A titration of an unknown monoprotic acid was made with a NaOH solution of 0.0810M. As a result, the unknown monoprotic...
A titration of an unknown monoprotic acid was made with a NaOH solution of 0.0810M. As a result, the unknown monoprotic acid gave an MM = 201 g / mol, gave a Pka = 5.55 and a Ka of 3.01x10 ^ (-6). What monoprotic acid could you deduce based on the results?
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A titration of an unknown monoprotic acid was made with a NaOH solution of 0.0810M. As a result, the unknown monoprotic...
35.25 mL of NaOH solution are required to titrate 0.5745 g of an unknown monoprotic acid....
35.25 mL of NaOH solution are required to titrate 0.5745 g of an unknown monoprotic acid. Prior standardization of the NaOH determined its concentration as 0.1039 M. 1. Use the data provided to determine the molar mass of the unknown acid 2. If 20 mL of a 1.0 M solution of the unknown monoprotic acid is placed into a beaker and 10 mL of 0.1 M NaOH is added, the pH of the final solution is 1.9. What is the...
In the titration of a solution of weak monoprotic acid with a 0.1275 M solution of NaOH, the pH h...
In the titration of a solution of weak monoprotic acid with a 0.1275 M solution of NaOH, the pH half way to the equivalence point was 4.48. In the titration of a second solution of the same acid, exactly twice as much of a 0.1275 M solution of NaOH was needed to reach the equivalence point. What was the pH half way to the equivalence point in this titration?
In the titration of a solution of weak monoprotic acid with...
A solution of an unknown monoprotic acid has a mass concentration of 2.8 g L-1. A...
A solution of an unknown monoprotic acid has a mass concentration of 2.8 g L-1. A titration was performed and the concentration was found to be 0.038 mol L-1. What is the molar mass of the unknown monoprotic acid in solution?
A beaker contains a 25 mL solution of an unknown monoprotic acid that reacts in a...
A beaker contains a 25 mL solution of an unknown monoprotic acid that reacts in a 1:1 stochiometric ratio with NaOH. Titrate the solution with NaOH to determine the concentration of the acid. Perform a titration by setting the concentration of the NaOH solution and adding it to the acid solution using the different Add Base buttons. The equivalence point of the titration is passed when the solution color changes. The unknown sample can be titrated multiple times by pressing...
5. The Ka and Molar Mass of a Monoprotic Weak Acid a. Suppose that–unknown to you–the...
5. The Ka and Molar Mass of a Monoprotic Weak Acid a. Suppose that–unknown to you–the primary standard KHP (potassium hydrogen phthalate, KHC8H4O4) had a potassium iodide impurity of approximately one percent by mass. How would this have influenced the calculated molarity of your sodium hydroxide solution? Would your calculated value be too low, too high, or unchanged? Explain your answer. b. Sketch a typical titration curve for a monoprotic weak acid titrated with a strong base. Label the axes...
If the pH at the equivalence point for titration of a monoprotic weak acid with NaOH...
If the pH at the equivalence point for titration of a monoprotic weak acid with NaOH is 9.00, and 10 mL of base is required to reach the equivalence point, how would you determine the pKa of the acid? the pKa is 9.00 determine the pH after 5 mL of base is added; this is the pKa determine the pH when 20 mL of base is added; this is the pKa the pKa is -log(9)
A sample of 0.2140 g of an unknown monoprotic acid was dissolved in 25.0 mL of...
A sample of 0.2140 g of an unknown monoprotic acid was dissolved in 25.0 mL of water and titrated with 0.0950 M NaOH. The titration required 30.0 mL of base to reach the equivalence point, at which point the pH was 8.68. a) What is the molecular weight of the acid? b) What is the pKa of the acid?
A beaker contains a 25 mL solution of an unknown monoprotic acid that reacts in a...
A beaker contains a 25 mL solution of an unknown monoprotic acid that reacts in a 1:1 stochiometric ratio with NaOH. Titrate the solution with NaOH to determine the concentration of the acid. Perform a titration by setting the concentration of the NaOH solution and adding it to the acid solution using the different Add Base buttons. The equivalence point of the titration is passed when the solution color changes. The unknown sample can be titrated multiple times by pressing...
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 ?
please ignore question1 A student titrated 0.180 g of an unknown acid with 0.10 M NaOH...
please ignore question1
A student titrated 0.180 g of an unknown acid with 0.10 M NaOH solution and the follow data set was obtained: mL of 0.1M NAOH mL of 0.1M pH pH NaOH 0 2.20 20 6.32 22 2 3.25 6.70 4 4.00 4.25 24 7.00 26 6 9.00 8 11.20 4.50 28 10 4.81 30 11.70 12 5.25 32 12.00 5.55 14 34 12.22 16 5.75 36 38 12.40 18 6.10 12.60 1. Prepare a titration curve using...
In the titration of a solution of weak monoprotic acid with a 0.1275 M solution of NaOH, the pH half way to the equivalence point was 4.48. In the titration of a second solution of the same acid, exactly twice as much of a 0.1275 M solution of NaOH was needed to reach the equivalence point. What was the pH half way to the equivalence point in this titration?
In the titration of a solution of weak monoprotic acid with...
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 ?
please ignore question1
A student titrated 0.180 g of an unknown acid with 0.10 M NaOH solution and the follow data set was obtained: mL of 0.1M NAOH mL of 0.1M pH pH NaOH 0 2.20 20 6.32 22 2 3.25 6.70 4 4.00 4.25 24 7.00 26 6 9.00 8 11.20 4.50 28 10 4.81 30 11.70 12 5.25 32 12.00 5.55 14 34 12.22 16 5.75 36 38 12.40 18 6.10 12.60 1. Prepare a titration curve using...
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