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A 0.040M solution of a monoprotic acid is 14% ionized. Calculate the Ka for the weak acid. ---------------- so: HX H+ + X- Ka= [H+][X-]/ [HX] Since its a monoprotic acis i know the concentration of H and X will

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  1. Chemistry

    A 0.040M solution of a monoprotic acid is 14% ionized. Calculate the Ka for the weak acid. ---------------- so: HX H+ + X- Ka= [H+][X-]/ [HX] Since its a monoprotic acis i know the concentration of H and X will be equal And the HX will be 86% (100%-14%)
  2. chemistry

    A. Strong Base 1.) What is the concentration of a solution of KOH for which the pH is 11.89? 2.) What is the pH of a 0.011M solution of Ca(OH)2? B. Weak Acid 1.) The pH of a 0.060M weak monoprotic acid HA is 3.44. Calculate the Ka of the acid. 2.) The pH
  3. Chemistry

    A 0.490 M solution of an unknown monoprotic weak acid, HA, is 2.80% ionized. What is the value of Ka for HA?
  4. chemistry

    Weak Acid 1.) The pH of a 0.060M weak monoprotic acid HA is 3.44. Calculate the Ka of the acid. 2.) The pH of 0.100M solution of weak monoprotic acid HA is 2.85. What is the Ka of the acid?
  5. chemistry

    Weak Acid 1.) The pH of a 0.060M weak monoprotic acid HA is 3.44. Calculate the Ka of the acid. 2.) The pH of 0.100M solution of weak monoprotic acid HA is 2.85. What is the Ka of the acid?
  6. Chemistry 104

    A 0.30M solution of a weak monoprotic acid is 0.41% ionized. what is the acid-ionization constant, Ka for this acid? Use. HA + H2O H3O + A to figure out X for H3O and A
  7. 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
  8. 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
  9. Chemistry-Dr Bob help!!

    0.100 M solution of a weak acid, HX, is known to be 15% ionized. The weak acid has a molar mass of 72 g/mol. 1. What is Ka for the weak acid? 2. What is the pH of the buffer prepared by adding 10.0 g of the sodium salt of the acid (NaX) to 100.0 mL of
  10. chemisty

    0.100 M solution of a weak acid, HX, is known to be 15% ionized. The weak acid has a molar mass of 72 g/mol. 1. What is Ka for the weak acid? 2. What is the pH of the buffer prepared by adding 10.0 g of the sodium salt of the acid (NaX) to 100.0 mL of
  11. AP CHEMISTRY

    Determine the volume of 0.125 M NaOH required to titrate to the equivalence point 25.0 mL of a 0.175 M solution of a monoprotic weak acid that is 20% ionized. Answer is 35.0 mL. How do you find it?! It's been a really long time since we talked about
  12. Chemistry

    A 0.108 M sample of a weak acid is 4.16% ionized in solution. what is the hydroxide concentration of this solution? I know that i set up an ice table. The equation would be weak acid + H20 goes to OH + the acid. What do i do with the 4.16 %? How does that
  13. Chemistry

    An unknown monoprotic acid has a pH of 2.87. Is this acid weak or strong if 22.32 mL of 0.112 M NaOH is required to titrate 25.00 mL of the acid? If the acid is weak, calculate its Ka. Answer is Ka = 1.8 x 10^-5, but I don't know how to get there. Any help
  14. 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
  15. Chemistry

    An aqueous solution of a monoprotic acid is prepared. This acid is known to have a pKa of 8.6. If the acid is 37.5% ionized when in solution, what is the pH of the solution? Not really sure where to start with this question? Thanks in advance
  16. AP Chemistry

    A 0.00100 M solution of a weak acid HX is 6% ionized. Calculate Ka for the acid.
  17. Chem

    a) A weak acid, HX, is 1.3% ionized in .20 M solution. What percent of HX is ionized in a .030 M solution? b) Does the percent ionization increase or decrease upon dilution? c) Does the H3O+ concentration of the above weak acid increase or decrease?
  18. chemistry

    a 23.74 mL volume of .0981 M NaOH was used to titrate 25 mL of a weak monoprotic acid solution to the stoichiometric point. determine the molar concentration of the weak acid solution. express in correct sig figs.
  19. Chemisty

    calculate pH of 50.0 mL of a .100 M solution of the weak monoprotic acid HX
  20. Chemistry

    A 0.10M solution of a certain monoprotic weak acid has a pH of 2.44. Calculate Ka.
  21. chemistry

    a 23.74 ml volume of .0981 M NaOH was used to titrate 25 mL of a weak monoprotic acid solution to the stoichiometric point. determine the molar concentration of the weak acid solution. Express your answer to the correct number of significant figures.
  22. chemistry

