1. chemistry

    Why is it recommended to carry out iodometric titration as quickly as positive and to get the first end point?
  2. chemistry

    consider a iodometric titration. why we add starch indicator just before the end point????. why cannot we add it before we start the titration???
  3. chemistry

    why is it recommended to carryout iodometric titrations as quickly as possible and to get the first endpoint
  4. Chemistry

    1.Describe the apparent relationship between H30+ and OH- concentrations when an endpoint is reached in an acid-base titration 2. The indicated end-point of an acid-base titration seldom occurs at a pH of 7. What determines the pH of the end point? 1. They
  5. Chemistry-iodometric titration

    In an iodometric titration, excess potassium iodide solution (KI) is added to the sample.Analyte such as chlorine liberates iodine from KI under acidic condition. Liberated iodine is titrated against standard sodium thiosulphate. The concentration of
  6. Chemistry

    A 10.0 mL sample of supernatant liquid from the system described by equation 1 was titrated with 0.01022 M EDTA solution to an end-point at 16.90 mL. Titration of the blank gave a titre (end-point) at 1.45 mL. Determine the titration volume required to
  7. chemistry.

    in the titration between Na2CO3 and HCl... 1) at the first end point what reaction is stoiciometrically complete? 2)At the start of titration where HCl=0 is the solution acidic or basic. ExPlain? 3) At the 2nd end point what reaction is stiociometrically
  8. chemistry

    Equations for iodometric titration of carbon monoxide
  9. CHM 300

    Experiment: Redox titration;determination of ascorbic acid by an iodometric back-titration Why is sodium carbonate added to the thiosulfate solution ? why is the water used for preparing the thiosulfate solution boiled ?
  10. chemistry

    in HNO3 titration, you add few drops of phenolphthalein indicator to 50.0 mL of acid in a flask. you quickly add 20.00 mL of 0.0547 M NaOH but overshoot the end point, and the solutions turn deep pink. instead of starting over, you add 30.00 mL of acid,
  11. science

    OBJECTIVE: to find out which of two indicators, methyl orange or phenolphthalein, gives more reliable and consistent results in the titration of H3PO4 with NaOH. REQUIREMENT: (1). Phosphoric acid solution of unknown concentration. (2). Standard NaOH
  12. science, chemistry

    OBJECTIVE: to find out which of two indicators, methyl orange or phenolphthalein, gives more reliable and consistent results in the titration of H3PO4 with NaOH. REQUIREMENT: (1). Phosphoric acid solution of unknown concentration. (2). Standard NaOH
  13. Chemisty

    In titrations of acids and bases, what is the difference between the end point of the titration, and the equivalance point? Also, what is chemically occuring during the buffer zone? Thanks! Good question and one that students sometimes have trouble with.
  14. CHM 300

    How do you find the Mass of Vitamin C in tablet? we did Redox Titration (Determination of ascorbic acid by Iodometric Back-Titration) I have fillied out the data table for Standardization of 0.07 M Na2S2)3 for the determination of unknown I cannot figure
  15. Chemistry 20 titration

    1) oi50 . tinypic . com / ejh6vm . jpg The most suitable indicator for the titration is: A)methyl violet B)chlorophenol red C)methyl orange D)phenolphthalein 2-A base is titrated with an acid solution until the indicator changes colour. This change in the
  16. chemistry

    difference stoichiometric end point and end point in an acid-base titration
  17. chem

    Consider the titration of 20 mL of .105M Butric Acid HBut, with .125M sodium Hydroxide? calculate the pH before titration calculate the volume of added base to reach the end point calculate the pH halfway to the equivalence point kb(But-)= 6.6x 10^-10 and
  18. chemistry

    Determine the Molarity of a 125 mL NaOH solution if upon titration with 5.5 mL of an 2.5 M HCl solution, the end point of the titration was reached
  19. Chemistry Lab

    Last week, I did titration of Zn with EDTA experiment. I used calmigte as the indictor. The endpoint of this titration is supposed to be blue. The color change go from wine-red to violet to Blue. I did a mistake by stopping the titration at the violet
  20. Chemistry Lab

