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.

36,390 results
  1. CHEMISTRY

    HOW CAN U TELL IF HNO3 +KNO3 IS A BUFFER SOLUTION A buffer solution must contain a weak acid and its conjugate base OR a weak base and its conjugate acid. HNO3 is a strong base and KNO3 is the salt of a strong base (KOH) and a strong acid (HNO3);

  2. 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

  3. chemistry

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

  4. 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

  5. Chemistry

    Lactic acid, a chemical responsible for muscle fatigue, is a monoprotic acid. When 0.578 g of lactic acid is titrated with 0.206 M NaOH, a volume of 31.11 mL of NaOH is used. What is the molar mass of lactic acid? HA + NaOH > NaA + H2O (also does the A

  6. 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

  7. 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%)

  8. Chem 1A

    A 15.00 g sample of an ionic compound NaA, where A- is the anion of a weak acid, was dissolved in enough water to make 100.0 mL of solution and was then titrated with 0.100 M HCl. After 700.0 mL of HCl was added, the pH was 5.00. The experimenter found

  9. 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

  10. organic chemistry

    1)Why benzoic acid is soluble in NaOH? 2)Why HCl is insoluble in titration of benzoic acid and NaOH? Benzoic is soluble in a solution of NaOH because the base forms the sodium salt with the acid to form sodium benzoate. The sodium salt is soluble. The

  11. 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

  12. 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

  13. Chemistry

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

  14. 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,

  15. 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

  16. 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!

  17. 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?

  18. chemistry

    1.The equilibrium constant for the oxidation of elemental iron metal, Fe, by oxygen, O2 to form hematite, according to the reaction 2Fe + (3/2)O2 = Fe2O3 is known to have the value K=exp(+68.8) at 1000C. The equilibrium constant for the formation of CO2

  19. 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

  20. Chemistry

    You are asked to prepare a pH = 4.00 buffer starting from 1.50 L of 0.0200 M solution of benzoic acid (C6H5COOH) and some added sodium benzoate salt (C6H5COONa). a) Find the pH of the benzoic acid solution BEFORE adding the salt. b) Use the

  21. 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

  22. 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

  23. 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?

  24. 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

  25. 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

  26. 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?

  27. 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?

  28. Chemistry

    Just some homework. Would like to know if I am right, thanks. 1. Adding salt of a weak acid to a solution of the weak acid: a)lowers the concentration of the nonionized acid and the concentration of the H30+ b)lowers the concentration of the nonionized

  29. 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

  30. 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^- +

  31. Chemisty

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

  32. 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

  33. 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

  34. 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

  35. Chemistry

    Identify the salt that is produced from the acid-base neutralization reaction be- tween sodium hydroxide and hydrocyanic acid (HCN). 1. sodium cyanide 2. sodium acetate 3. sodium amide 4. sodium formate

  36. 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

  37. Chemistry

    Salt of a Strong Base and a Weak Acid. pH of Solution. Calculate the pH of a 5.90×10-1 M aqueous solution of sodium nitrite (NaNO2). (For nitrous acid, HNO2, Ka = 4.00×10-4).

  38. 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,

  39. Chemistry

    Propanoic acid that, along with its sodium salt, can be used to make a buffer that has a pH of 5.25. If you have 532.9 mL of a 0.250 M solution of that acid, how many grams of the corresponding sodium salt do you have to dissolve to obtain the desired pH?

  40. 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

  41. 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

  42. 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

  43. Chemistr ll

    A buffer solution is composed of 0.370M HA, a weak monoproctic acid, and 0.370M NaA, the sodium salt of the acid. The solution has a pH of 3.50. What is the Ka of the weak acid, Ha?

  44. chemistry

    a) What is fellesioneffekten? Veronal is a barbiturate (structure see above). Barbiturates is a substance class which occur in a variety of drug classes, including sleep medications (hypnotikasedativa), in painkillers (anesthetics) and anticonvulsants. A

  45. chemistry

    #1)hydrochloric acid is a relatively strong acid . imagine that HCl is added to a buffer solution containing the weak acid phosphoric acid and a salt a)will HCl react with weak acid (H3PO4), or will it react with the salt (Na2HPO4)? b)one product of this

  46. 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

  47. 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.

