8.(c) A student plans to determine the concentration, in moldm, of CH,COOH in a botle ofvinegar. The student will carry out a titration with aqueous barium hydroxide, Ba(OH),(ag)The student's method is outlined belowDilute 10.0cm of vinegar from the bottle with distilled water and make the solutionup to 250.0cm3Add the diluted vinegar to the burette.Titrate 25.0 cm volumes of 0.0450 mol dm Ba(OH), with the diluted vinegar.The mean titre of the diluted vinegar is 25.45 cmThe reaction in the student's titration is shown below.2CH,COOH(aq) + Ba(OH),(aq) (CH,COO),Ba(aq) + 2H,0(1)(i) Calculate the concentration, in moldm-3, of CH,COOHthe original bottle of vinegar.Show your working.

Given Molarity of Ba(OH)2 solution = 0.0450 mol. dm-3 Volume of Ba(OH)2 solution = 25.0 cm3 Volume…

(c) A student plans to determine the concentration, in moldm- of CH,COH in a bottle of vinegar. The student will carry out a titration with aqueous barium hydroxide, Ba(OH) (aq) The student's method is outlined below. Dilute 10.0cm of vinegar from the bottle with distilled water and make the solution up to 250.0cm Add the diluted vinegar to the burette. Titrate 25.0 cm volumes of 0.0450 mol dm Ba(OH), with the diluted vinegar. The mean titre of the diluted vinegar is 25.45 cm The reaction in the student's titration is shown below. 2CH,COOH(aq) + Ba(OH),(aq) (CH,COO),Ba(aq) + 2H,0(1) (i) Calculate the concentration, in moldm, of CH,COOH in the original bottle of vinegar

(c) A student plans to determine the concentration, in moldm- of CH,COH in a bottle of vinegar. The student will carry out a titration with aqueous barium hydroxide, Ba(OH) (aq) The student's method is outlined below. Dilute 10.0cm of vinegar from the bottle with distilled water and make the solution up to 250.0cm Add the diluted vinegar to the burette. Titrate 25.0 cm volumes of 0.0450 mol dm Ba(OH), with the diluted vinegar. The mean titre of the diluted vinegar is 25.45 cm The reaction in the student's titration is shown below. 2CH,COOH(aq) + Ba(OH),(aq) (CH,COO),Ba(aq) + 2H,0(1) (i) Calculate the concentration, in moldm, of CH,COOH in the original bottle of vinegar

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

A student is asked to standardize a solution of barium hydroxide. He weighs out 0.934 g potassium hydrogen phthalate (KHC3H,04, treat this as a monoprotic acid). It requires 37.5 mL of barium hydroxide to reach the endpoint. A. What is the molarity of the barium hydroxide M solution? This barium hydroxide solution is then used to titrate an unknown solution of hydroiodic acid. B. If 22.7 mL of the barium hydroxide solution is required to neutralize 28.8 mL of hydroiodic acid, what is the molarity of the hydroiodic acid solution? M
Solid sodium sulfide is slowly added to 125 mL of a 0.0536 M iron(II) acetate solution. The concentration of sulfide ion required to just initiate precipitation is M.
A student prepares a dilute solution of sodium hydroxide, NaOH (aq), starting with 6 M sodium hydroxide. She then titrates a 1.372 g sample of KHP with the dilute sodium hydroxide solution, NaOH (aq), to a phenolphthalein end point. A.) If the titration required 21.84 mL of sodium hydroxide, NaOH (aq), calculate the molar concentration of the sodium hydroxide solution, NaOH (aq). (Remember that KHP is potassium hydrogen phthalate, KHC8H4O4, NOT potassium hydrogen phosphorus!) B.) The student uses the same sodium hydroxide to titrate 10.00 mL of vinegar to a phenolphthalein end point. If the titration required 27.48 mL of sodium hydroxide, NaOH (aq), calculate the molar concentration of acetic acid, HC2H3O2 (aq), in the vinegar. C.) Calculate the mass percent of acetic acid, HC2H3O2 (aq), in the vinegar using the molar concentration for acetic acid, HC2H3O2 (aq), determined in part b and assuming the density of the solution is 1.01 g/mL.
Determining the volume of base needed to titrate a given mas... A chemistry student weighs out 0.348 g of ascorbic acid (H,C,H,0), a diprotic acid, into a 250. mL volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.1800M NaOH solution. Calculate the volume of NaOH solution the student will need to add to reach the final equivalence point. Round your answer to 3 significant digits. mL dla Explanation Check O 2021 McGraw-Hill Education. All Rights Reserved Terms of Use Privacy Accessibility MacBook Air
25 mL of a bleach (NaOCl) sample is diluted to 500 mL. An excessive amount of KI is added to the 20 mL solution taken from here and the I2 released is titrated with 35.5 mL of 0.0409 M NaS2O3. Accordingly, calculate the percent by volume of NaOCl in the sample (MaNaOC: 74.4 g/mol) A. %10,50 B. %15,75 C. %5,25 D. %20,85
Use the solubility rules to predict whether the following ionic compounds are soluble in water: (a) AgCl; (b) AgNO3; (c) Ca(NO3)2; (d) Ca(OH)2. (a) insoluble (b) soluble (c) soluble (d) soluble 8
A lifeguard spills 160.43 mL of 0.877 M hydrochloric acid (also known as muriatic acid) solution while sanitizing a pool. How many milliliters of 0.6 M sodium carbonate must be poured on the spill to neutralize the hydrochloric acid? (Hint: Enter your answer to the ones place) 2 HCl(aq) + Na2CO3(s) -> H2O(l) + CO2(g) + 2 NaCl(aq)
4. Sodium hydroxide solution was standardized against one gram of potassium acid phthalate. First trial used 52.0 ml of the solution while the second trial used 52.4 of the solution to reach the end point. Determine: (a) the standardized concentration of the solution? (b) the percent accuracy if you are going to prepare a one tenth of a molar solution The standardized basic solution was then used in getting the total acidity of a food sample. Ten milliliter of the acidic sample consumed 10.3mL in the first trial then 10.0mL in the second trial to reach endpoint. Determine: (c) the normality of the acidic sample? Compute the total acidity of the food sample assuming that ten grams of sample was dissolved to 25ml of solution if the sample is: (e) Juice (MW, citric acid = 192.4; one mole citric acid reacts with three moles NaOH) If you are a food safety inspector, would the sample pass if (include reason) () The stomach can only withstand 0.39-1.1% citric acid?
A chemistry student needs to standardize a fresh solution of sodium hydroxide. She carefully weighs out 303 mg of oxalic acid, a diprotic acid that can be purchased inexpensively in high purity, and dissolves it in 250mL of distilled water. The student then titrates the oxalic acid solution with her sodium hydroxide solution. When the titration reaches the equivalence point, the student finds she has used 104.5 mL of sodium hydroxidesolution. Calculate the molarity of the student's sodium hydroxide solution. Round your answer to 3 significant digits.
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 0.491 g sample of sodium propanoate, NaC, H,O, , is added to a 55.0 mL sample of a 0.270 M solution of propanoic acid. Assume that no change in the volume of the solution occurs. How many moles of C,H,0, are present from the addition of sodium propanoate? mol C,H,05 = mol What is the volume of solution in liters? volume solution = What is the concentration of the propanoate ion, C,H,0, (aq), in the solution? [C,H,O,] = M
Solid potassium hydroxide is slowly added to 175 mL of a 0.0631 M magnesium acetate solution. The concentration of hydroxide ion required to just initiate precipitation is М.