9. A student carries out a titration to determine the molar mass of an unknown acid, A • The student dissolves 2.24 g of acid A in distilled water and makes the solution up to 250.0 cm. The student titrates a 25.0 cm" portion of this solution with 0.120 mol dm NaOH. 25.25 cm of 0.120 mol dm NaOH are required to reach the end point. (a) Name the apparatus that the student should use to • make up the acid solution to 250.0 cm measure the 25.0 cm' portion of acid solution. make up the acid solution to 250 cm: ....... measure the 25.0 cm' portion: (b) The acid reacts with NAOH in a 1:1 molar ratio. Calculate the molar mass of acid A. molar mass of acid A = g mol (c) The student is not confident that their titre is accurate. Suggest what the student should do next to reduce the effect of any random error in the titration. ....**... .....*..

9. A student carries out a titration to determine the molar mass of an unknown acid, A • The student dissolves 2.24 g of acid A in distilled water and makes the solution up to 250.0 cm. The student titrates a 25.0 cm" portion of this solution with 0.120 mol dm NaOH. 25.25 cm of 0.120 mol dm NaOH are required to reach the end point. (a) Name the apparatus that the student should use to • make up the acid solution to 250.0 cm measure the 25.0 cm' portion of acid solution. make up the acid solution to 250 cm: ....... measure the 25.0 cm' portion: (b) The acid reacts with NAOH in a 1:1 molar ratio. Calculate the molar mass of acid A. molar mass of acid A = g mol (c) The student is not confident that their titre is accurate. Suggest what the student should do next to reduce the effect of any random error in the titration. ....**... .....*..

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

Solid zinc nitrate is slowly added to 175 mL of a 0.0572 M potassium sulfide solution. The concentration of zinc ion required to just initiate precipitation is M.
A student is asked to standardize a solution of barium hydroxide. He weighs out 0.929 g potassium hydrogen phthalate ( KHC8H404, treat this as a monoprotic acid). It requires 36.8 mL of barium hydroxide to reach the endpoint. A. What is the molarity of the barium hydroxide solution? M This barium hydroxide solution is then used to titrate an unknown solution of hydrobromic acid. B. If 28.5 mL of the barium hydroxide solution is required to neutralize 13.3 mL of hydrobromic acid, what is the molarity of the hydrobromic acid solution? M
a student weights out 1.118 g of impure KHP, dissolves the sample in deionized water and titrates it with 0.1001 M NaOH solution. If the titration requires 2710 mL of the NaOH solution, and non of the impurities react with NaOH, what is the percent KHP in the sample?
3
A group of students determined the titratable of two brands of tetra pack juice. Titratable acidity is a measure of the total acid concentration in a food sample. Titratable acidity in fruit are commonly expressed as (mg) of hydrous citric acid (H3CitH2, MM: 210.14 g/mol) per solution Initially, they have prepared the sodium hydroxide solution and standardized it with oxalic acid dihydrate (H2C204*2H2O; MM: 126.02 g/mol; 99.5% purity up to the faint pink endpoint of the phenolphthalein. The volumes of the duplicate trial of the standardization were summarized in the table. In the Sample analysis, 5.00 ml each of tetra pack was diluted with 50.0 ml of distilled water and titrated up to the end point of 8.2 using a pH meter. Consider the tables below and answer the following questions. T1. Standardization of the NaOH titrant Grams of primary standard Volume NaOH used (ml) þ.2490 39.4 0.2510 39.5 T2. Titration of the Sample with the standardized titrant. Sample Volume Readout of Burette…
What mass of Fe(OH)3 will be obtained when 100. mL of 0.240 M FeClz is mixed with 200. mL of 0.182 MNAOH? |g Fe(OH)3
A 0.8159 g sample of HCl was placed into a 50 mL volumetric flask and the sample was thoroughly dissolved in water to make 50 mL of solution. It required 22.07 mL of NaOH to reach the endpoint in the titration. What is the molarity of the NaOH solution? I mg IHE/ 2.022 4 mol 0.81599 Hcl 36.4bg.
You determine the molarity of an unknown acid by titrating it with 0.38 M KOH. You use a 73.08 mL sample of the acid and it requires 24.57 mL of base to reach the endpoint. What is the molarity of the acid? (Only enter the number, do not enter units)
Solubility Curves of Selected Compounds 150 140 130 120 110 100 NaNO, 90 80 70 60 NH C KCI Nac 50 40 30 20 KCIÓ 10 Cez(SO4)3 10 20 30 40 50 60 70 90 100 Temperature (C) The compound whose solubility increases the fastest with an increase in temperature is: OKI O NANO3 O KNO3 O NH, O NH&CI O KCI O NaCI O KCIO, O Ce:(SOala DELL Grams of solute per 100 g H,O NH FONX
1. A sample (0.212g) of an unknown acid was dissolved in water and analyzed by titrating with 0.1760 M NaOH. A volume of 15.48 mL of NaOH was required to completely neutralize the acid. Calculate the molar mass of the acid in g/mol.
6. A student titrated 30.00 mL of a hydrochloric acid solution with 1.00 M sodium hydroxide. The sodium hydroxide was initially tilled to the 2.30 mL mark on the burette. Once the level in the burette reached 50.00 mL, the student was forced to refill the burette and did so to the 5.06 mL mark. The endpoint was finally reached when the sodium hydroxide level dropped to 32.09 mL on the burette. What is the molarity of the acid solution? Show work.
A 21.25 g of a mixture of the solid salts, sodium chloride and lead II nitrate, is added to distilled water and stirred. The precipitate that is formed is filtered and dried. Its mass was determined to be 11.06 g. Analysis of the remaining solution shoed that the following ions were present: Pb2+, Na+ and NO3". Determine the percent (by mass) of lead (II) nitrate in the mixture. Assume 100 % yield.