution? (b) What is the pH after the addition of 5.00 mL potassium hydroxide solution? (c) What volume of potassium hydroxide solution is required to reach halfway to the equivalence point? (d) Calculate the pH at the point halfway to the equivalence point. (e) What volume of potassium hydroxide solution is required to reach the equivalence point? (see [c]) (f) Calculate the pH at the equivalence point. (g) Calculate the pH of the solution when an additional 5.0 mL of potassium hydroxide has been added (5.00 mL in addition to the amount required to reach the equivalence point).