Which of the following statements is true concerning the titration of a weak base by a solution of hydrochloric acid? Question 9 options: At the equivalence point, the pH is 7. At the equivalence point, there is excess hydrochloric acid.

27,091 results
  1. 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

  2. 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

  3. Chemistry

    The graph shows the titration curve for 25.0mL of an aqueous solution of B titrated with 0.100MHCl. Which of the following best estimates the initial concentration of the solution of the weak base? (Initial pH of 12 and equivalence point at 50mL with pH of

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  5. Chemistry

    What is true about H+ and OH- when the endpoint is reached in an acid-base titration?

  6. AP Chemistry

    Rank these compounds in order of increasing hyroxide ion concentration: weak base, weak acid, strong base, strong acid.

  7. Chemistry

    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: a) Before titration b) After adding 24.9 mL of NaOH c) At equivalence pt d) After adding 25. 1 mL of NaOH e) The pH of

  8. Chemistry

    Which of the following statements are true about a strong base and a weak base at a pH of 11? A) HCl will not bring the pH of either solution to pH 7. B) Both bases require the same amount of HCl to reach pH 7 because they are both at the same initial pH.

  9. Chemistry

    A base has a Kb of 2.5 x 10–11. Which of the following statements is true? This is a concentrated base. This base ionizes slightly in aqueous solution. This is a strong base. An aqueous solution of this base would be acidic.

  10. chemistry

    A weak base with a concentration of 1.3 mol/L has a percent ionization of 0.72%. What is the Kb of this weak base?

  11. Chemistry

    A weak acid with a Ka of 1.8 × 10–5 is titrated with a strong base. During the titration,12.5 mL of 0.10 M NaOH is added to 50.0 mL of 0.100 M acetic acid. What is the pH after the addition of the NaOH? A. 7.22 B. 5.13 C. 4.26 D. 8.59 I know without any

  12. 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

  13. AP Chemsitry

    A solution of an unknown monoprotic weak acid was titrated with 0.100 M NaOH. The equivalence point was reached when 37.48 ML of base had been added. From a second buret, exactly 18.74 of 0.100 M HCl were added to the titration solution. The pH was then

  14. chemistry

    Which of the following statements is true concerning the titration of a weak base by a solution of hydrochloric acid? Question 9 options: At the equivalence point, the pH is 7. At the equivalence point, there is excess hydrochloric acid. At the equivalence

  15. Chemistry

    Calculate the pH for each of the following cases in the titration of 50.0 mL of 0.140 M HClO(aq) with 0.140 M KOH(aq).HClO is a weak acid with a Ka of 4.0× 10–8. It reacts with strong base to produce ClO–. (e) after addition of 60.0 mL of KOH

  16. Chemistry

    Write the balanced NET IONIC equation for the reaction that occurs when ammonium chloride and calcium hydroxide are combined. This reaction is classified as A. Strong Acid + Strong Base B. Weak Acid + Strong Base C. Strong Acid + Weak Base D. Weak Acid +

  17. Chemistry

    Given that 20 ml of a weak acid (HA) was titrated with NaOH and the titration curve of pH vs titrant volume in ml is given, find the initial concentration of the acid? The problem gives the full titration curve starting at pH=2.2 at 0 ml added and with the

  18. Chemistry: Equilbrium

    2. Which of the following statements are true about a strong base and a weak base at a pH of 11? HCl will not bring the pH of either solution to pH 7. Both bases require the same amount of HCl to reach pH 7 because they are both at the same initial pH. The

  19. Chemistry

    In the titration of a weak acid with a strong base, the pH at the equivalence point is affected mostly by a.hydrolysis (reaction with water) of the weak acid b.the dissociation of water molecules c.the presence of excess base d.the hydrolysis of the

  20. Chemistry

    I was just wondering how I would determine the pKb of a weak base that was titrated with a strong acid on a titration curve at the EQUIVALENCE POINT. And from this, how would I find the pH? PLEASE HELP!!

  21. chemistry; acids and bases

    Since Ka x Kb = Kw, is the conjugate base of a weak acid a weak base or a strong base?

  22. chemistry

    I am giving a titration curve of a weak base and strong acid. The pH on the y scale is from 0-14 and the volume of titrant in mL is from 0-34. It looks like the equivalene point is around 22? The question is: "The above titration curve was obtained when a

  23. Chemistry

    why is a weak acid weak base titration different from strong acid strong base/ weak acid strong base/strong acid weak base?

