A 25-mL sample of 0.160M solution of NaOH is titrated with 17 mL of an unknown solution of H2SO4 What is the morality of the sulfuric acid solution

39,002 results
  1. AP Chemistry

    An unknown amount of water is mixed with 350 mL of a 6 M solution of NaOH solution. A 75 mL sample of the resulting solution is titrated to neutrality with 52.5 mL of 6 M HCl. Calculate the concentration of the diluted NaOH solution. Answer in units of M

  2. Chemistry

    15.00mL sample of a solution of H2SO4 of unknown concentration was titrated with 0.3200 N NaOH. The titration required 21.30mL of the base. What was the normality of the acid solution? what was the molarity of the acid solution?

  3. AP Chemistry

    An unknown amount of water is mixed with 350 mL of a 6 M solution of NaOH solution. A 75 mL sample of the resulting solution is titrated to neutrality with 52.5 mL of 6 M HCl. Calculate the concentration of the diluted NaOH solution. Answer in units of M I

  4. chemistry

    A 27.00 mL sample of an unknown H3PO4 solution is titrated with a 0.110 M NaOH solution. The equivalence point is reached when 25.78 mL of NaOH solution is added. What is the concentration of the unknown H3PO4 solution? The neutralization reaction is:

  5. Chemistry

    Commercial vinegar was titrated with NaOH solution to determine the content of acetic acid, HC2H3O2. For 20.0 milliliters of the vinegar 26.7 milliliters of 0.600-molar NaOH solution was required. What was the concentration of acetic acid in the vinegar if

  6. Chemisty

    A 25-mL sample of 0.160M solution of NaOH is titrated with 17 mL of an unknown solution of H2SO4. What is the molarity of the sulfuric acid solution? A. 0.004M H2SO4 B. 0.235M H2SO4 C. 0.117M H2SO4 D. 0.002M H2SO4

  7. Chemistry

    A 0.179 g sample of a vitamin C tablet was titrated with 0.1000 M NaOH according to the procedure in this experiment. The titration required 7.08 mL of NaOH solution. How many moles of NaOH were used in the titration? How Many moles of Vitamin C were in

  8. chem

    An impure sample of (COOH)2 ·2 H2O that has a mass of 3.4 g was dissolved in water and titrated with standard NaOH solution. The titration required 42.7 mL of 0.156 molar NaOH solution. Calculate the percent (COOH)2 · 2 H2O in the sample. Answer in units

  9. Chem

    A 20.00−mL sample of an unknown HClO 4 solution requires titration with 22.92mL of 0.2200M NaOH to reach the equivalence point. What is the concentration of the unknown HClO 4 solution? The neutralization reaction is: HClO 4 (aq)+NaOH(aq)¨H 2

  10. Chemistry

    A .288 g sample of an unknown monoprotic organic acid is dissolved in water and titrated with a .115 M sodium hydroxide solution. After the addition of 17.54 mL of base, a pH of 4.92 is recorded. The equivalence point is reached when a total of 33.83 mL of

  11. Chemistry

    An unknown amount of water is mixed with 350 mL of a 6 M solution of NaOH solution. A 75 mL sample of the resulting solution is titrated to neutrality with 51.2 mL of 6 M HCl. Calculate the concentration of the diluted NaOH solution. Answer in units of M

  12. Chemistry

    A 29.00 mL sample of an unknown H3PO4 solution is titrated with a 0.100 M NaOH solution. The equivalence point is reached when 24.63 mL of NaOH solution is added? What is the concentration of the unknown H3PO4 solution? The neutralization reaction is

  13. chem-please help!!!!!

    when a 25.0 mL sample of an unknown acid was titrated with a 0.100 M NaOH solution. Determine Ka for the unknown acid. Volume NaOH = 25 mL; pH=8.25