    2- A 0.310 M solution of a weak acid, HX, has a pH of 2.53 a. Find the [H+] and the percent ionization of nitrous acid in this solution. b. Write the equilibrium expression and calculate the value of Ka for the weak acid. c. Calculate the pH of the
  23. chemistry

    enzoic acid is a weak monoprotic acid with Ka = 6.5×10-5 M. NaOH(s) was gradually added to 1.00 L of 8.66×10-2 M benzoic acid. 1. Calculate the pH of the solution before the addition of the base. 2. Calculate the pH of the solution after the addition of
  24. chemistry

    A 0.040M solution of a weak acid has a pH of 3.02 at 25°C . What is the value of Ka for the acid?
  25. Chemistry

    I need help with this question, I don't know how to set up the formula to work it out? Calculate the dissociation constant of a weak monoprotic acid if a 0.08 M solution of this acid gives a hydrogen-ion concentration of 0.0001 M?
  26. Chemistry

    In a 1.760 M aqueous solution of a monoprotic acid, 3.21% of the acid is ionized. What is the value of it's Ka? x=1.760M * 3.21/100 - .0565M Ka expression is Ka= {[H+][A-]} / [HA]
  27. chemistry

    In a 1.070 M aqueous solution of a monoprotic acid, 4.81% of the acid is ionized. What is the value of its Ka?
  28. Chemistry

    The pH of a weak monoprotic acid, HA, is 4.55. It took 39.22 ml of 0.2334 M NaOH to titrate 25.00 ml of the acid. a. Write an equation for the above reaction. b. Calculate the molarity of the weak acid c. Write the equilibrium equation. Construct a table
  29. Chem

    stomach wall has a protective lining of mucous that prevent the acid from penetrating the underlying tissues. using asprin too often can damage the stomach wall. Aspirn is a weak carboxlyliic acid with a Ka of 3.2 x 10^-4. HC8H7O2CO2(aq) H^+(aq) +
  30. chemistry

    i need help solving this Benzoic acid is a weak, monoprotic acid (Ka = 6.3 × 10−5). Calculate the pH and the percent dissociation of each of the following solutions of benzoic acid. Then use Le Châtelier’s principle to explain the trend in percent
  31. chemistry

    Suppose that 0.483 g of an unknown monoprotic weak acid, HA, is dissolved in water. Titration of the solution with 0.250 M NaOH(aq) required 42.0 mL to reach the stoichiometric point. After the addition of 21.0 mL, the pH of the solution was found to be
  32. chemistry

    I have no clue, please help and explain! =) Find the pH of a 0.150 M solution of a weak monoprotic acid having Ka=1.2×10−5. Find the percent dissociation of this solution. Find the pH of a 0.150 M solution of a weak monoprotic acid having
  33. chemistry

    A 0.010 M solution of a weak monoprotic acid has a pH of 3.70. What is the acid-ionization constant, Ka, for this acid? a. 2.0 ´ 10-4 b. 2.0 ´ 10-5 c. 4.0 ´ 10-6 d. 4.0 ´ 10-7 e. 4.0 ´ 10-8
  34. Chemistry

    A sample of 0.314g of unknown monoprotic weak acid, HA was dissolved in 25.00 mL of water and titrated with 0.1M KOH. The acid required 27.20 mL of the base to reach equilibrium point. Find the pH of the solution if 40 mL KOH is added to the acid solution.
  35. chemistry

    The weak acid, HA, is 0.1 % ionized in a 0.2 M solution. (a) What is the equilibrium constant for the dissociation of the acid (Ka)? (b) What is the pH of the solution?
  36. chemistry

    The weak acid, HA, is 0.1 % ionized in a 0.2 M solution. (a) What is the equilibrium constant for the dissociation of the acid (Ka)? (b) What is the pH of the solution
  37. chemistry

    The weak acid, HA, is 0.1 % ionized in a 0.2 M solution. (a) What is the equilibrium constant for the dissociation of the acid (Ka)? (b) What is the pH of the solution
  38. Biochemistry

    weak acid, HA, is 0.1 % ionized in a 0.2 M solution. (a) What is the equilibrium constant for the dissociation of the acid (Ka)? (b) What is the pH of the solution?
  39. Chemistry

    The weak acid, HA, is 0.1 % ionized in a 0.2 M solution. (a) What is the equilibrium constant for the dissociation of the acid (Ka)? (b) What is the pH of the solution?
  40. chem

