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A: We will use stoichiometry of the reaction to get the answer.
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Q: 1. A 20.00-mL sample of aqueous oxalic acid, H2C2O4, was titrated with a 0.09113-M solution of…
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Q: Titration of 0.2342 g of pure Na,C,O, (134.0 g/mol) required 13.45 ml of KMNO, solution according to…
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- An artificial fruit beverage contains 12.0 g of tartaric acid, H2C4H4O6, to achieve tartness. It is titrated with a basic solution that has a density of 1.045 g/cm3 and contains 5.00 mass percent KOH. What volume of the basic solution is required? (One mole of tartaric acid reacts with two moles of hydroxide ion.)You are given four different aqueous solutions and told that they each contain NaOH, Na2CO3, NaHCO3, or a mixture of these solutes. You do some experiments and gather these data about the samples. Sample A: Phenolphthalein is colorless in the solution. Sample B: The sample was titrated with HCl until the pink color of phenolphthalein disappeared, then methyl orange was added. The solution became pink. Methyl orange changes color from pH 3.01 (red) to pH 4.4 (orange). Sample C: Equal volumes of the sample were titrated with standardized acid. Using phenolphthalein as an indicator required 15.26 mL of standardized acid to change the phenolphthalein color. The other sample required 17.90 mL for a color change using methyl orange as the indicator. Sample D: Two equal volumes of the sample were titrated with standardized HCl. Using phenolphthalein as the indicator, it took 15.00 mL of acid to reach the equivalence point; using methyl orange as the indicator required 30.00 mL HCl to achieve neutralization. Identify the solute in each of the solutions.Chromium(III) chloride forms many compounds with ammonia. To find the formula of one of these compounds, you titrate the NH3 in the compound with standardized acid. Cr(NH3)xCl3(aq) + x HCl(aq) x NH4+(aq) + Cr3+(aq) + (x + 3) Cl(aq) Assume that 24.26 mL of 1.500 M HCl is used to titrate 1.580 g of Cr(NH3)xCl3. What is the value of x?
- Potassium hydrogen phthalate (KHPKHP) is often used as a primary standard in acid–base titrations. If 20.05 mL NaOH20.05 mL NaOH is required to neutralize 0.397 g KHP,0.397 g KHP, what is the concentration of the NaOH?5 b) Benzoic acid, HC7H5O2, is a weak monoprotic acid. A stock HC,H5O2 solution with unknown concentration was prepared. A 25.00 mL sample of the stock HCH5O2 solution was titrated with 0.1234 M sodium hydroxide to the equivalence point, using phenolphthalein as an indicator. The titration took 20.26 mL of titrant (sodium hydroxide). (b) Write a balanced complete ionic equation for the chemical reaction that occurs in this titration.5 a) Benzoic acid, HC-H5O2, is a weak monoprotic acid. A stock HC7H5O2 solution with unknown concentration was prepared. A 25.00 mL sample of the stock HC;H502 solution was titrated with 0.1234 M sodium hydroxide to the equivalence point, using phenolphthalein as an indicator. The titration took 20.26 mL of titrant (sodium hydroxide). (a) Write a balanced formula equation for the chemical reaction that occurs in this titration.
- In a titration of 20.37 mL of 0.1773 M H2SO4, 35.89 mL of a NaOH solution are needed. What is the concentration (in mol/L) of the NaOH solution? Include only the numerical answer (no units). In carrying out the first standardization in this experiment, a student used 0.5067 g of potassium hydrogen phthalate (KHP) and 24.97 mL of a NaOH solution are needed to reach the equivalence point. What is the concentration (in mol/L) of the student's NaOH solution? Include only the numerical answer (no units).Potassium hydrogen phthalate (KHP) is often used as a primary standard in acid–base titrations. If 19.45 mL NaOH is required to neutralize 0.442 g KHP, what is the concentration of the NaOH?A sodium hydroxide solution is standardized by titrating 0.8592 g of ordinary standard potassium hydrogen phthalate (204.22 g/mol) to a phenolphthalein end point, requiring 32.67 ml. What is the molarity of the NaOH solution? cO,K cO;K + NaOH + H,0 COH Pim yg pla
- A sample weighing 10.91 g containing an unknown amount of H3PO4 was diluted with water and titrated with a standardized concentration of 0.7255 M NaOH. The endpoint was reached after 27.03 mL of the titrant was added. What is the % H3PO4 (97.994 g/mole) in the sample? H3PO4 + 2 NaOH --> Na2HPO4 + 2H2O ROUND OFF FINAL ANSWER TO FOUR (4) SIG FIGSYou are running an acid-base titration with hydrochloric acid and calcium hydroxide. The calcium hydroxide is your titrant; it has a known concentration of 0.0891 M. You have added 25.0 mL of the hydrochloric acid solution to an Erlenmeyer flask along with 2 drops of phenolphthalein (fee’-nol-thay-leen) indicator. To begin your first trial, you fill a clean 50 mL buret with the calcium hydroxide solution. Your starting volume is 0.25 mL. After the addition of solution from the buret, you see a color change in the flask, and the end point of the reaction is reached. You note the final volume in the buret to be 18.75 mL. You begin again for your second titration trial. You add 24.8 mL of the hydrochloric acid solution to a clean flask along with 2 drops of indicator. You refill the buret to an initial volume of 1.42 mL. When the reaction is complete, you note the final volume in the buret at 16.74 mL. Then you complete a third trial. You add 25.6 mL of hydrochloric acid solution…7B-3. A 15.00 mL sample of an unknown perchloric acid solution is titrated with a 0.687 M barium hydroxide solution. It takes 29.31 mL of the base solution to reach the endpoint. а. Write a balanced chemical equation for the reaction that occurs. b. What is the molarity of the unknown acid solution?