  14. chemistry

    A 125.0 mg sample of an unknown, monoprotic acid was dissolved in 100.0 mL of distilled water and titrated with a 0.050 M solution of NaOH. The pH of the solution was monitored throughout the titration, and the following data were collected. Determine the

  15. Chemistry

    1. You have been given a sample of unknown molarity. Calculate the molarity of a solution which has been prepared by dissolving 8.75 moles of sodium chloride in enough water to produce a solution of 6.22l. 2. You have a sample which consists of 428g sodium

  16. Chemistry

    A sample of 1.018 g of KHP (potassium hydrogen phthalate, molar mass = 204.22 g/mol) was dissolved in ~ 25 mL distilled water and titrated with a NaOH solution of unknown concentration. If 28.69 mL of base was used to reach the endpoint, what was the

  17. Chemistry

    Expt #1- Molecular Weight of Unknown Acid Unknown Acid: #2 Mass of Unknown solid acid transferred:0.414g Volume of volumetric flask: 100.00 mL Concentration of NaOH: 0.0989 M Aliqot of acid titrated with NaOH: 25.00 mL Average volume of Naoh from

  18. General Chemistry

    A 0.179 g sample of a vitamin C tablet was titrated with 0.1000 M NaOH according to the procedure in this experiment. The titration required 7.08 mL of NaOH solution. How many moles of NaOH were used in the titration?

  19. chem help w/ Lab

    Weight of the mustard package Sample: 3.02 (g) Weight of the mustard package Solution: 33.3 (g) Trial #1 Trial #2 Trial #3 Weight of Mustard Package Solution Delivered (g) : 1.09 .948 .909 Weight of NaOH Solution Delivered (g) : .354 .304 .269

  20. CHECK MY CHEMISTRY WORK PLEASE ASAP

    1. You have been given a sample of unknown molarity. Calculate the molarity of a solution which has been prepared by dissolving 8.75 moles of sodium chloride in enough water to produce a solution of 6.22l. 2. You have a sample which consists of 428g sodium

  21. ap chemistry

    please explain titration problems. I'm a total noob at this and am trying to answer some prelab questions. Examples: 1. How many mL of a 0.800 M NaOH solution is needed to just neutralize 40 mL of a 0.600 M HCl solution? 2. You wish to determine the

  22. Chemistry

    A 0.5224g sample of an unknown monoprotic acid was titrated with 0.0998M of NaOH. The equivalence point of the titration occurs at 23.82 mL. Determine the molar mass of the unknown acid.

  23. College Chemistry

    The Question Is: "A student weighs 0.347 g of KHP on a laboratory balance. The KHP was titrated with NaOH and the concentration of the NaOH determined to be 0.110 M. For the second titration, the student correctly diluted 6 M HCl from the reagent shelf

  24. chemistry

    A 15.0 ml sample of an unknown HClO4 solution requires 50.3 ml if 0.101 M NaOH for complete neutralization. What was the concentration of the unknown HClO4 solution? The neutralization reaction is: HClO4(aq)+ NaOh(aq)yields H2O(l)+ NaClO4 (aq) If anyone

  25. chem

    A 26.8 mL sample of an unknown HClO4 solution requires 46.8 mL of 0.101 M NaOH for complete neutralization. What was the concentration of the unknown HClO4 solution? The neutralization reaction is shown below. HClO4(aq) + NaOH(aq) H2O(l) + NaClO4(aq) i got

  26. Chemistry

    Tartaric acid has two acidic (ionizable) hydrogens. The acid is often present in wines and precipitates from solution as wine ages. A solution containing an unknown concentration of the acid is titrated with NaOH. It requires 22.62 mL of 0.2000 M NaOH

  27. Chemistry

    A 25-mL sample of 0.160M solution of NaOH is titrated with 17 mL of an unknown solution of H2SO4 What is the morality of the sulfuric acid solution.