    A weak acid, HA, has an ionization constant of 9.29 x 10-6. If we prepare a solution that is 0.727 M in HA what percent of the acid will be ionized?
  41. chem

    A weak acid, HA, has an ionization constant of 4.34 x 10-8. If we prepare a solution that is 0.273 M in HA what percent of the acid will be ionized
  42. chemistry

    A 0.500M solution of a weak acid, HX, is only partially ionized. The [H+] was found to be 4.02 x 10^-3 M. Find the dissociation constant for this acid.
  43. Chemistry

    1 g of acid was mixed with 120 ml of distilled water and the solution was filtered into a clean dry beaker. A 25 ml aliquot of this solution was titrated with 0.1120 M NaOH. The pH of the acid was recorded to be 4.42. Calculate the initial concentration of
  44. chemistry

    the following titration data were collected: a 10 mL portion of a unknown monoprotic acid solution was titrated with 1.12340 M NaOH and required 23.95 mL of the base solution for neutralization. calculate the molarity of the acid solution calculate the
  45. Chemistry

    The pH of a 0.010 M aqueous solution of a weak monoprotic acid, HX, is 4.5. What is the value of the acid ionization constant?
  46. Chemistry

    The Ka of a monoprotic weak acid is 3.39 × 10-3. What is the percent ionization of a 0.125 M solution of this acid? I just do not know where to even start...
  47. chemistry

    A 0.010 M solution of a weak monoprotic acid is 3.0% dissociated. What is the equilibrium constant, Ka, for this acid?
  48. Chemistry

    The Ka of a monoprotic weak acid is 8.11 x 10 ^ -3. What is the percent ionization of a 0.125M solution of this acid?
  49. Chemistry

    The Ka of a monoprotic weak acid is 2.04 × 10-3. What is the percent ionization of a 0.181 M solution of this acid?
  50. Chemistry

    The Ka of a monoprotic weak acid is 4.47 × 10-3. What is the percent ionization of a 0.184 M solution of this acid?
  51. Chemistry

    The Ka of a monoprotic weak acid is 3.29 × 10-3. What is the percent ionization of a 0.176 M solution of this acid?
  52. Environmental Chemistry

    Calculate the pH when the following volumes of 10^(-1,1) M XOH are added into 1 L of a 10^(-2.5) M HA solution. XOH is a strong base and HA is a weak monoprotic acid (pKa=4.5)
  53. Chemistry

    If the Ka of a monoprotic weak acid is 4.5x10^-6 what is the pH of a .10M solution of this acid. I don't even know how to start this problem, I'm totally lost please help!
  54. chemistry

    a solution of 2.5 M weak acid is .52% ionized. what is the Ka value of this acid? ive been stuck on this one for a long time and cant figure out where to even start...if someone could walk me through this itd be great! thanks
  55. Chemistry

    1. Calculate the pH of a buffer solution that contains 0.32 M benzoic acid (C6H5CO2H) and 0.17 M sodium benzoate (C6H5COONa). [Ka = 6.5 × 10-5 for benzoic acid] Round your answer to two places past the decimal. 2. A solution is prepared by mixing 470 mL
  56. Chemistry

    1. Calculate the pH of a buffer solution that contains 0.32 M benzoic acid (C6H5CO2H) and 0.17 M sodium benzoate (C6H5COONa). [Ka = 6.5 × 10-5 for benzoic acid] Round your answer to two places past the decimal. 2. A solution is prepared by mixing 470 mL
  57. MATH

    A 0.26 M solution of a weak acid HA is 0.35 % ionized. What are the H+ , A- , and HA concentrations at equilibrium? What is Ka?
  58. Chemistry

    Suppose 50.0 mL of an aqueous solution containing an unknown monoprotic weak acid is titrated with 0.250 M KOH. The titration requires 31.52 mL of the potassium hydroxide solution to reach the equivalence point. What is the concentration (in molarity) of
  59. chemistry

    What is the pH of a solution of a monoprotic acid with a pKa of 6.6 if it is 39.3 % ionized in solution? Just provide the numerical answer, do not prefix with pH. Give your answer to two decimal places. Remember the definition of Ka
  60. Chemistry

    An unknown monoprotic weak acid, HA, has a molar mass of 65.0. A solution contains 2.20 g of HA dissolved 750. mL of solution. The solution has a pH of 2.200. What is the value of Ka for HA?
  61. Chemistry!! Please Help!