    Last week, I did titration of Zn with EDTA experiment. I used calmigte as the indictor. The endpoint of this titration is supposed to be blue. The color change go from wine-red to violet to Blue. I did a mistake by stopping the titration at the violet
  21. Chemistry

    HC2H3O2 + NaOH --> NaC2H3O2 + H2O? a. when the titration is only half over, what species are present in the reaction flask b. what can be said about the pH at this point when the titration is half over? c. what is the pH at the equivalence point of this
  22. chem lab

    KMn04 with iron(II) ammonium sulphate hexahydrate-redox titration. 1-what is the purpose of adding H2SO4 to iron sample before the titration? 2-why is there no indicator used to determine the end point for this titration? 3-suggest another possible
  23. anaytical chemistry

    experiment: potentiomeric titration 1. Why is continuos stirring (use of stirrer and magnetic stir bar)important in potentiometric titration? 2. Why should the increments of addition of titrant be narrowed down as the titration approaches the equivalence
  24. CHEMISTRY

    What is difference between equivalence point and end point in the titration ?
  25. Chem

    In procedure B2, you will titrate a saturated solution to find out how much of the anion dissolved. Assume you we're able to dissolve about 0.12g of potassium hydrogen tartrate in 25.0 mL of water. For the titration, you will use 10.00mL of this sample.
  26. chem

    Right hand side of cell was titrated with Nh3 while monitoring cell voltage: Ag(s)IAg^+ (aq, 0.1 M, 25.0 mL)II Ag^= (aq, 0.1 M, 75.0 mL)I Ag(s) With 1.52 M ammonia titrant, the end point was observed at 9.8 mL. The measured cell voltage was near -0.15 V at
  27. titrations

    I have to find the correct acid-base indicator to use for the following titrations (methyl orange with end point @ pH 4, bromthymol blue with end point @ pH 7, or phenopthanlein with end point @ pH 9). I have several problems given to me, but first I'm
  28. Phenolphtalein vs Methyl Orange (check my reasonin

    Why can either phenolphthalein or methyl orange be used for an HCl-NaOH titration, but only phnolphthalein is suitable for an acetic acid-NaOH titration? Sol: for a while,I misunderstood the question and suggested that Phenol. has a wider array of pH. But
  29. chemistry

    why are the equivalence point and the end point different in a titration?
  30. Chemistry

    When looking at a titration curve, I have to determine which is not true and I have it narrowed down to two options: The initial starting point on the titration curve is where pH depends only on [HA]0 or The finial point on a titration curve the pH depends
  31. Chemistry

    Plot the titration of a weak base with a strong acid. Show the titration curve using .106M NH3 and .225M HCl for a 50.00mL sample of the ammonia. No idea where to start here. I'm supposed to plot the curve from 2mL increments (0-30). Tip on homework:
  32. Chemistry PLEASE HELP!

    Check all of the following statements which are TRUE for a titration. Select one or more: a. A suitable primary standard must be available. b. The concentration of the solution in the buret (the titrant) must be known before the titration is begun. c.
  33. chemistry

    11.During an acid-base titration, 25 mL of NaOH 0.2 M were required to neutralize 20 mL of HCl. Calculate the pH of the solution for each of the following: 12.Before the titration. 13.After adding 24.9 mL of NaOH. 14.At the equivalence point. 15.After
  34. chem lab (webwork)

    When a good indicator has been chosen, the pH at which the solution changes color is very close to the point of the titration. Complete the table below: If this "point" for a particular titration occurs at pH x, a good indicator for for the titration would
  35. CHEMISTRY TITRATION Q

    The titration of 25.00mL of Ba(OH)2 solution with an aqueous solution of 0.500 M HCl reaches an end point when 30.20 mL of the HCl solution is added. Determine the concentration of M of the Ba(OH)2 solution. Soo 25.00mL=0.025L 30.20mL= 0.0302L moles= MxL
  36. Chemistry

