In the acetic ačid determination in vinegar experiment; NaOH was standardized with 0.35 g KHP (molar mass = 204.22 g/mol). The KHP was dissolved in 75.0 mL distilled water in a 250 mL Erlenmeyer flask and titrated to the endpoint colour by dispensing 17.10 mL of NaOH from the burette. Calculate the molarity of NaOH. O a. 0.35 M O b. 0.25 M Oc. 0.15 M

In the acetic ačid determination in vinegar experiment; NaOH was standardized with 0.35 g KHP (molar mass = 204.22 g/mol). The KHP was dissolved in 75.0 mL distilled water in a 250 mL Erlenmeyer flask and titrated to the endpoint colour by dispensing 17.10 mL of NaOH from the burette. Calculate the molarity of NaOH. O a. 0.35 M O b. 0.25 M Oc. 0.15 M

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...

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Introductlon In Part (a) of this experiment you will prepare a primary standard. Potassium hydrogen phthalate (KHP) is a monoprotic acid with the formula KHC,H.O. In this experiment KHP is used as the primary standard. A standard solution is one whose solute concentration is accurately known. If a solute can be obtained in a very pure, stable, weighable form, a primary standard solution of it can be prepared directly. You will then use the standardized sodium hydroxide solution to determine the acetic acid content of a dilute unknown solution. Procedure (0) Preparation of a Primory Standard Potassium hydrogen phthalate (KHP) is a primary standard. Weigh accurately by difference, approximately 0.8 g of KHP in a clean, dry weighing bottle and transfer it into a 250 ml conical flask. Add 75 ml of distilled water. Swirl gently. Cover the flask and leave to dissolve, swirling periodicaly. Cautlon: KHP is not highly soluble and care must be taken to ensure it is all dissolved before you…
A solid containing tris was dissolved in water and brought to a total volume of 50.00 ml. A 10.00 ml aliquot of the solution was titrated with 0.09978 M HCl to a bromcresol green endpoint. The aliquot consumed 38.93 ml of titrant. Calculate the weight of tris in the original sample.
Mean titre is 16.86 2 reading were taken.
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a primary standard of (COOK)2.H2O was prepared up to 0.05M. This primary standard was then titred against an unknown concentration of 50cm3 of KMnO4. An average titre value of 13 was obtained. The balanced equation is as follows: 5(COOK)2.H2O + 2KMnO4 + 8H2SO4 = 6K2SO4 +2MnSO4 + 10CO2 +18H2O. Find the concentration of the KMnO4.
MAX OF 15 MINUTES A solution contains NaOH (FM = 40), NaHCO3 (FM = 84), and NazCO; (FM = 106), either alone or in a permissible combination. Titration of a 50 mL portion to a phenolphthalein end point requires 16.3 mL of 0.100 M HCI. A second 50.0-mL aliquot requires 38.2 mL of the HCI when titrated to a bromocresol green end point. %3D %3D What is the % w/w composition of the following? Express answers in two decimal places. If the component is not present, write 0.00 in the answer box. NAOH: NazCO3: NaHCO3: 96
Extraction of DNA involves the use of a 1 M phosphate buffer (1-liter volume) having the hydrogen ion concentration of 6.165950019 x 10-9 M. Three pKa of phosphoric acid are available Concentrated phosphoric acid (85% w/w; Sp. Gr. = 1.70; MW = 98 g/mol) Sodium dihydrogen phosphate monohydrate (MW = 138g/mol) Sodium biphosphate heptahydrate (MW = 268g/mol) Tribasic sodium phosphate monohydrate (MW = 182 g/mol) Sodium hydroxide pellets (40 grams/mol) Question: What is the pH of the solution? (answer in two decimal places) How much of the weak acid component should be used? (Note for answer: Round to the nearest hundredth and include the unit such as "grams or milliliters"; Ex. 100.00 grams or 100.00g for weight & 100.00 milliliters or 100.00 mL for volume) Question: What is the suitable buffer component to be used? (Note for the answer: Separate the two components with “and”; Ex: Ammonia and Ammonium chloride) Question: How much of the salt component should be used?…
1)A bottle of concentrated aqueous sulfuric acid, labeled 95.00 wt% H2SO4, has a concentration of 16.5 M. Calculate the density of 95.00 wt% H2SO4. 2)Ascorbic acid in 5 vitamin C tablets was measured by a titration against (100 ± 0.002 M) NaOH solution. It required 10.00 ± 0.05 mL NaOH solution to reach the equivalent point. What is the average quantity of ascorbic acid per vitamin tablet?
Calculate the mass percent of the ascorbic acid in the same show full solution Situation: The pounded Vitamin C tablet was half into two below are the calculated data in the experiment. Each of the half are transfered in a 250ml erlen meyer flask and added 75ml of deionized water for the vitamin C to dissolve. Then it was prepared for titration where the burette was filled with 0.09794M standardize NaOH solution then a total of with 3 drops 2% phenolphthalein indicator was added to each erlen meyer flask l, swrill it and begin the titration. below are the following data gathered: Vitamins used: Nature Made vitamin C 500mg tablet Trial 1 Mass: 0.3108g of Vitamin C tablet Initial volume: 1.6mL Final volume: 15.4mL Trial 2 Mass: 0.3349g Initial volume: 15.4 mL Final volume: 30.2 mL
4- A sample containing H2C204 had a purity equal to 90.50% (w/w). An unknown mass of this sample was dissolved in water and transferred to a 50.00 mL flask. An aliquot of 25.00 mL was transferred to an erlenmeyer flask and 50.00 mL of a 0.2000 mol L^-1 NaOH solution were added. %3 Excess NaOH was titrated with 0.09000 mol L^-1 HCI solution using 2.000 mL. Calculate the mass (g) of the sample used. Data: H = 1.008 C= 12.01 O = 16.00
250.0 ml of the mineral water sample was precipitated with potassium sodium tetraphenyl bromate: K+ + B(C6H5)4-  KB(C6H5)(s). The precipitate was filtered, washed and dissolved in an organic solvent. An excess of HgY2- was added to the solution: 4 HgY2- + B(C6H5)4- +4H2O  H3BO3 + 4C6H5Hg+ + 4HY3- + OH-. The liberated EDTA was titrated with 0.05581 M Mg 2+ solution, which consumed 29.64 mL. Calculate the potassium concentration [mg/l] in the sample.
The standardization of same titrant during the determination of BOD5 of water sample was done separately for Day 1 and Day 5. Upon standardization, it turned out that the concentration of the titrant in Day 1 is higher than the concentration of the same batch of titrant in Day 5. How would you explain this discrepancy? (A) There were bubbles at the tip of the burette during titration. (B) Too much starch indicator was added in the conical flask. Sulfuric acid was added first before potassium iodide. (D) The water used to prepare the Na₂S₂O3 solution was not boiled resulting to proliferation of bacteria.