  24. AP Chemistry

    A solution is prepared by titrating a 100.0 mL sample of 0.10 M HF (Ka = 7.2 × 10-4) with 0.10 M NaOH a. Does the solution contain a strong acid with a strong base, a strong acid with a weak base, a weak acid with a strong base, or a weak acid with a weak

  25. Science

    C6H5NH2 + H2O C6H5NH3+ + OH- 1. Aniline, a weak base, reacts with water according to the rxn above. a. A sample of aniline is dissolved in water to produce 25.0 ml of a .10 M soln. The pH of soln is 8.82. What is Kb for this rxn? b. The soln in part b,

  26. english

    Which one of the following statements is true for the base forms of verb? A. when the subject of a sentence is singular, add "-s" to the base form. B. Add "to" to the base form to create an adjective. C.Do not use a base form with plural subjects. D.Add

  27. chemistry- check!

    1. A pure salt solution can be any of the following except a. basic b. buffered *** c. alkaline c. acidic 2. You can make a buffer with all the following except a. weak acid + conjugate base b. weak base + salt of weak base c. strong acid + salt of strong

  28. AP Chemistry

    Hi! For a strong acid-weak base titration what's an example of a titrant, analyte, appropriate indicator, pH at neutralization, and a typical graph of the titration? Help is much appreciated Thank you so much

  29. chemistry

    If the acid base reaction HA(aq)+B^-(aq)---> HB(aq)+A^-(aq)

  30. Organic Chemistry

    Please help! Thank you! Alcohols can act either as weak acids or as weak bases, just as water can. Show the reaction of methyl alcohol, CH3OH, with a strong base such as Na+ -NH2

  31. Chemistry

    A base has a Kb of 2.5 x 10–11. Which of the following statements is true? A.This is a concentrated base. B.This base ionizes slightly in aqueous solution. C.This is a strong base. D.An aqueous solution of this base would be acidic. My answer is D...?

  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

    if 0.4M NaOH is titrated with 0.4M HF, how do we calcualte the ph at equivalence. The book assumes each is 1L, but why do we use 1L * chemistry - Dr.Jim, Thursday, November 11, 2010 at 5:31am HF is a weak acid, so you need the dissociation constant. The pH

  34. chemistry (buffers)

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  35. math

    △GHJ∼△MNP Which statements are true? Select each correct answer. m∠J=m∠P (TRUE) ∠H≅∠N (TRUE) HJ¯≅NP¯ (it has the line over them) false GH=MN (TRUE) GJ/MP=GH/MN ( TRUE )

  36. 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:

  37. Chemistry 12

    name a compound that acts as a weak base? methanol? define the term weak bronsted-lowry base im not sure how to put this in words, but a weak base is found when you got a strong acid, when your ka is high, kb will be low.

  38. chemistry-please someone answer...i am clueless

    When a monoprotic weak acid is titrated with a strong base, the titration curve contains these many inflection points: a.zero b.one c.two d.three Can you also explain why you choose your answer to this question...thanks

  39. chemistry

    Select only the True statements about buffer systems. Select all that are True. 1. Starting with NH3(aq) and adding a small amount of HCl(aq) will make a buffered solution. 2. The blood buffer, among other things, is supported by carbonic acid and its

  40. Chemistry

    You have two buffer solutions 1) weak acid and its conjugate base 2)weak base and its conjugate acid. Write explicitly ( considering generic formula for acid and base) the equations of neutralization when you: a) add strong acid and strong base 1) b) add

  41. Chem+ASAP+2 fill in the blank questions+ASAP!!!

    PLease check this. They are fill in the blank and I just need to know if they are right. Thanks! 9. Compared to a strong acid-strong base titration curve, a weak acid-strong base titration curve has a (higher, lower) __higher___ initial pH value. 10.

  42. chemistry

    A weak base with a concentration of 1.3 mol/L has a percent ionization of 0.72%. What is the Kb of this weak base? could someone help me with this question or how to get started?

  43. chemistry

    For 0.250 M of weak acid (NaHS) the Kb is given by 1.22 x10-13 , calculate the pH of the weak base.

  44. chemistry

    When titrating a strong acid with a strong base, which is true? 1. the titration curve slopes upward 2. an indicator that changes at pH 8 would be acceptable 3. the pH changes slowly at the equivalence point

  45. Chemistry

    Why is the equivalence point of a weak acid-strong base titration above 7.0? How can the data reflect this? The titration of a weak acid with a srong base produces a salt of the two. The anion is hydrolyzed in water solution but the cation is not. A^- +

  46. 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

  47. Chemistry

    A solution of a weak acid will consist of the acid and its conjugate base. True or False false Yes, of course: Take acetic acid acetic acid + H2OH3O+ + acetateion- The system is in equilibrium. true

