0.5 pts Question 1 A student titrates 0.139 g of an unknown monoprotic weak acid to...
A sample of 0.2140 g of an unknown monoprotic weak acid was dissolved in 25.0 mL of water and titrated with 0.0950 M NaOH. The acid required 15.50 mL of NaOH to reach the equivalence point. What is the molar mass of the unknown acid?
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.
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 ?
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...
Following the Procedure of this experiment, a student titrated 0.653 g of an unknown weak, monoprotic acid with 0.100 M NaOH and monitored the titration with a pH meter. His titration data were: Volume of NaOH solution added, mL /// pH 0.00 | 3.30 2.00 | 4.22 4.00 | 4.55 6.00 | 4.76 8.00 | 4.92 10.00 | 5.06 12.00 | 5.18 14.00 | 5.29 16.00 | 5.40 18.00 | 5.51 20.00 | 5.62 22.00 | 5.74 24.00 | 5.88...
A student adds 13.11 grams of propionic acid (a monoprotic acid with molar mass = 74.08 g/mol) to water. When she takes a 25.00 g sample of this solution, and titrates it with 0.1111 M NaOH(aq), she finds that she needs to add 17.17 mL of this solution to reach the endpoint. What was the percent by mass of propionic acid in the solution she made?
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 ?
A sample of 0.2140 grams of an unknown monoprotic weak acid was dissolved in 25.0mL of water and titrated with 0.0950M NaOH. The acid required 15.50mL of NaOH to reach the equivalence point. What is the molar mass of the unknown acid?
Given the following information: 1.6 g of an unknown monoprotic acid (HA) required 50.80 mL of a 0.35 M NaOH solution to reach the equivalence point calculate the molar mass (g/mol) of the acid. Enter the value ONLY. Do not include the units,
QUESTION 1 The equivalence point of a weak, monoprotic acid with a volume of 22.00 ml was reached after adding 22.10 mL of 0.1025 M NaOH(aq) and the pH at this volume was 8.91. The pH was 3.37 when the volume of NaOH(aq) added was 11.05 mL. What is the value of Ka for this unknown acid? O 0.1025 1.23 x 10-9 0.1030 8.91 3.37 4.2710-4