  28. College Chemistry

    1) A 25mL sample of the .265M HCI solution from the previous question is titrated with a solution of NaOH. 28.25mL of the NaOH solution is required to titrate the HCl. Calculate the molarity of the NaOH solution. 2) A 1.12g sample of an unknown monoprotic

  29. chemisry

    An unknown amount of water is mixed with 350 mL of a 6 M solution of NaOH solution. A 75 mL sample of the resulting solution is titrated to neutrality with 52.5 mL of 6 M HCl. Calculate the concentration of the di- luted NaOH solution. Answer in units of M

  30. CHEMISTRY

    n unknown amount of water is mixed with 350 mL of a 6 M solution of NaOH solution. A 75 mL sample of the resulting solution is titrated to neutrality with 52 . 5 mL of 6 M HCl. Calculate the concentration of the di- luted NaOH solution. Answer in units of

  31. chem--please help me!!

    when a 25.0 mL sample of an unknown acid was titrated with a 0.100 M NaOH solution. Determine Ka for the unknown acid. Volume NaOH = 12.5 mL; pH=3.80 please help me explain in details!!!

  32. Chemistry lab

    A 1.340gram sample of an unknown acid, H3A, was placed in a 250.0 mL volumetric flask and diluted to volume with water. A 45.35 mL sample of this acid solution was titrated with 37.77 mL of a 0.1006M NaOH solution. A) Using one set - up dimensional

  33. chemistry

    A 15.00 mL sample of an unknown monoprotic weak acid solution is titrated with 0.35 M NaOH. The initial buret reading is 0.23 mL. The phenolphthalein indicator turns the solution light pink when the buret reads 29.58 mL. A. what volume of 0.35 M NaOH was

  34. Chemistry

    1-A sample of potassium hydrogen oxalate, KHC2O4, weighing 0.717 g, was dissolved in water and titrated with 18.47 mL of an NaOH solution. Calculate the molarity of the NaOH solution. 2-A 35 mL drinking water sample, whose pH is buffered to 10, is titrated

  35. CHEMISTRY

    You have been given a sample of unknown molarity. Calculate the molarity of a solution which has been prepared by dissolving 8.75 moles of sodium chloride in enough water to produce a solution of 6.22l. 2. You have a sample which consists of 428g sodium

  36. Chemistry

    I there, this is my lab worksheet, I am having trouble filling it out. Please help me with it. Expt #1- Molecular Weight of Unknown Acid Unknown Acid: #3 Mass of Unknown solid acid transferred:1.0g Volume of volumetric flask: 100.00 mL Concentration of

  37. Chemistry

    A very old and tired , grey haired AP Chem instructor wanted to determine the Ka of an unlabelled monoprotic acid in his stockroom. He dissolved an unknown amount of acid in an unknown amount of water and proceeded to titrate the sample with a solution of

  38. AP Chemistry

    A very old and tired , grey haired AP Chem instructor wanted to determine the Ka of an unlabelled monoprotic acid in his stockroom. He dissolved an unknown amount of acid in an unknown amount of water and proceeded to titrate the sample with a solution of

  39. Chemistry

    A very old and tired , grey haired AP Chem instructor wanted to determine the Ka of an unlabelled monoprotic acid in his stockroom. He dissolved an unknown amount of acid in an unknown amount of water and proceeded to titrate the sample with a solution of

  40. chem

    A sample of potassium hydrogen oxalate, KHC204, weighing 0.717 g, was dissolved in water and titrated with 18.47 mL of an NaOH solution. Calculate the molarity of the NaOH solution.

