In the laboratory a student combines 27.0 mL of a 0.109 M potassium bromide solution with 25.3 mL of a 0.343 M ammonium bromide solution.. What is the final concentration of bromide anion ? M Submit Answer Retry Entire Group 9 more group attempts remaining
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- 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 weight percent by volume of NaOCl in the sample. (Ma(NaOC:74,4 g/mol)A 6.00-mL portion of an 8.00 M stock solution is to bediluted to 0.400 M. What will be the final volume afterdilution?When 25.00 mL of unknown were passed through a Jones reductor, molybdate ion (MoO4^2-) was converted into Mo3+. The filtrate required 16.43 mL of 0.010 33 M KMnO4 to reach the purple end point. MnO4- + Mo3+ --> Mn2+ + MoO2^2+. A blank required 0.04 mL. Balance the reaction and find the molarity of molybdate in the unknown.
- It is required to know the concentration of an aqueous solution of H2SO4 that appeared in the laboratoryChemistry III and it's unlabeled. To this end, a student of analytical chemistry carried out the followingProcedure: He took 5.00 mL of a fresh and standardized solution of 0.525M NaOH and brought them to a250.0 mL balloon to be completed with distilled water. Subsequently, he poured 15.00 mL of the solutionH2SO4 of unknown concentration in an Erlenmeyer flask and added 2 drops of phenolphthalein.Using a burette filled with the last NaOH solution, he noticed that when adding 39.40 mL of the hydroxidethe Erlenmeyer solution reached a faint but permanent pink. With the above dataDetermine the concentration and pH of the H2SO4 solution.Solve the following problem: Zinc in a 0.7457 g sample of foot powder was titrated with 22.57 mL of 0.01639 M EDTA. Calculate the percentage of Zinc in this sample.A 1.025 g sample containing Cl- is analyzed through the Mohr method. The sample is dissolved in 250 mL of water, and a 50mL aliquot is taken, and it consumed 25.0mL of 0.100 M AgNO3. Calculate the: a. milliequivalent Cl gram Cl b. percentage Cl on the sample
- 400 g sample containing chloride ions (MW=35.45 g/mol) was dissolved in 50.0mL of distilled water. A 15.0 mL aliquot was taken, and was further diluted to 50.0 mL using distilled water. The diluted solution was then titrated using a 0.0989 M AgNO3 solution, and it consumed a total of 31.9 mL of the titrant in order to reach the end point. What is the concentration of the undiluted chloride solution? Round off to three (3) significant figures. What is the % (w/v) concentration of the undiluted chloride solution? Round off to two (2) decimal points. What is the % (w/w) of Cl- composition of the sample? Round off to two (2) decimal points.Shana, a student in the Analytical Chemistry class, performed a Redox Titration to determine the content of hypochlorite ions (% w/w) in an unknown solution. First, Shana prepared a primary standard solution of KIO3 by dissolving 0.4791 g dry KIO3 in 250.00 mL DI water. Next, using the procedure in your lab manual, Shana used 50.00 mL of this primary standard solution to standardize the Na2S2O3 titrant, and 26.25 mL of titrant was consumed. Next, Shana prepared the unknown solution by diluting 12.8624 g of the solution in 250.00 mL of DI water. A 50.00 mL portion of this dilute unknown solution was titrated using the procedure in your lab manual, and 19.25 mL of Na2S2O3 solution was consumed. Answer the following questions about this titration. Recall the stoichiometry of the NET chemical equation for this reaction. Note: use appropriate significant figures in your answer! A. Calculate the concentration (M) of Na2S2O3 titrant. B. Determine the amount (g) of hypochlorite ion in 50.00 mL…How many milligrams of MgI2 must be added to 275.0 mL of 0.0788 M KI to produce a solution with [I−] = 0.1000 M?
- What volume of concentrated ammonia should be used to prepare 200 ml of 0.600 M solution?Purity 28% w/wdensity 0.9 g/ml4. Ascorbic acid (Vitamin C, MW = 176.126g/mol) is a reducing agent, reacting as follows: C6H8O6 C6H6O6 + 2H+ + 2e- It can be determined by oxidation with a standard solution of I2. A 200.0-mL sample of a citrus fruit drink is acidified, and 10.00mL of 0.0500 M I2 is added. After the reaction is complete the excess I2 is titrated with 38.62 mL of 0.0120 M Na2S2O3 . Calculate the number of milligrams of ascorbic acid per milliliter of fruit drink. I2 +2e 2I- I2 + 2Na2S2O3 2NaI + Na2S4O6A 30 ml solution of I- was treated with 50 ml of 0.365 M AgNO3. The resulting AgI precipitate was filtered. The resulting filtrate was back-titrated with 37.60 ml of 0.287 M KSCN. According to these data, how many grams of I- are in the sample? (I:127) (Ag:107,86),(N:14),(O:16),(K:39,098),(C:12,011),(S:32,066)