  48. Chemistry (Titration Curves)

    Which of the following Acid+Base titration combinations would have a buffering region in their plot? 1)Strong Acid+Strong base (HCl+NaOH) 2)Weak acid and strong base (Acetic+NaOH) 3)Strong Acid and weak base (HCl+NH3) 4)Weak Acid and weak base (Acetic+NH3)

  49. titrations

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  50. chemistry

    A 1.0 M acetic acid solution (CH3COOH, pKa = 4.7) is neutralized by dissolving NaOH(s) (a strong base) in the solution. Estimate the pH at the equivalence point of the neutralization process: 4.7 7.0 9.3 Which one of the following statements best explains

  51. Chemistry

    How would I get the Ice of the titration of 40.00ml of 0.100M H2NNH2(aq) having a Kb of 3.0x10^-6 by 0.100M HClO4(aq)? Trying to plot a pH curve. I know the combination of acid base is strong acid weak base

  52. Chemistry (A level)

    I was given a Chemistry question on the titration of a strong base being added to a weak acid. The question was: "Calculate the pH in a titration when 10.0cm^3 of a 0.10moldm^-3 solution of NaOH is added to a 10.0cm^3 of 0.25moldm^-3 solution of ethanioc

  53. Chemistry

    I have an assignment Q A 0.1 mol L-1 water solution of NH4CH3CO2 has a pH of approx 7. Explain this using two equations. I have one equation CH3COO-(aq) + H2O(l) --> CH3COOH(aq) + OH-(aq) What could the other equation be? NH4CH3CO2 is the salt of a weak

  54. 1 chem question

    A base has a Kb of 2.5 x 10–11. Which of the following statements is true? This is a concentrated base. This base ionizes slightly in aqueous solution. This is a strong base. An aqueous solution of this base would be acidic. (do explain. i don't

  55. analytical chemistry

    When a monoprotic weak acid is titrated with a strong base, the titration curve contains these many inflection points: a.zero b.one c.two d.three Can you also explain why you choose your answer to this question...thanks

  56. chem

    Is lithium hydroxide a strong or weak base? It is 100% ionized so, by definition, it is a strong base. Try looking up Kb for LiOH in a set of tables. It won't be there, further proof that it is not a weak base. thank you!

  57. chemistry

    1. An aqueous solution of weak base B of unknown concentration is tritrated with a known concentration of strong acid, HA. (a) Write the balanced chemical equation for this acid-base reaction, identifying the conjugate acid/base pairs. (b) If the

  58. Organic chemistry: dehydrohalogenation

    Hello. I know you guys don't do organic chemistry but because I got so much help from you guys in general chemistry, I was wondering if you guys can help me out again. :P Here's my question. In dehydrohalogenation, how do you know whether a reaction is E1

  59. Organic Chem

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  60. Chemistry

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  61. SCIENCE PLZZ HELP!!!

    Given equal concentrations, which of the following produces the fewest hydronium ions in an aqueous solution? strong acid weak acid strong base weak base This is the only question i need help on and i have no clue what ut is! any help?

  62. Chemistry

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  63. Math

    1.Suppose we are given logic statements p, q, and r. a. If p → q and p → r, may we conclude that q → r? Answer yes or no and give a reason why. b. What is the converse of the following: not p → not q c. What is the contrapositive of r → q? d. The

  64. Chem

    What simplifying assumptions do we usually make in working problems involving equilibria of salts of polyprotic acids? Why are they usually valid? Answer by selecting all true statements. Are the answers: a,b,d,and f A)If the two ionization constants are

  65. 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

  66. Chemistry

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  67. Math

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  68. chemistry

    Can you tell if I'm correct. Which combination in titration has ph=pka and buffer region strong acid-strong base- no to both strong acid-weak base- yes to both weak acid-strong base- yes to both weak acid-weak base- I'm not sure about this one. Can anyone

  69. chemistry

    Can you tell if I'm correct. Which combination in titration has ph=pka and buffer region strong acid-strong base- no to both strong acid-weak base- yes to both weak acid-strong base- yes to both weak acid-weak base- I'm not sure about this one. Can anyone

  70. Chemistry

    How do you find the initial concentration of the acid give the titration curve of a weak acid-strong base titration?

