Suppose a group of students put 2.92 grams of an unknown solid acid into a 250-mL Erlenmeyer flask and filled it up to the mark with deionized water. The students then proceeded to make 250- mL of a 0.18 M NaOH(aq) solution in another 250-mL Erlenmeyer flask. The students took a 22-mL aliquot of the acid solution and transfer it to another 250-mL Erlenmeyer flask. The students were given a pH meter that was already calibrated by their teaching assistant (T.A.) and they got the following result shown in the table below. What is the molar mass of the solid acid in units of grams/mole to 2 decimal places? Table 2. Titration curve data. VNAOH VN2OH pH pH (mL) (mL) 2.65 8.00 6.32 1 3.29 8.10 10.45 2 3.63 8.20 10.93 3.88 8.30 11.16 4 4.10 8.40 11.30 4.32 8.50 11.41 4.57 8.60 11.50 7.00 4.93 8.70 11.57 7.10 4.98 8.80 11.63 7.20 5.03 8.90 11.68 7.30 5.09 9 11.73 7.40 5.16 10 12.03

Suppose a group of students put 2.92 grams of an unknown solid acid into a 250-mL Erlenmeyer flask and filled it up to the mark with deionized water. The students then proceeded to make 250- mL of a 0.18 M NaOH(aq) solution in another 250-mL Erlenmeyer flask. The students took a 22-mL aliquot of the acid solution and transfer it to another 250-mL Erlenmeyer flask. The students were given a pH meter that was already calibrated by their teaching assistant (T.A.) and they got the following result shown in the table below. What is the molar mass of the solid acid in units of grams/mole to 2 decimal places? Table 2. Titration curve data. VNAOH VN2OH pH pH (mL) (mL) 2.65 8.00 6.32 1 3.29 8.10 10.45 2 3.63 8.20 10.93 3.88 8.30 11.16 4 4.10 8.40 11.30 4.32 8.50 11.41 4.57 8.60 11.50 7.00 4.93 8.70 11.57 7.10 4.98 8.80 11.63 7.20 5.03 8.90 11.68 7.30 5.09 9 11.73 7.40 5.16 10 12.03

