To a 25.00 mL volumetric flask, a lab technician adds a 0.375 g sample of a weak monoprotic acid, HA , and dilutes to the mark with distilled water. The technician then titrates this weak acid solution with 0.0923 M KOH . She reaches the endpoint after adding 44.93 mL of the KOH solution.
After the technician adds 15.35 mL of the KOH solution, the pH of the mixture is 5.73. Determine the p?a of the weak acid.
To a 25.00 mL volumetric flask, a lab technician adds a 0.375 g sample of a...
To a 25.00 mL volumetric flask, a lab technician adds a 0.300 g sample of a weak monoprotic acid, HA, and dilutes to the mark with distilled water. The technician then titrates this weak acid solution with 0.0867 M KOH. She reaches the endpoint after adding 41.23 mL of the KOH solution. Determine the number of moles of the weak acid in the solution. moles of weak acid: mol Determine the molar mass of the weak acid. molar mass =...
To a 25.00 mL volumetric flask, a lab technician adds a 0.350 g sample of a weak monoprotic acid, HA, and dilutes to the mark with distilled water. The technician then titrates this weak acid solution with 0.0868 M KOH. She reaches the endpoint after adding 43.65 mL of the KOH solution. Determine the number of moles of the weak acid in the solution. moles of weak acid: mol Determine the molar mass of the weak acid. molar mass =...
An analytical chemist weighs out 0.106g of an unknown monoprotic acid into a 250mL volumetric flask and dilutes to the mark with distilled water. He then titrates this solution with 0.1500MNaOH solution. When the titration reaches the equivalence point, the chemist finds he has added 7.3mL of NaOH solution.Calculate the molar mass of the unknown acid. Round your answer to 2 significant digits.
An analytical chemist weighs out 0.082g of an unknown monoprotic acid into a 250mL volumetric flask and dilutes to the mark with distilled water. He then titrates this solution with 0.1100M NaOH solution. When the titration reaches the equivalence point, the chemist finds he has added 14.2mL of NaOH solution.Calculate the molar mass of the unknown acid. Round your answer to 2 significant digits.
An analytical chemist weighs out 0.041 g of an unknown monoprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. She then titrates this solution with 0.1700 M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 5.2 mL of NaOH solution. Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits. x 6 ?
An analytical chemist weighs out 0.144 g of an unknown monoprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. She then titrates this solution with 0.0900 M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 22.2 mL of NaOH solution. Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits. mol x 6 ?
An analytical chemist weighs out 0.260g of an unknown diprotic acid into a 250mL volumetric flask and dilutes to the mark with distilled water. She then titrates this solution with 0.1400M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 24.7mL of NaOH solution. Calculate the molar mass of the unknown acid. Round your answer to 3 significant digits.
an analytical chemist weighs out 0.435g of an unknown triprotic acid into a 250mL volumetric flask and dilutes to the mark with distilled water. She then titrates this solution with 0.1700M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 40.0mL of NaOH solution.Calculate the molar mass of the unknown acid. Round your answer to 3 significant digits.
5.00 mL of a solution containing a monoprotic acid was placed in a 100-mL volumetric flask, diluted to the mark with deionized water and mixed well. Then, 25.00 mL of this diluted acid solution was titrated with 0.08765 M NaOH. 9.23 mL of NaOH was required to reach the endpoint. a. What does the term monoprotic mean? b. Determine the molar ratio between the acid and NaOH. c. Calculate the moles of NaOH used in this titration. d. Calculate the...
An analytical chemist weighs out 0.274 g of an unknown diprotic acid into a 250 ml volumetric flask and dilutes to the mark with distilled water. She then titrates this solution with 0.0600 M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 68.1 ml of NaOH solution. Calculate the molar mass of the unknown acid. Round your answer to 3 significant digits. mol X2 ?