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A student adds 13.11 grams of propionic acid (a monoprotic acid with molar mass = 74.08...
To a 25.00 mL volumetric flask, a lab technician adds a 0.300 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...
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 1.300 grams of an unknown monoprotic acid into a 250 mL...
An analytical chemist weighs out 1.300 grams of an unknown monoprotic acid into a 250 mL volumetric flask and dilutes to the mark. The chemist then obtains 100 mL of the solution and titrates the 100mL of the solution with 0.1 M NaOH. When the titration reaches the equivalence point, the chemist finds he has added 24.50 mL of NaOH solution. Calculate the molar mass of the unknown
2. A student titrates 30.5 mL of a 3.50 g/L monoprotic acid (HA) with 15.0 mL...
2. A student titrates 30.5 mL of a 3.50 g/L monoprotic acid (HA) with 15.0 mL of 0.10 M NaOH solution. a. Determine the concentration of to monoprotic acid (the ratio of the acid to base is 1:1). b. Determine the molar mass of the acid.
0.5 pts Question 1 A student titrates 0.139 g of an unknown monoprotic weak acid to...
0.5 pts Question 1 A student titrates 0.139 g of an unknown monoprotic weak acid to the equivalence point with 44.6 mL of 0.100 M NaOH (aq). What is the molar mass of the weak acid? O 0.0615 g/mol 0.0312 g/mol 13.9 g/mol 31.2 g/mol O 61.5 g/mol
An analytical chemist weighs out 0.041 g of an unknown monoprotic acid into a 250 mL...
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...
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 ?
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 0.375 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.
calculate the molar mass of the unknown acid round your answer to three significant digits. An...
calculate the molar mass of the unknown acid round your answer
to three significant digits.
An analytical chemist weighs out 0.280 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 0.1400 M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 26.7 ml of NaOH solution Calculate the molar mass of the unknown acid. Round your answer...
5.00 mL of a solution containing a monoprotic acid was placed in a 100-mL volumetric flask,...
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...
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 =...
2. A student titrates 30.5 mL of a 3.50 g/L monoprotic acid (HA) with 15.0 mL of 0.10 M NaOH solution. a. Determine the concentration of to monoprotic acid (the ratio of the acid to base is 1:1). b. Determine the molar mass of the acid.
0.5 pts Question 1 A student titrates 0.139 g of an unknown monoprotic weak acid to the equivalence point with 44.6 mL of 0.100 M NaOH (aq). What is the molar mass of the weak acid? O 0.0615 g/mol 0.0312 g/mol 13.9 g/mol 31.2 g/mol O 61.5 g/mol
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 ?
calculate the molar mass of the unknown acid round your answer
to three significant digits.
An analytical chemist weighs out 0.280 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 0.1400 M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 26.7 ml of NaOH solution Calculate the molar mass of the unknown acid. Round your answer...
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