  41. College Chemistry

    I need help with this question!! a sample of pure KHP weighing .8097g dissolved in water and titrated with 40.25 mL of NaOH solution. The same NaOH solution was used to titrate a solution of a weak diprotic acid H2X. A sample of 0.18694g of the weak acid

  42. chemistry help asap

    Please check these thanks. 1. In a titration, 33.21 mL 0.3020M rubidium hydroxide solution is required to exactly neutralize 20.00 mL hydrofluroic acid solution. What is the molarity of the hydrofluroic acid solution? Answer: 0.502HF 2. A 35.00 mL-sample

  43. College Chemistry

    "A student weighs 0.347 g of KHP on a laboratory balance. The KHP was titrated with NaOH and the concentration of the NaOH determined to be 0.110 M. For the second titration, the student correctly diluted 6 M HCl from the reagent shelf using a graduated

  44. chemistry

    If you pass 10.0mL of a 50.0mL solution of [Co(en)2Cl2]Cl that has been reduced with Zn through a cation exchange column, you will obtain a solution that has three H+ ions for every Co3+ ion that was originally present in the sample. These H+ ions are

  45. Chemistry

    An impure sample of (COOH)2 · 2 H2O that has a mass of 2.9 g was dissolved in water and titrated with standard NaOH solution. The titration required 32.4 mL of 0.144 mo- lar NaOH solution. Calculate the percent (COOH)2 · 2 H2O in the sample.

  46. chem

    An impure sample of (COOH)2 · 2 H2O that has a mass of 4.3 g was dissolved in water and titrated with standard NaOH solution. The titration required 44.5 mL of 0.11 mo- lar NaOH solution. Calculate the percent (COOH)2 · 2 H2O in the sample. Answer in

  47. Chemistry

    A 100.0 ml sample of .50 M HCl (aq) is titrated with a .10 M NaOH. What volume of the NaOH solution is required to reach the endpoint of the titration?

  48. College Chemistry (DrBob222)

    A solution of an unknown weak acid, HA, is titrated with 0.100 M NaOH solution. The equivalence point is achieved when 36.12 mL of NaOH have been added. After the equivalence point is reached, 18.06 mL of 0.100 M HCl are added to the solution and the pH at

  49. Chemistry

    A 5.00-mL sample of a sulfuric acid solution of unknown concentration is titrated with a 0.1401 M Sodium Hydroxide solution. A volume of 5.99 mL of the base was required to reach the endpoint. What is the concentration of the unknown acid solution? Write

  50. Chemistry

    A Student Performing a lab weighed a 1.0993g sample, containing an unknown KHP, which required 18.06mL of 0.1879M NAOH to reach the phenolphtalein endpoint. a) How many moles of base were consumed by the KHP in this sample? b) How many grams of KHP were

  51. AP Chemistry

    There is an unknown amount of unlabelled monoprotic acid in an unknown amount of water titrated with a sample with a solution of NaOH of unknown molarity. After adding 10.0 mL of NaOH, the pH=5.0. The equivalence point is 32.22 mL of NaOH. What is the Ka?

  52. Chemistry

    A 5.00-mL sample of an H3 PO4 solution of unknown concentration is titrated with a 0.1003 M NaOH solution. A volume of 6.55 mL of the NaOH solution was required to reach the endpoint. What is the concentration of the unknown H3 PO4 solution?

  53. chemistry help

    a 3.54 grams solid sample of an unknown monoprotic acid was dissolved in distilled water to produce a 47.0 mL solution at 25 degrees. This solution was then titrated with 0.2 M NaOH. The equivalence point was reached when 35.72 mL of 0.2 M NaOH was

  54. chemistry

    a 3.54 grams solid sample of an unknown monoprotic acid was dissolved in distilled water to produce a 47.0 mL solution at 25 degrees. This solution was then titrated with 0.2 M NaOH. The equivalence point was reached when 35.72 mL of 0.2 M NaOH was

  55. AP Chemistry

    A 5.0 M solution of HNO3 is titrated with 0.3 M NaOH. Identify the species that have the highest concenttrations in the solution being titrated halfway to the equivalence point. A 25.15 ml of 0.35 m HNO3 was titrated with an unknown concentration of NaOH.