    Hi everyone, I have been trying to figure out this titration equation all day and for some reason I am stumped. Here is the question in full: Potassium hydrogen phthalate, KHP, can be obtained in high purity and is used to determine the concentrations of
  37. Chemistry

    When looking at a titration curve, I have to determine which is false and I have it narrowed down to two options: The initial starting point on the titration curve is where pH depends only on [HA]0 or The finial point on a titration curve the pH depends
  38. Chemistry

    Consider the titration of 20.00 mL of 0.1728 M Ascorbic acid (Ka = 7.9 x 10-5) with 0.4329 M NaOH. Match the following regions in the titration curve with the appropriate pH range. 1.Initial pH 2.Before equivalence point 3.At equivalence point 4.After
  39. Chemistry

    Say true or false. (1)The end point of titration attend on equivalent point. (2)All exothermic process are spontaneous process.
  40. AP Chemistry

    In a titration of 50 mL 1 Molar HC2H3O2 with 1 Molar NaOH, a student used bromcresol green as an indicator (Ka = 1 X 10^-5). About how many mL of NaOH would it take to reach the end point with this indicator? What would be a better indicator for this
  41. Chemistry

    Consider the titration of 20.0mL of 0.300M acetic acid, HAc, with 0.150M NaOH solution. Ka=1.75*10^-5 HAc + NaOH ---> NaAc + H2O What is the composition of the solution at the equivalence point of the titration? Give both the formula of the compound and
  42. chemistry

    Thymol blue in its acid range is not a suitable indicator for the titration of HCl by NaOH(aq) . Suppose that a student uses thymol blue by mistake in the titration of Figure 17-9 in the textbook and that the indicator end point is taken to be pH=2.0.
  43. Chemistry

    q1. The label on an antacid remedy states that each tablet contains 750 mg of aluminum hydroxide. Calculate the volume of stomach acid, 0.10 mol/L HCl(aq), which can be nuetralized by one antacid tablet. Q2. Compare equivalence point to endpoint q1. The
  44. Chemistry

    Consider the titration of 25.0mL of 0.10M HAc with 0.10M NaOH. That is, NaOH is added to HAc. (a)pH at the beginning of titration. (b)pH at the equivalence point of the titration. (c) pH at the midpoint of the titration.
  45. Science - Electrochemistry

    In an experiment 0.0500 M AgNO3 was used to titrate 20 mL of 0.12 M NaCl solution. When silver electrode is used together with the pH electrode to measure potential at each point during the titration, the potential measured at equivalence point is 0.055 V.
  46. Chemistry

    When a good indicator has been chosen, the pH at which the solution changes color is very close to the equivalience point of the titration. If this "point" for a particular titration occurs at pH x, a good indicator for the titration would be indicator. X
  47. chemistry

    100 ml of a raw water sample on titration with 1/50N h2so4 required 12ml of the acid to phenolpthalein end-point and 15.5 ml of the acid to methyl orange end point. determine the type and extent of alkalinity present in the water sample. please explain me
  48. Chemistry

    A weak acid with an initial pH of 3.2 was titrated with a strong base. 15 mL of 0.1 M NaOH was added to the acid to reach the equivalence point at a pH of 8.6. What would you expect the approximate pH of the analyte to be after the first 5 mL of 0.1 M NaOH
  49. Science (chemistry)

    Pls help.. Q: prepare a table of value for acid-base titration using 26.40cm^3 as end point
  50. Chemistry- titration

    OK I REALLY NEED HELP!!! and i AM DESEPRATE!! I have a titration courswork tomorow and i need to know the measurment,procedual and significant errors that are made in titration and how they can be improved. Also i need help with the evaluation bit. I
  51. chemistry

    There is a titration of 5.00 mL .010 M NaOH with .005 M HCl. Indicate the pH of the initial and final solutions and the pH at the stoichiometric point. What volume of HCl has been added at the stoichiometric point and the halfway point of the titration? I
  52. Chemistry