    A 0.285 M solution of the sodium salt, NaA, of the weak monoprotic acid, HA, has a pH of 9.65. Calculate Ka for the acid HA. I think I am having issues with the equation and then the math part. I figured out what 'x' was from the pH, which I believe is
  62. chemistry

    A certain monoprotic weak acid with Ka = 6.7 × 10-8 can be used in various industrial processes, but is no longer used in chemistry teaching labs because it tends to explode when it gets old. (a) What is the [H+] for a 0.558 M aqueous solution of this
  63. chemistry

    The pH of a 0.060 M weak monoprotic acid, HA is 3.44. Calculate the Ka of the acid.
  64. Chemistry

    What is the ionization constant for a weak acid HA that is 1.60% ionized in 0.095M solution?
  65. Chemistry

    For the weak acid HX, what is the pH of a 0.10 M solution if the acid is 4.0% ionized?
  66. chemistry

    For the weak acid HX, what is the pH of a 0.10 M solution if the acid is 4.0% ionized?
  67. Chemistry

    In a 0.05M solution of a weak monoprotic acid,[H+]=.0018.What is its Ka?
  68. Chemistry

    A 0.225g sample of a weak monoprotic acid requires 37.50 mL of 0.100 M NaOH solution to reach the equivalence point. What is the molar mass of the acid?
  69. Chemistry

    0.10 M solution of a weak monoprotic acid has a hydronium-ion concentration of 5.0 * 10^-4 M. What is the equilibrium constant, Ka, for this acid? a. 5.0 *10^-2 b. 5.0 * 10^-3 c. 2.5 * 10^-4 d. 2.5 * 10^-5 e. 2.5 * 10^-6 2. (Points: 1) What is the
  70. Chemistry

    I am trying to solve a buffer problem. I know I need to use the Henderson-Hasselblach equation but I am not getting the correct answer. The problem is: Propionic acid is a weak monoprotic acid with Ka = 1.3×10-5 M. NaOH(s) was gradually added to 1.00 L of
  71. science

    If the Ka of a monoprotic weak acid is 8.3 × 10-6, what is the pH of a 0.28 M solution of this acid?
  72. Chemistry

    If the Ka of a monoprotic weak acid is 4.3*10^-6, what is the pH of a 0.16 M solution of this acid?
  73. Chemistry

    If the Ka of a monoprotic weak acid is 9.0 × 10-6, what is the pH of a 0.26 M solution of this acid?
  74. chemistry

    Lactic acid is a weak acid with the formula , HCH3H5O3, the Ka for lactic acid is 1.38 x 10-4. In aqueous solution, lactic acid partially dissociates according to the following reaction: HCH3H5O3 ⇔ CH3H5O3- + H+ Use the Ka equation to calculate the pH of
  75. Chemistry

    44.70 ml of 0.100 M NaOH are required to completely neutralize 50.00 ml of a weak monoprotic acid, HA. When 34.43 ml of NaOH are added to another 50.00 ml of the acid, the pH reading was 4.80. Calculate Ka for the acid using the partial neutralization
  76. chem

    Acetic acid is a weak acid with the formula , CH3COOH, the Ka for acetic acid is 1.76 x 10-5. In aqueous solution, acetic acid partially dissociates according to the following reaction: CH3COOH ⇔ CH3COO- + H+ Use the Ka equation to calculate the pH of
  77. general chem

    A certain monoprotic weak acid with Ka = 0.49 can be used in various industrial processes. (a) What is the [H+] for a 0.191 M aqueous solution of this acid and (b) what is its pH? Round the [H+] to three significant figures and the pH to two places past
  78. general chem

    A certain monoprotic weak acid with Ka = 0.49 can be used in various industrial processes. (a) What is the [H+] for a 0.191 M aqueous solution of this acid and (b) what is its pH? Round the [H+] to three significant figures and the pH to two places past
  79. Chemistry

    Benzoic acid (C6H5COOH)is a monoprotic weak acid with Ka=6.30*10^-5. What is the pH of a solution of benzoic acid that is 0.559M and has 2.25*10^-2M NaOH added?
  80. Chemistry

    What volume of 0.200M of aqueous solution of formic acid, a weak monoprotic acid (KA = 1.78x10-4) and 0.200M aqueous solution of NaOH would you mix to prepare a 500mL of a buffer solution of pH = 4.0.
  81. chemistry

    Lactic acid is a weak monoprotic acid. If a 0.10 M solution of it has a pH of 2.44, what is the dissociation constant (Ka) for lactic acid. I got 1.3x10^-4? Is that right?
  82. chem

    Assume that 35.0 mL of a 0.13 M solution of a weak base B that accepts one proton is titrated with a 0.13 M solution of the monoprotic strong acid HX. (a) How many moles of HX have been added at the equivalence point?
  83. chemistry