  56. Chemistry

    An unknown amount of water is mixed with 310 mL of a 6 M solution of NaOH solution. A 75 mL sample of the resulting solution is titrated to neutrality with 58.2 mL of 6 M HCl. Calculate the concentration of the diluted NaOH solution. Answer in units of M

  57. Chemistry

    An unknown amount of water is mixed with 310 mL of a 6 M solution of NaOH solution. A 75 mL sample of the resulting solution is titrated to neutrality with 58.2 mL of 6 M HCl. Calculate the concentration of the diluted NaOH solution. Answer in units of M

  58. chemistry

    You weigh a sample of a monoprotic unknown acid and dissolve it in 50.00 mL of distilled water. Exactly half of this solution is titrated with Sodium Hydroxide to the phenolphthalein end point. The pH of the other half of the original solution is measured

  59. chemistry help

    A 15.00 mL sample of an unknown monoprotic weak acid solution is titrated with 0.35 M NaOH. The initial buret reading is 0.23 mL. The phenolphthalein indicator turns the solution light pink when the buret reads 29.58 mL. B. How many moles of NaOH were

  60. College Chemistry

    You weigh a sample of a monoprotic unknown acid and dissolve it in 50.00 mL of distilled water. Exactly half of this solution is titrated with Sodium Hydroxide to the phenolphthalein end point. The pH of the other half of the original solution is measured

  61. chemistry

    You weigh a sample of a monoprotic unknown acid and dissolve it in 50.00 mL of distilled water. Exactly half of this solution is titrated with Sodium Hydroxide to the phenolphthalein end point. The pH of the other half of the original solution is measured

  62. CHEMISTRY URGENT

    1. You have been given a sample of unknown molarity. Calculate the molarity of a solution which has been prepared by dissolving 8.75 moles of sodium chloride in enough water to produce a solution of 6.22l. 2. You have a sample which consists of 428g sodium

  63. general, organic and biochemistry

    when a solution prepared by dissolving 4.00g of an unknown monoprotic acid in 1.00L of water is titrated with 0.600M NaOH, 38.7mL of the NaOH solution is needed to neutralize the acid. What was the molarity of the acid solution? what is the molecular

  64. organic chemistry

    An unknown H2So4 sample of 25.00mL vl is titrated with 0.149 M NaOH. If 45.22mL of NaOH were needed to reach the pink endpoint, what was the molarity of the unknown acid? Show work using conversion factors????? H2SO+2NaOH --> Na2SO4+2H2O Dont know where or

  65. chemistry

    a 1.32g sample on unknown containing KHP as a component was titrated with 22.48mL of 0.105 M NaOH to a pheolphthalein end point. what is the weight percent of KHP in the unknown sample?

  66. Chemistry

    a 15.00mL sample of NaOH was titrated to the stoichiometric point with 17.40mL of 0.2340M HCl. a) what is the molar concentration of the NaOH solution? b)calculate the grams of NaOH in the solution.

  67. Chemistry

    A sample of 1.029g of KC8H5O4 was titrated with an NAOH solution of unknown concentration. If 22.83 mL of base was used to reach the endpoint, what was the concentration of NaOH? What mass of KC8H5O4 should be used such that a volume of NaOH between 35-40

  68. chemistry

    A volume of 12.47 mL of 0.1080 M NaOH solution was used to titrate a 0.583 g sample of unknown containing K2HPO4. What is the percent by mass of K2HPO4 in the unknown? In this problem what mass of sample in grams would be needed to deliver about 23.40 mL

  69. Chemistry

    10.00 mL of an unknown base solution is titrated with .100 M HCl solution. The pH versus the volume of NaOH added is shown below. There is a graoh where there are two dotted lines signifying a pH: the highest at pH 6.31 and the lower at pH 3.92. What is

  70. chemistry

    A 0.8743 g sample of KHP was titrated 42.45-mL of NaOH solution until the phenolphthalein endpoint. What is the molarity of the NaOH solution?