    The half-equivalence point of a titration occurs half way to the end point, where half of the analyte has reacted to form its conjugate, and the other half still remains unreacted. If 0.220 moles of a monoprotic weak acid (Ka = 5.7 × 10-5) is titrated
  53. chemistry

    The half-equivalence point of a titration occurs half way to the end point, where half of the analyte has reacted to form its conjugate, and the other half still remains unreacted. If 0.220 moles of a monoprotic weak acid (Ka = 3.7 × 10-5) is titrated
  54. chemistry

    The half-equivalence point of a titration occurs half way to the end point, where half of the analyte has reacted to form its conjugate, and the other half still remains unreacted. If 0.460 moles of a monoprotic weak acid (Ka = 3.8 × 10-5) is titrated
  55. Chemistry

    q1. The label on an antacid remedy states that each tablet contains 750 mg of aluminum hydroxide. Calculate the volume of stomach acid, 0.10 mol/L HCl(aq), which can be nuetralized by one antacid tablet. Q2. Compare equivalence point to endpoint q1. The
  56. chemisty

    Consider the titration of 50 mL of 0.15 M NH3 with 0.1 M HCl. What is the pH at the equivalence point of the titration? (Kb= 1.8X 10-5 Ka= 5.6X10-10)
  57. chemistry

    Consider the titration of 40.0 mL 0.250 M ethylamine, C2H5NH2, with 0.350 M HCl. Determine each of the following and sketch the titration curve. Kb of ethylamine = 5.6x 10-4 a. The volume of added acid required to reach the equivalence point. b. The
  58. science-chem- theory questions

    please, help me.. i think i know the answers, but i just want to make sure! i'd love your feed back :) 1) an air bubble is trapped in the tip of a buret before a titration. during the titration, the bubble is passed from the buret tip. will the reported
  59. chemistry

    On the axis below, draw the titration curve for the titration of CH3COOH (a weak acid) with NaOH (a strong base). In the titration, the equivalence point occurs when 40 mL of NaOH has been added. Make sure to label your x- and y-axis and put numbers on
  60. chemistry

    In the following questions, assume that no excess distilled water was added from a wash bottle during the titration of 10.00 mL of vinegar with your standardized solution of NaOH. A. calculate the pH of vinegar. B. what was the pH of the solution after
  61. chemistry help

    In the following questions, assume that no excess distilled water was added from a wash bottle during the titration of 10.00 mL of vinegar with your standardized solution of NaOH. A. calculate the pH of vinegar. B. what was the pH of the solution after
  62. Chemistry

    Would your calculated Ksp value be greater, less, or the same, if the following occurred, please explain your reasoning. a. The CaSO4 was not saturated b. You accurately measured 20.00 mL instead of 25.00 mL using a pipet c. The CaSO4 solution contained
  63. Physics

    a 2x10^-6 point charge travels a distance of.002m between two parallel charged plates from the negative end toward the positive end. The field has a strength of 500 N/C What is the change in voltage?
  64. chemistry

    What volume in ml of 0.0985 m NaOH solution is required to reach the end point in the complete titration of a 15.0 ml sample of 0.124 M phosphoric acid?
  65. chem- acids and bases

    sorry to take up your time again, acids and bases just really confuse me, i'd really appreciate your help again. "What is the pH at the end point for the titration of 0.20M HNO2 by 0.20M NaOH? Ka nitrous acid= 4.5 x 10^-4." this is what i do know: - end
  66. Chemistry

    I've been stuck on this question for awhile now. I'm having a lot of trouble figuring out how to start it. If you had added exactly 20.00 mL do d.i. water before the titration, calculate the molar concentration of OAc- would have been at the end of the
  67. Chemistry

    How many grams of KHP (204.22 g/mol) were present in container if 49.36 mL of 0.2264M NaOH were needed to reach the end point of a titration? I'm confused on the formula you would use for this.
  68. Chemistry

    In a titration of 35 mL of 0.40 M H3PO4 with 0.30 M KOH solution, what volume (in mL) of KOH solution is needed to reach the last equivalence point (i.e., point in the titration where enough KOH has been added to neutralize all three of the acidic protons
  69. Chemistry

