If a 1.065 g sample of magnesium oxide of 84.736% were treated with 50 mL of 1.017 N sulfuric acid, what volume of 1.103 N sodium hydroxide would be required in the back titration? Question #1: What is the unknown volume?
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- help ASAP Compare the two quantities based on the given condition: A solution containing KOH and KHCO3 is titrated with 0.100 M HCl using a one-flask method. I. Volume of titrant from 0.00 mL to the phenolphthalein endpoint II. Volume of titrant from the phenolphthalein end point to the methyl red end point. (a) I < II (b) I = II (c) I > II (d) The two quantities cannot be compared due to insufficient information.4. A 0.2521-g sample of an unknown weak acid is titrated with a 0.1005 M NaOH, requiring 42.68 mL to reach the phenolphthalein end point. Determine the compound's equivalent weight. Which of the following compounds is most likely to be the unknown weak acid? Name Formula MM, g/mol Туре Ascorbic acid C6H8O6 176.1 Monoprotic Malonic acid C;H4O4 104.1 Diprotic Succinic acid C,H¿O4 118.1 Diprotic Citric acid C,H8O7 192.1 TriproticIn the titration of a volume of 50 mL of a hydrochloric acid solution with Solution density 1.045 g / mL; 29.71 mL of potassium hydroxide with a concentration of 1,963 M were needed, using phenolphthalein as an indicator. Calculate the% m / m of the hydrochloric acid.
- A student is conducting molecular weight determination of an unknown diprotic acid. He first prepared a 250 mL NaOH (39.997 g/mol) titrant solution, which he then standardized with 0.5830 g of KHP (204.22g/mol) which consumed 24.02 mL of the titrant. After standardization, he weighed 0.2108 g of unknown diprotic acid and the titration reached the endpoint at a volume of 21.58 mL. (a) What is the standardized concentration of the titrant? Choices: 0.1000 M 0.1189 M 0.1286 M 0.1419 M (b) What is the molar mass of the diprotic acid? Choices: 82.19 g/mol 137.68 g/mol 164.38 g/mol 195.37 g/molA student is conducting molecular weight determination of an unknown diprotic acid. He first prepared a 250 mL NaOH (39.997 g/mol) titrant solution, which he then standardized with 0.5830 g of KHP (204.22g/mol) which consumed 24.02 mL of the titrant. After standardization, he weighed 0.2108 g of unknown diprotic acid and the titration reached the endpoint at a volume of 21.58 mL. (a) What is the standardized concentration of the titrant? (b) What is the molar mass of the diprotic acid?#5: Titration of 0.1212 g of pure Na2C2O4 (134 g/mol) required 19.14 mL of KMnO4. What is the molarity of the KMnO4 solution? The net ionic equation for this reaction is: 2MnO4- + 5C2O42- + 16H+ ---> 2Mn2+ + 8H2O + 10CO2 Choices: 0.0189 M 0.0473 M 0.0722 M 0.1181 M
- 9:1. A 250.0-mg sample of an organic weak acid was dissolved in an appropriate solvent and titrated with 0.0556 M NaOH, requiring 32.58 mL to reach the end point. Determine the compound’s equivalent weight4) Students were asked to perform a lab to identify an unknown acid.The experiment has several parts. First the students had to make a sodium hydroxide solution with a molarity of approximately 0.2M. Then the students had to perform a titration with potassium hydrogen phthalate to standardize their solution. Finally they had to perform a titration with the unknown acid to find the pKa and the molar mass, then using theirdata they had to determine which of the weak acids they had used.Part 1) Make a sodium hydroxide solutionA student measured 4.03 grams of NaOH in a tared weigh boat. They then dissolved it into approximately 200 mL of deionizedwater in a beaker. Once it was completely dissolved the student poured the solution into a 500.0 mL volumetric flask. The student rinsed the beaker with deionized water and added the rinse water to the volumetric flask. They repeated with process, adding the rinse water to the volumetric flask again, they mixed this thoroughly. Finally, they…Use a primary standard to determine an unknown concentration using an acid-base titration. Potassium hydrogen phthalate is a solid, monoprotic acid frequently used in the laboratory as a primary standard. It has ths unwieldy formula of KHC3H,O. This is often written in shorthand notation as KHP. If 34.47 mL of a barium hydroxide solution are needed to neutralize 1.279 grams of KHP, what is the concentration (mol/L) of the barium hydroxide solution? M Check & Submit Answer Show Approach étv A hulu 20 ITA 44 F7 411 4A F10 DOO F8 F9 %24 4 %23 8. 6.
- Given the balanced equation: H2SO4 + Na2CO3 --> Na2SO4 + H2O + CO2 In a titration where H2SO4 is added from a buret to an aqueous solution of 0.850 g Na2CO3, 46.75 mL of H2SO4 are needed to reach the permanent endpoint of the titration. A) Find the number of moles of Na2CO3 in the reaction. B) Find the number of moles of H2SO4 in the reaction. C) Find the mass/mass % of H2SO4 based on the above information about reaching the endpoint of the titration. The molar mass of Na2CO3 is 105.99 g/mol. The molar mass of H2SO4 is 98.08 g/mol. The density of H2S04 is 0.985 g/mL.0.915g of KHP (204.22g/mol) was dissolved in 100ml of distilled water and titrated euth sodium hydroxide solution. 27.55ml titrant was needed to reach the equivalenec point. There is 0.00448 moles of KHP present in the sample. a) How many moles of sodium hydroxide are needed to neutralize each mole of KHP? b) Therefore, how many moles of NaOH were needed to neutralize the KHP sample? c)What is the molar concentration (mol/L) of the sodium hydroxide solution?A student performed titration to determine the concentration of potassium permanganate solution with oxalic acid. The net ionic equation is as follows: 2MnO4– + 16H+ + 5C2O42- → 2Mn2+ + 10CO2 + 8H2O The titration consumed 42.31 mL of 0.1001 M oxalate solution to reach the endpoint. Determine the concentration of permanganate (M) if 25 mL was used.