  71. chemistry

    A sample of potassium hydrogen oxalate, KHC2O4, weighing 0.717 g, was dissolved in water and titrated with 18.47 mL of an NaOH solution. Calculate the molarity of the NaOH solution.

  72. Chemistry

    The Question Is: "A student weighs 0.347 g of KHP on a laboratory balance. The KHP was titrated with NaOH and the concentration of the NaOH determined to be 0.110 M. For the second titration, the student correctly diluted 6 M HCl from the reagent shelf

  73. Chemistry

    Unknown Acid: #2 Mass of Unknown solid acid transferred:0.414g Volume of volumetric flask: 100.00 mL Concentration of NaOH: 0.0989 M Aliqot of acid titrated with NaOH: 25.00 mL Average volume of Naoh from titration: 13.9 mL Here's where I need help: No of

  74. chemistry

    2.) If you pass 10.0mL of a 50.0mL solution of [Co(en)2Cl2]Cl that has been reduced with Zn through a cation exchange column, you will obtain a solution that has three H+ ions for every Co3+ ion that was originally present in the sample. These H+ ions are

  75. chemistry

    35.0 mL of an aqueous solution of HNO3 of unknown concentration is titrated with a standard solution made up of 0.453 m NaOH

  76. Help!!!!!!!!!!!!

    A 0.391 g sample of KHP will be titrated with a NaOH solution with an assumed concentration of 0.100 M. Calculate the volume of NaOH that should neutralize the KHP sample.

  77. Chemistry

    A 20.0-mL sample of 0.300 M HBr is titrated with 0.150 M NaOH. What is the pH of the solution after 40.3 mL of NaOH have been added to the acid?

  78. chemistry

    A 20.0 mL sample of 0.687 M HBr is titrated with a 0.216 M NaOH solution. The pH after the addition of 10.0 mL of NaOH is __________.

  79. Chemistry

    A 25 mL sample of wine is found to have a concentration of acetic acid of 0.23 M. If this was titrated with a 0.16 M NaOH solution how many mL's of NaOH would be required?

  80. chemistry

    50.0 mL of an unknown HCl solution was titrated with 0.449 M NaOH. To reach the equivalence point, 38.4 mL of the NaOH was used. What was the concentration of the HCl?

  81. chemistry

    25.0g of 5.0% (by mass) acetic acid solution are titrated with 0.300 M NaOH. What volume of NaOH will be needed to neutralize this sample?

  82. chemistry

    i am calculating an unknown acid for both monoprotic and diprotic assumptions. I calculated the monoprotic by multiplying the M NaOH by the liters of NaOH used to titrate. 0.0984M x 0.02396= 0.00236. I then take the unknown sample weight and divide it by

  83. Chemistry

    The student used the KHP in a subsequent titration experiment where he titrated 25.00 +/- 0.03 ml of the acid against an unknown solution of NaOH. The titration required 23.70 +/- 0.10 ml of the base. What is the concentration of NaOH?

  84. Chemistry

    a 30 mL sample of vinegar is titrated with .1098 M NaOH. it takes 43.28 mL naOH solution to reach the endpoint. Determine the acetic acid concentration in the vinegar solution?

  85. chemistry

    A 15.0 ml sample of an unknown HClO4 solution requires 50.3 ml if 0.101 M NaOH for complete neutralization. What was the concentration of the unknown HClO4 solution? The neutralization reaction is: HClO4(aq)+ NaOh(aq)yields H2O(l)+ NaClO4 (aq) If anyone

  86. chemistry

    A 15.0 ml sample of an unknown HClO4 solution requires 50.3 ml if 0.101 M NaOH for complete neutralization. What was the concentration of the unknown HClO4 solution? The neutralization reaction is: HClO4(aq)+ NaOh(aq)yields H2O(l)+ NaClO4 (aq) If anyone