    In a titration of 35 mL of 0.40 M H3PO4 with 0.30 M KOH solution, what volume (in mL) of KOH solution is needed to reach the last equivalence point (i.e., point in the titration where enough KOH has been added to neutralize all three of the acidic protons
  70. 1CHEM

    In a titration of 35 mL of 0.40 M H3PO4 with 0.30 M KOH solution, what volume (in mL) of KOH solution is needed to reach the last equivalence point (i.e., point in the titration where enough KOH has been added to neutralize all three of the acidic protons
  71. Maths

    A circle C has center at the origin and radius 9. Another circle K has a diameter with one end at the origin and the other end at the point (0,17). The circles C and K intersect in two points. Let P be the point of intersection of C and K which lies in the
  72. Calculus

    A circle C has center at the origin and radius 9. Another circle K has a diameter with one end at the origin and the other end at the point (0,17). The circles C and K intersect in two points. Let P be the point of intersection of C and K which lies in the
  73. Math

    A circle C has center at the origin and radius 9. Another circle K has a diameter with one end at the origin and the other end at the point (0,17). The circles C and K intersect in two points. Let P be the point of intersection of C and K which lies in the
  74. Calculus

    A circle C has center at the origin and radius 9. Another circle K has a diameter with one end at the origin and the other end at the point (0,17). The circles C and K intersect in two points. Let P be the point of intersection of C and K which lies in the
  75. chem12

    Hey guys i only have this question left on my review and i just can't fingure it out! Sketch a pH curve for the titration of 40.00mL of 0.100 M hydrazine, H2NNH2, having a K of 3.0x10^-6 by 0.100 M HCIO4 a) what combination of acide-base titration is this?
  76. Chemistry 12

    Hey guys i only have this question left on my review and i just can't fingure it out! Sketch a pH curve for the titration of 40.00mL of 0.100 M hydrazine, H2NNH2, having a K of 3.0x10^-6 by 0.100 M HCIO4 a) what combination of acide-base titration is this?
  77. Analytical Chemistry

    Predict the effect (Increase, Decrease, No effect, Indeterminate)and explain why 1. Condition: In the determination of water hardness, the water sample contained appreciable amount of ferric ions Paameter: ppm CaCO3 2. Condition: Instead of MgCl2*H2O,
  78. Chemistry

    The electrophoresis of a mixture of histidine (His), aspartic acid (Asp) and phenylalanine (Phe) is carried out a pH of 5.91. What amino acid will This bear no net charge at pH 5.91 and so will remain at the origin, carry a net negative charge at pH 5.91
  79. Chemistry

    In my titration method it says trial titration. In my table it says rough titration. I know the meaning of both. But, are they the same thing and could i say my first titration rough value is both the trial titration and rough titration?
  80. chemistry

    In an acid-base titration, 33.12ml of 0.1177 M H2C2O4 was titrated with 0.2146 M NaOH to the end point. What volume of the NaOH solution was used?
  81. Chemistry

    A drop of liquid is about 0.05 mL. When doing a titration lab, 73 drops of base were used to reach end point; how many liters of base were required to neutralize the acid?
  82. Chemistry

    A laboratory technician wants to determine the aspirin content of a headache pill by acid–base titration. Aspirin has a Ka of 3.0 × 10-4. The pill is dissolved in water to give a solution that is about 10-2 M and is then titrated with KOH solution. Find
  83. chemistry

    CH3NH2(aq)+H2O(l)=>CH3NH3+(aq)+OH-(aq) Kb=4.4 x 10^-4 Methylamine, CH3NH2, is a weak base that reacts with water according to the equation above. A student obtains a 50.0 mL sample of a methylamine solution and determines the pH of the solution to be
  84. AP Chemistry

    CH3NH2(aq)+H2O(l)=>CH3NH3+(aq)+OH-(aq) Kb=4.4 x 10^-4 Methylamine, CH3NH2, is a weak base that reacts with water according to the equation above. A student obtains a 50.0 mL sample of a methylamine solution and determines the pH of the solution to be
  85. Chemistry

