A 0.1500-M solution Ba(OH)2 was used to titrate a cleaning solution containing acetic acid. A 50.00-mL sample used 43.40 mL Ba(OH)2. Calculate the %w/v of acetic acid in the sample.
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- A vinegar solution was prepared by diluting 25.00 mL of vinegar to 250.0 mL. From this solution, 50.00 mL portion was taken, and this required 30.00 mL of 0.1000M NaOH solution to reach neutralization end point. What is the percentage (w/v) of HOAc in the sample? Mol wt HOAc = 60.0 g/molA solution containing AgNO3 is mixed with a solution of NaCl to form a solution that is 0.10 M in AgNO3 and 0.075 M in NaCl. What will happen once these solutions are mixed? Given: Ksp (AgCl) = 1.77 x 10-10In standardizing a solution of NaOH against 1.431g of KHC8H4O4, the analyst uses 35.50 mL of the alkali and has to run back with 5.12 mL of acid ( 1mL ≎0.0031g Na2O) What is the normality of NaOH?
- *** CALULATE FINL CONCENTRATION USING 2 IG FIGS AND APPROPRIATE UNITS A 6.0 mLmsample of a 50.0 % (mm/vv) acetic acid (HC2H3O2) solution is added to water to give a final volume of 34 mL.If a buret of 15mL of standardized 0.0024 M K2CrO4 was added to a clean 100mL volumetric flask and diluted to the 100mL mark with NaNO3. What will be the concentration of CrO42- in the solution. Please show all the steps when solving. ThanksIn one trial determination of the concentration of NaOCl in the diluted bleach sample, 10.00 mL of the diluted bleach solution required 23.32 mL of 0.0195 M Na2S2O3 titrant to reach the endpoint. What is the molar concentration of NaOCl in the diluted bleach solution?
- A 14.00 mL sample of sulfuric acid is diluted to 50.00 mL. A 10.00 mL aliquot is titrated to a phenolphthalein endpoint with 42.80 mL of 0.1020 M NaOH. What is the molarity of the original solution.A 125-mL aqueous solution contains 0.421 g NaH2PO4, 0.786 g CaCl2, and 2.45 mL acetone. a. What is % m/v of NaH2PO, in the solution? b. What is the %v/v of acetone in the solution? c. What is the % m/m of CaCl2 in the solution? p of solution = 1.02 g/ml.Dr. Donwonree tried to determine the vitamin C content in apple juice which he bought at CheMarket. He measured out 50.0 mL of the juice and added the HCl, KI, and starch. Then he started the titration by adding KIO3 solution into the juice. The concentration of the KIO3 solution was 0.200 M and it took only 1.50 mL of KIO3 to reach the endpoint. How much vitamin C (mg) is contained in 1.00 L of this apple juice?
- What is Molarity of a 5.00% (v/v) acetic acid ? Density of pure acetic acid is 1.05 g/mL. MM Acetic Acid: 60.05 g/molIn standardizing a solution of NaOH against 1.431g of KHC8H4O4, the analyst uses 35.50 mL of the alkali and has to run back with 5.12 mL of acid (1mL = 0.0031g Na20) What is the normality of NaOH? Additional instructions: Make it handwritten Include up to 4 decimal places Please include explanations of the process Thank you so much!Which of the following is a strong electrolyte? a. 70% v/v ethanol b. 1.0 M citric acid c. 10.0 mL, 1.0 M Mg(OH)2 and 10.0 mL, 1.0 M HNO3 mixture d. Glacial acetic acid