  71. Chemistry

    A weak acid with a Ka of 1.8E-5 is titrated with a strong base. During the titration, 12.5 mL of 0.10 M N(base a)OH is added to 50.0 mL of 0.100 M acetic acid. What is the pH after the addition of the N(base a)OH? A. 4.26 B. 5.13 C. 7.22 D. 8.59 I have no

  72. CHEMISTRY

    How can we determine the equivalence point ( or end point ) in the curves in titration ( strong acid/weak base and weak acid/strong base )

  73. Chemistry

    If an equal number of moles of the weak acid HOCN and the strong base KOH are added to water, the resulting solution will be acidic, basic or neutral? There is a complicated answer and a sensible answer. Both arrive at the same answer. But here is the

  74. AP Chemistry

    A solution is prepared by titrating a 100.0 mL sample of 0.10 M HF (Ka = 7.2 × 10-4) with 0.10 M NaOH a. Does the solution contain a strong acid with a strong base, a strong acid with a weak base, a weak acid with a strong base, or a weak acid with a weak

  75. Chemistry

    What is the pH of the solution created by combining 2.00 mL of the 0.10 M base[ammonia] with 8.00 mL of the 0.10 M acid[acid acid]? I tried this problem so many times, but always got it wrong. It's a weak base and acid titration. but i don't know the

  76. 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

  77. chemistry

    A weak base that encompasses a concentration of 1.4 mol per litre has a percent ionization of 0.63%. Calculate the Kb of this weak base

  78. Chemistry

    A buffer contains the weak acid HA abd its conjugated base A-. The weak acid has a Ka of 1.51 x10^-5 and the buffer has a pH of 4.25. Which statement is true about the relative concentrations of HA and A- in the buffer? A) [HA]>[A-] B) [HA]

  79. chemistry

    do we have buffering region and ph=pka in any of these conditions: strong base vs strong acid strong base vs weak acid weak base vs strong acid weak base vs weak acid

  80. Chem

    The following questions refer to the following system: A total of 30.0 mL of a .10M solution of a monophonic acid (Ka = 1.0 x 10 ^-5) is titrated with .20M sodium hydroxide solution. 1) Before the titration begins, the pH of the solution is about A) 2 B) 5

  81. Chemistry

    I have a question regarding the titration curve. When the ph is equal pKa that mean there are equal amount of conjugate acid to conjugate base. When a weak acid dissociates for example H3Po4 H+ H2PO4- My problem: I don’t understand how the ph rises

  82. Chemistry

    A buffer is prepared by mixing 110. mL of 0.442 M HCl and 0.545 L of 0.400 M sodium acetate. How many grams of KOH must be added to 0.500 L of the buffer to change the pH by 0.10 units? The pH I have calculated to be 5.28. What do I to figure this out? I

  83. analytical chemistry

    A solution containing 0.40 M B (a weak base) and 0.20 M BH+ (the salt of the weak base) has a pH = 10.30. What is the pH after 25 mmol of HCl is added to 250 mL of this solution?

  84. Chemistry

    TRUE OR FALSE? 1) A solution that is made out of 1.00mol/L ammonia and 0.50mol/L of ammonium chloride is a basic buffer. 2) The pH at the equivalence point of a weak base with a strong acid is expected to be less than 7 because the acid that is added is

  85. Chemistry

    I don't know how to reply to an answer. First of all thank you! For the question I just asked about the titration curves. Would that mean that titrating with barium hydroxide would take half the volume that is used when titrating with sodium hydroxide? Oh

  86. Chemistry

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  87. Chemistry

    If 32.6 mL of 0.240 M oxalic acid are required to titrate 48.9 mL of unknown sodium hydroxide: How many moles of acid are used in the titration? How many moles of base are used in the titration? What is the molarity of the unknown NaOh base? Please help I

  88. Chemistry

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  89. Chemistry

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  90. Chemistry

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  91. Chemistry

    I don't understand how to work out the volumes of weak acid and strong base to mix to make 1L of buffer when given the concentrations of weak acid and strong base (in my case 0.160M NaOH and 0.200M H3PO4) and the pH required (7.00). Specifically the

  92. Integrated Science

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  93. Chemistry

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  94. 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

  95. Chem

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  96. chemistry

    I need help setting up a problem to calculate pH during the titration of 20.00ml Of 0.1000M (CH3CH2)3N (Kb= 5.2 x 10-4) with 10.00ml of .1000M HCL. I can do it with a weak acid - strong base but this is a weak base - strong acid and I don't know if its the

  97. chemistry

    When a monoprotic weak acid is titrated with a strong base, the titration curve contains these many inflection points: a.zero b.one c.two d.three Can you also explain why you choose your answer to this question...thanks

  98. 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

  99. Chemistry

    When 23.5 mL of 0.12 M HCl are added to 50.0 mL of a 0.15 M solution of a weak monoprotic base, the pH of the solution is 10.00. What is the Kb of the weak base?

  100. Chemistry

    When 23.3 mL of 0.14 M HCl are added to 50.0 mL of a 0.16 M solution of a weak monoprotic base, the pH of the solution is 10.50. What is the Kb of the weak base? do u find moles of both and then add the moles for HB+ and then just use the B- moles for the

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