  87. chemistry

    A 20.0 mL sample of 0.687 M HBr is titrated with a 0.216 M NaOH solution. The pH after the addition of 10.0 mL of NaOH is __________. A. 0.413 B. 0.386 C. 0.163 D. 0.579 E. 0.237

  88. chem

    A 27.4 mL sample of an unknown HClO4 solution requires 45.4 mL of 0.101 M NaOH for complete neutralization. What was the concentration of the unknown HClO4 solution? The neutralization reaction is shown below. HClO4(aq) + NaOH(aq) H2O(l) + NaClO4(aq)

  89. Chemistry

    A buret is partially filled with NaOH solution, to a volume of 1.14 mL. A 20-mL sample of 0.1011 M HCl is titrated to a faint pink phenolphthalein endpoint. The final buret reading is 22.37 mL. What is the molartiy of the NaOH solution?

  90. Chemistry

    Instead of using ratios for back titrations we can also use molarities if our solutions are standardized. A 0.188g sample of antacid containing an unknown amount of triprotic base Al(OH)3 was reacted with 25.0mL of 0.101M HCl. The resulting solution was

  91. Chemistry

    Instead of using ratios for back titrations we can also use molarities if our solutions are standardized. A 0.188g sample of antacid containing an unknown amount of triprotic base Al(OH)3 was reacted with 25.0mL of 0.101M HCl. The resulting solution was

  92. Chemistry

    A 0.120 g sample of a diprotic acid of unknown molar mass is dissolved in water and titrated with 0.1218 M NaOH. The equivalence point is reached after adding 12.4 mL of base. What is the molar mass of the unknown substance?

  93. CHEMISTRY

    1) An NaOH solution of unknown concentration is titrated with HCl. 51.9 mL of 0.400 mol/L HCl will neutralize 75.0 mL of the NaOH. What is the concentration of the NaOH solution ? Record your answer in decimal notation. I think the answer is 0.277 mol/L.

  94. Chemistry

    A .682 g sample of an unknown weak monoprotic acid, HA, was dissolved in sufficient water to make 50mL of solution and was titrated with a .135 M NaOH solution. After the addition of 10.6mL of base, a pH of 5.65 was recorded. The equivalence point was

  95. Chemistry

    A 0.750 g sample of an unknown solid is dissolved in 100 mL of water and acidfied with 25 mL of 3 M H2SO4 then titrated with a 0.0200 M KMnO4 solution. If the unknown solid requires 12.5 mL of the KMnO4 solution to reach the endpoint, what is the % sodium

  96. chemistry

    The acidity of a water with initial pH of 5.5 was tested using the following procedure: The pH of a volume of 50.00 mL water sample was adjusted to 4.0 using 5 mL 0.1 N H2SO4 solution. Then this sample was titrated using 0.2 N NaOH. After addition of 7 mL

  97. Chemistry

    1)What is the pH of a 0.25 M solution of acetate (CH3COO-) with a pKa of 4.76? 2)If the [OH] of a solution is 2.95 x 10-5M, what is the pH of the solution? 3)Determine the pH at the equivalence point when 25.00 mL of 0.1056 M CH3COOH is titrated with

  98. Chemistry

    In this experiment NaOH is standardized to titrate it with vinegar so thtat the percent by mass of the acetic acid can be determined. How does dissolved CO2 in distilled water affect the accuracy of the determination of a NaOH solution's concentration? How

  99. chemistry

    A 27.00mL sample of an H2SO4 solution of unknown concentration is titrated with a 0.1422M KOH solution. A volume of 40.22mL of KOH was required to reach the equivalence point. What is the concentration of the unknown H2SO4 solution? Any help would be

  100. chemistry

    Vanadium is an environmental pollutant originating from some types of steel, but also from the combustion of fossil fuels. The amount of V2+ in an unknown sample is determined by potentiometric titration by 7.62 mM permanganate ion, MnO4 - . 25.00 mL of

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