1. When H2SO4(aq) was reacted with NaOH(aq) in the titration, why was a precipitate not formed? 2. What do we mean by standardization of an aqueous solution of H2SO4? 3. In this acid-base titration, what did we use to measure the volume of the H2SO4(aq)?
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- What does it mean to standardize the KMnO4 solution? In the titration, which substance is reduced and oxidized? What is the mole ratio of MnO4-/C2O42- in the chemical reaction in this experiment? What is the purpose of the 3 M H2SO4 solution? What is the purpose of the manganese (II) sulfate? Why is it necessary to titrate slowly in this experiment?A 44.6 mL of 0.103 M HCI is added to an antacid sample. The solution is titrated to a bromophenol blue endpoint using 19.8 mL of 0.0998M NaOH. How many moles and how many grams of the base are in the antacid sample? Assume the active ingredient is MgCO3. Moles of NaOH? Moles of HCl? Moles of MgCO3? Mass of MgCO3?What is the value of pH for the soultion of CH3COOH and NH3 and why? In other words, in tittration reaction between CH3COOH and NH3, which value will i get in equivalence point?
- 0.9563 g KHCO3 (M.r.(KHCO3) = 100.12 g/mol (mg/mmol)) have measured, and 50.0 cm3 stock solution have been prepared from it. 10.00 cm3 individual samples from it was titrated with HCl titrant in order to determine its concentration. The average HCl consumption was 19.18 cm3. The same HCl solution with were used to determine the concentration of NaOH titrant. The base consumption for 20.00 cm3 HCl was 21.35 cm3 NaOH. 1. concentration of HCl 2. concentration of NaOHFor the adjustment of 0.1 M HCl standard solution, 0.1345 g Na2CO3 in primary standard purity was weighed, dissolved in 50 mL of distilled water and titrated with HCl solution. As a result of the titration, 14 mL of acid solution was consumed. Accordingly, what is the true concentration of the HCl solution?a. Which anion or anions may be present in an acidic solution that forms precipitate upon addition of AgNO3(aq)? b. Which anion or anions may be present in a neutral solution that forms a pale yellow precipitate upon addition of AgNO3(aq)?
- During the titration of an HClO4 solution with 0.10320 M NaOH, a student, Lovely became distracted and overshot the endpoint. A fellow student Ashley suggested that he should record the present volume of NaOH added and titrate the excess with a standard acid solution. If the original sample volume was 25.000 mL, the volume of NaOH added was 28.060 mL. It took 3.4700 mL of 0.10940 M HCl to back-titrate the NaOH and calculate the molar concentration of the original HClO4The protein content of wheat flour can be determined reasonably accurately by multiplying the percentage of nitrogen present by 5.7. A 2.06-g sample of flour was taken through a Kjeldahl procedure and the ammonia produced was distilled into a boric acid solution. If this solution required 34.70 mL of 0.174 N HCl for titration to the methyl red end point, what is the a) % Nitrogen and b) % protein in the flour? (Use 1:1 stoich ratio between N and HCl)what is the Molarity of the NaOH solution? Mass of H2C2O4·2H2O=1.32191 g Volume of the H2C2O4·2H2O solution=250.0 mL Volume of NaOH solution used in titration=21.45 mL
- The standardization of iodine solution was conducted using 10.0 mL of a standard 1.00 mg/mL ascorbic acid solution. Titration with the iodine solution required 17.50 mL to reach the end point. I2(aq)+C6H8O6(aq)⟶C6H6O6(aq)+2H+(aq)+2I−(aq)I2(aq)+C6H8O6(aq)⟶C6H6O6(aq)+2H+(aq)+2I−(aq) What is the molarity of the iodine solution?Briefely explain the meaning of the following terms as they relate to this experiment. a) Titration b) end point c) indicator d) Standard solution e) meniscusa. Why was HCl added to the unknown sulfate solution before adding the BaCl2 solution? b. Suppose that a small portion of the sulfate precipitated as lead sulfate rather than as barium sulfate. How would this change the result of the analysis?