    Describe the procedure you would follow to determine the concentration of vitamin c in a sample if the volume of dcpip required to reach the end point were more than the 10-mL graduated cylinder could hold. The titration must still be carried out in the
  86. 11th grade CHEMISTRY TITRATION LAB!

    i have a tritation lab due tomorrow and i am stumped on a couple things. its a titration lab using sodium hydroxide (NaOH)- 250 mL 0.300 M concentration, 10 mL of an unknown substance of vinegar, the avg. of titrated NaOH in the flask with vinegar is 27.7
  87. AP Chem

    1.513g of monoprotic acid (HX) is dissolved in water, and the volume is 250.0 ml after the dissolving. The solution was then titrated 38.12g of .100 M NaOH to reach the end point of the titration. What is the molecular weight of HX?
  88. Jill

    State the relationship of A to B (i.e. <, >, = or can't be determined). 1. Using a 0.05 M Ag+ titrant A.VEP in titration 25-mL of 0.01 M MgCl2 B.VEP in titrating 25-mL of 0.01 M AlCl3 2. A 25.0-mL solution contains 0.015 M NaCl and 0.010 M HCl A.VEP
  89. Physics Classical Mechanics

    A body of mass m= 1 kg is moving along the x-axis. Its potential energy is given by the function U(x)=2(x2−1)2 Note: The units were dropped for the numbers in the equation above. You should note that 2 would carry units of J⋅m−4 and 1
  90. chemistry

    1a) why is it advisable to prepare a slightly more conc. soln. of kMnO4 when preparing its standard solution? b) what else do u have to do? (2). what will happen if NH4Cl is used to standardized the KMnO4. (3a). A student noticed traces of brown deposit
  91. science

    I am doing a titration lab and need help with a problem. (i used .100M H2SO4)(I used 10.0 ml of Ba(OH)2 solution and added 50.0 ml of distilled water making 60.0 ml total.) 1. Use the titration results to calculate the moles of H2SO4 that were used to
  92. chem 3

    80 ml of 1.0M ch3 cooh(aq), are titrated with 2.0M KOH(aq) in the rreaction Ch3cooh(s)+ KOH(aq)reacts with kch3coo(aq)+ H2O what is the volume of potassium hydroxide was used to reach the end point of titration
  93. chemistry

    If the end point in the titration of oxalic acid with NaOH solution is super-passed (too pink), will the molar concentration of NaOH be hiegher or lower than the actual value ? Explain ..
  94. chemistry

    Consider the titration of 100.0 mL of 0.500 M NH3 (Kb = 1.8 x 10-5) with 0.500 M HCl. At the stoichiometric point of this titration, the [H+] is:
  95. 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
  96. Chemistry

    Prepare a theoretical titration curve for titration of 25.0 mL of 0.1037 formic acid (HCOOH; pKa = 3.75) solution (diluted to 100 mL volume with deionized water) by 0.0964 M solution of KOH. I have to determine volume of KOH needed to reach equivalence
  97. English

    Which of the following is a strong introductory sentence? A. Should each of the United States allow citizens to openly carry a weapon? B. I don’t agree with any open-carry laws. C. This essay will explain the open-carry laws in the United States. D. To
  98. English

    Which of the following is a strong introductory sentence? A. Should each of the United States allow citizens to openly carry a weapon? B. I don’t agree with any open-carry laws. C. This essay will explain the open-carry laws in the United States. D. To
  99. English

    Which of the following is a strong introductory sentence? A. Should each of the United States allow citizens to openly carry a weapon? B. I don’t agree with any open-carry laws. C. This essay will explain the open-carry laws in the United States. D. To
  100. chemistry

    Calculate the concentration of the chromate ion that should be present at the final point of the titration of 50, 00mL of a solution of KBr 0, 02mol/L with a solution of AgNO3 0, 01mol/L, if the maximum theoretical error for titration is 1.0%.