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

On their third titration trial, the CHM 111 student used 18.80 mL of 0.205 M NaOH(aq) to neutralize 25.0 mL of HCl(aq). Calculate the molar concentration of the HCl solution to the correct number of significant figures.
In a lab, you diluted a sample of bleach to 1/10 concentration in a 250 volumetric flask. Then quantitatively transferred 25 ml of the 1/10 concentration diluted bleach into a beaker and titrated it with a standard sodium thiosulfate solution that has a molarity of 0.1215M. You repeated this 3 times. The data below is the amount of sodium thiosulfate that was titrated in the 3 runs. Calculate the molarity in each run of the diluted bleach and the concentration of undiluted bleach sample. Titration 1: 45.55 ml Titration 2: 45.67 ml Titration 6: 45.58 ml
You add 12.5mL of a 5.00M stock solution of sodium hydroxide to a 500mL volumetric flask and dilute to the mark with distilled water. What is the concentration of the resulting solution?
One way in which the useful metal copper is produced is by dissolving the mineral azurite, which contains copper(II) carbonate, in concentrated sulfuric acid. The sulfuric acid reacts with the copper(II) carbonate to produce a blue solution of copper(II) sulfate. Scrap iron is then added to this solution, and pure copper metal precipitates out because of the following chemical reaction: Fe (s) + CuSO4 (aq) → Cu (s) + FeSO4 (aq)Suppose an industrial quality-control chemist analyzes a sample from a copper processing plant in the following way. He adds powdered iron to a 200.mL copper(II) sulfate sample from the plant until no more copper will precipitate. He then washes, dries, and weighs the precipitate, and finds that it has a mass of 73.mg . Calculate the original concentration of copper(II) sulfate in the sample. Be sure your answer has the correct number of significant digits.
One way in which the useful metal copper is produced is by dissolving the mineral azurite, which contains copper(II) carbonate, in concentrated sulfuric acid. The sulfuric acid reacts with the copper(II) carbonate to produce a blue solution of copper(II) sulfate. Scrap iron is then added to this solution, and pure copper metal precipitates out because of the following chemical reaction: Fe(s) + CuSO4(aq) → Cu(s) + FeSO4 (aq) Suppose an industrial quality-control chemist analyzes a sample from a copper processing plant in the following way. He adds powdered iron to a 350. mL copper(II) sulfate sample from the plant until no more copper will precipitate. He then washes, dries, and weighs the precipitate, and finds that it has a mass of 111. mg. Calculate the original concentration of copper(II) sulfate in the sample. Be sure your answer has the correct number of significant digits. 0-2 X 5
A chemist performs a gravimetric analysis. The chemist combines 1.00 L of 2.00 M AGNO, (ag) with 1.00 L of 4.00 M NaCl (aq) in an Erlenmeyer flask. Both the AGNO, (aq) solution and the NaCl(ag) solution are colorless. After the mixture has been stirred, a cloudy white substance is observed at the bottom of the flask. Which of the following is the complete ionic equation for the reaction that occurs in the beaker? A Ag+ (ag) + Cl- (aq) → AgCl (s) B Na (aq) + NO3 (aq) → NANO3 (s) Ag (aq) + NO, (aq) + Na (aq) + Cl-(aq) → AgCl(s) + Na* (aq) + NO, (aq) NaCl(aq) + AGNO, (aq) Ag (s) + NANO, (aq)
A chemist performs a gravimetric analysis. The chemist combines 1.00 L of 2.00 M AGNO3 (ag) with 1.00 L of 4.00M Nacl (ag) in an Erlenmeyer flask. Both the AgNO3 (ag) solution and the NaCl(ag) solution are colorless. After the mixture has been stirred, a cloudy white substance is observed at the bottom of the flask. Which of the following is the complete ionic equation for the reaction that occurs in the beaker? Ag* (aq) + Cl (ag) → AgCl (s) B) Nat (aq) + NO, (ag) → NaNO; (s) Ag+ (ag) + NO3 (ag) + Na* (ag) + Ci (ag) → AgCl(s) + Na* (ag) + NOS (ag) D) NaCl(aq) + AGNO, (ag) → Ag (s) + NANO3 (ag)
2. How many milliliters of 12.0 M HCI (aq) are required to prepare 250 milliliters of 1.0 M HCl(aq)? Corne
One way in which the useful metal copper is produced is by dissolving the mineral azurite, which contains copper(II) carbonate, in concentrated sulfuric acid. The sulfuric acid reacts with the copper(II) carbonate to produce a blue solution of copper(II) sulfate. Scrap iron is then added to this solution, and pure copper metal precipitates out because of the following chemical reaction: Fe (s) + CuSO4 (aq) → Cu (s) + FeSO4 (aq)Suppose an industrial quality-control chemist analyzes a sample from a copper processing plant in the following way. He adds powdered iron to a 300.mL copper(II) sulfate sample from the plant until no more copper will precipitate. He then washes, dries, and weighs the precipitate, and finds that it has a mass of 67.mg . Calculate the original concentration of copper(II) sulfate in the sample. Be sure your answer has the correct number of significant digits.
How many grams of Sodium Hydroxide (NaOH) were dissolved into a 732 mL 2.00 M solution?
A Chemistry Student Trainee at a certain University Chemical Laboratory was instructed by the Professor to standardize a Sodium hydroxide solution. If the said solution was 0.25N, what mass in grams of Potassium acid phthalate (204 g/mol) are needed so that the final burette reading will not exceed 40.0 mL?
A solution of NaOH(aq) was standardized by titration using oxalic acid (H₂C₂O4) as the primary standard. The following data was collected: Mass of H₂C₂O4(s) used = 1.02 g Volume of NaOH(aq) used = 40.6 ml. Calculate the concentration of the NaOH(aq)