    Captain Kirk, of the Starship Enterprise, has been told by his superiors that only a chemist can be trusted with the combination to the safe containing the dilithium crystals that power the ship. The combination is the pH of Solution A described below,
  84. Acid-Base chem

    Which of the following would for a buffer if added to 250.0 mL of .150 M SnF2? a).100 mol HCl b).060 mol HCl c).040 mol HCl d).040 mol NaOH e).040 mol HF I figured I could find out the pH of the solution with HCl/NaOH/HF added, and then find the pH when
  85. Chemistry

    The pH of an 0.0870 M solution of weak acid A is 2.20. The pH of an 0.0830 M solution of weak acid B is 4.07. The pH of an 0.0890 M solution of weak acid C is 5.13. Identify the three acids from among those listed below (the Ka values are listed in
  86. Chem

    if 0.24o moles of a monoprotic weak acid is titrated with NaOH, what is the PH of the solution at the 1/2 equivalence point.
  87. chemistry

    A student is given 3 beakers: Beaker 1- 50.0 ml of a solution produced by dissolving 6.00 grams of a weak monoprotic acid ,HX, in enough water to produce 1 liter of solution. The empirical formula of HX is CH2O. The solution contains 3 drops of
  88. Chemistry

    I Just don't know what to do, I think I understand, but im not sure because all of the compounds are liquid. I would know how to do it if they were aqueous, and just the water is liquid, but they are all liquid. Determine the acid dissociation constant for
  89. Chemistry

    A 50.0 mL sample of 0.51 M benzoic acid, C6H5COOH, a weak monoprotic acid, is titrated with 0.40 M NaOH. Calculate the pH at the equivalence point. Ka of C6H5COOH = 6.5 10-5. what am i supposed to do with this?
  90. chemistry

    A 0.1 molal solution of a weak monoprotic acid was found to depress the freezing point of water 0.1930C. Determine the Ka of the acid. You can assume 0.1 molal and 0.1 molar are equivalent.
  91. Chemistry

    At 20 degree celsius, Ka for an unknown monoprotic weak acid is 0.00088. Calculate the Delta G (in kJ/mol) for the reaction of this unknown acid with water. HA(aq) + H2O(l) H3O+(aq) + A-(aq)
  92. chemistry

    1)A solution has a [OH-] of 5.2 x 10-4. What is the [H3O+] in the solution? 2) A 0.25 M solution of a monoprotic acid, HA, has a pH of 2.54. What is Ka for this acid? The dissociation of HA is: HA + H2O H3O+ + A- (Hint: write the expression for pH) 3 A
  93. chemistry

    A 1.00M solution of a hypothetical weak acid (HB) has a pH of 2.85. A solution is created using 0.10M of a salt NaB ('B' being the anion of the weak acid HB) and 50.0 ml of 2.0M acid HB (assume no change in volume). What would be the pH of the solution and
  94. Chemistry

    A 50.0 mL sample of 0.42 M benzoic acid, C6H5COOH, a weak monoprotic acid, is titrated with 0.40 M NaOH. Calculate the pH at the equivalence point. Ka of C6H5COOH = 6.5 10-5. I know I have to set up an ICE chart, but I keep getting the wrong answer
  95. chemistry

    You need to determine the pKa of a weak, monoprotic acid. You add 0.500 moles of the acid to 1.00 L of water. The resulting pH was 1.87. What is the pKa of this weak acid? You may ignore the autoionization of water. 2.74 3.43 5.38 2.01 1.87
  96. chemistry

    A 1.213g sample of an unknown weak monoprotic acid was titrated to the endpoint with 27.25mL of a 0.3016M NaOH Calculate: -the number of moles of base reacted. -the number of moles of acid originally present. -the molar mass of the acid.
  97. Chem II

    A 0.10 M HF solution is 8.4% ionized. Calculate the H^+ ion concentration. The "8.4% ionized" is throwing me. This is my line of thinking. For every mole HF disolved yeilds one mole of H^+. Since there is 0.10 M HF and the solution is 8.4% ionized = 0.84
  98. Chemistry

    Acetic acid, HC2H3O2 is monoprotic. A 0.010M solution of lactic acid has a pH 2.44. calculate the ionization constant, Ka, for this acid.
  99. Mathematics

    Acetic acid, HC2H3O2 is monoprotic. A 0.010M solution of lactic acid has a pH 2.44. calculate the ionization constant, Ka, for this acid
  100. Chem

    A 0.649 m aqueous solution of a monoprotic acid (HA) freezes at -2.34°C. Find the pKa of this monoprotic acid. Kf of water = 1.86 °C/m

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