A 8.90 g sample of benzoic acid was dissolved in water to give 61.4 mL of solution. This solution was titrated with 0.360 M NaOH. What was the pH of the solution when the equivalence point was reached? K, of benzoic acid is 6.3 x 10. pH =
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- A 0.5131-g sample that contains KBr (MM: 119.0023) is dissolved in 50 mL of distilled water. Titrating with 0.04614 M AgNO3 requires 25.13 mL to reach the Mohr end point. A blank titration requires 0.65 mL to reach the same end point. Report the %w/w KBr in the sample.Silver nitrate can be standardized using primary standard KCl. A dried sample of analytical grade KCl of mass 0.918 g was dissolved and diluted to 250.0 mL. Repeat 10.00-mL aliquots of the potassium chloride solution were titrated with the silver nitrated solution. The mean corrected titration volume was 8.98 mL Calculate the molarity (M) of the silver nitrate solution.A 0.500-g sample containing BaBr2 (FM = 297.14) is dissolved in 50 mL of distilled water. Titrating with 0.0400 M AgNO3 requires 25.00 mL to reach the Mohr endpoint. A blank titration requires 0.50 mL to reach the same endpoint. Calculate the %w/w BaBr2 in the sample. Please provide a complete solution.
- Please Calculate the mass of sodium acetate trihydrate (CH3COONa●3H2O) solid and thevolume of 1.00 M acetic acid (CH3COOH) required to make 250.0 mL of 0.500 M buffer, pH 5.00. Thank you!100.0 mL of 0.050 M NH3 is titrated with 0.10 M HCl. Calculate the pH for each point during the titration. (The Kb of NH3 is 1.8 X 10-5) Show work below and put final pH values here. A) After 60.0 mLof HCl is added. pH=If we use 13.75 mL of the solution above to reach the endpoint titrating 15.00 mLof a 0.200 M HCI solution according to the reaction below, what is the working (actual) concentration of the NaOH solution? (do not forget about SF)
- A mixture containing only KCl and NaBr is analyzed by the Mohr method. A 0.3172-g sample is dissolved in 50 mL of water and titrated to the Ag,CrO4 end point, requiring 36.85 mL of 0.1120 M AgNO3. A blank titration requires 0.71 mL of titrant to reach the same end point. Report the %w/w KCl and NaBr in the sample.0.9350g of an impure solid containing oxalic acid was dissolved and diluted to 100.00mL. From this bulksolution 8.00mL samples were titrated with 0.01267M KMnO4, resulting in an average titration volumeof 24.55mL. The molar mass of oxalic acid is 90.0349 g/mol. determine the mass %! Thank you!Students Mola and Rity were tasked to analyze the acidity of a 10.0-mL fermented milk sample diluted with water in a 250-mL volumetric flask. Mola obtained a 15.0-mL aliquot of this solution, diluted it to 50.0 mL, and then titrated this diluted sample. Titration data were given to Rity and she found out that the 50.0-mL diluted sample contains 0.21 mmol of lactic acid. MW: Lactic Acid (90.08) a. What is the lactic acid concentration (in M) of the titrated sample? b. Determine the lactic acid content (in M) of the 10.0-mL fermented milk sample. c. What is the lactic acid concentration (in %w/v) of the 10.0-mL fermented milk sample?
- Weak acid HMa (0.150 M) has 65.00 mL is titrated with 0.15 M NaOH. The Kaminoan scientist adds 30.00 mL. The acid dissociation of acid HMa is 3.9 x 10-4 Determine the pH of the resulting solutionA titration experiment, using 0.0175M Ba(OH)2 just neutralized 14.5 ml of HNO3 solution. Calculate the molarity of the HNO3 solution. The titration data is below /9 Titration data of Ba(OH)2 Burette Reading Trial 1 Trial 2 Trial 3 Initial Vol (mL) 0 13.01 25.22 Final Vol (mL) 13.01 25.22 37.5Explain your reasoning, thank you! You find 5.00 g of an acid (C7H5O2H) and 5.00 g of a salt (KC7H5O2) in the lab and decide to prepare a 1.00 L buffer solution using these chemicals. Explain how to prepare a buffer at a pH of 4.0 with a maximum buffer capacity using the chemicals available. Ka = 6.46×10-5. Show all of your work and calculations and be sure to explain how many grams of each chemical should be used.