  48. 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

  49. Chem. Again

    28: You have a glass of pure water. Are chemical reactions occurring in the water? If so, what are they? If not, explain why not. 29: While investigating the effects of acid rain in your area, you discover a lake that is surprisingly resistant to changes

  50. Chemistry

    An aqueous sodium salt (NaCnH2n+1O3) solution has an osmotic pressure of 2.041 atm when 1.068 g of the salt are dissolved in 200. g of water at 25 degrees C. Assuming molality and molarity in such a dilute solution are the same and that the sodium salt is

  51. 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

  52. Chemistry

    You are asked to prepare a pH = 4.00 buffer starting from 1.50 L of 0.0200 M solution of benzoic acid (C6H5COOH) and some added sodium benzoate salt (C6H5COONa). a) Find the pH of the benzoic acid solution BEFORE adding the salt. b) Use the

  53. 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

  54. 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?

  55. 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

  56. Chemistry

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

  57. 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?

  58. 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?

  59. 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?

  60. 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

  61. Chemistry

    Only a chemist can be trusted with the combination to the safe containing a ton of money. The combination is the pH of solution A, followed by the pH of solution C. (for example: is the pH of solution A is 3.47 and the pH of solution C is 8.15 the

  62. 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

  63. Chemistry

    Asolution contains a weak monoprotic acid HA and its sodium salt NaA both at 0.1 M concentration. Show that [OH] Kw/Ka.

  64. chemistry

    A buffer solution is composed of 0.370M HA, a weak monoproctic acid, and 0.370M NaA, the sodium salt of the acid. The solution has a pH of 3.50. What is the Ka of the weak acid, Ha?

  65. 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

  66. 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?

  67. 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

  68. 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

  69. college-chemistry

    calculate the ph of a buffer solution prepared by adding 0.397 mole of the sodium salt of a weak organic acid HA to 0.474 L of 1.023m acid HA with pka=4.82 and diluting to 1.00 L WITH WATER

  70. chem

    Can someone please help me by explaining and correcting me? 1) A 0.057M solution of a weak acid has a pH of 4.93. Determine the ionization constant, Ka, of the acid. a) 2.1 x 10^-4 b) 2.4 x 10^-9 c) 4.1 x 10^-8 d) 2.8 x 10^-7 e) 1.4 x 10^-10 -- To be

  71. 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?

  72. chem

    When 0.285 g of a solid weak acid HA (molar mass = 184 g mol−1) is dissolved in water to a total volume of 25.0 mL, the pH of the solution is 3.59. What is the acid ionization constant (Ka) of the acid?

  73. 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

  74. 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?

  75. Chemistry

    The molar mass of an organic acid was determined by the following study of its barium salt. 4.290 g of the salt were to be converted to the free acid by reaction with 21.64 mL of 0.477 M H2SO4. The barium salt was known to contain 2 moles water of

  76. 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

  77. 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?

  78. 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.

  79. chemistry - titration

    Show that for the titration of a weak acid, HA, with NaOH solution, at half-titer, pH = pKa. Please explain your answer. Thank you. HA + NaOH ==> NaA + HOH Ka for HA = (H^+)(A^-)/(HA) and solve for H^+. (H^+) = Ka*[(HA)/(A^-) When HA is half neutralized,

  80. 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?

  81. 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

  82. chem

    the pH of a .100 M solution of sodium formate = 8.37. Calculate the value of Ka of formic acid. okay so I know that the anion of a weak acid is itself a weak base so A- +H2O---> OH- + HA pOH =14-8.37 so conc of OH is 10^-5.63 Ka=[OH][HA]/[A-] so we know

  83. 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.

  84. chemistry

    Hello! Please correct me if I'm wrong. For the following compound, predict whether the solution is acidic, basic, or neutral and why: NH4Cl. a) acidic, NH4Cl is the salt of a weak base b) neutral because there is no hydrolysis c) acidic, NH4Cl is a strong

  85. chemistry

    The following questions are about the reaction of sodium oxide with nitric acid. 1)What mass of sodium oxide would be needed to react with acid to form 0.5 mol salt? I said 1.5 2) How much sodium oxide would be required to neutralise 230cm3 of 1.0moldm-3?

  86. 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.

  87. chemistry

    hello, I can't seem to solve this question. i tried to look up someone else who may have asked this question. I found this girl named Sara,but her answer didn't really help me much because it did not answer the question. What is the pH when enough 0.10 M

  88. chemistry

    hello, I can't seem to solve this question. i tried to look up someone else who may have asked this question. I found this girl named Sara,but her answer didn't really help me much because it did not answer the question. What is the pH when enough 0.10 M

  89. chemistry

    A SOLUTION OF 0.05METER ACID PKA 6.10 IS MIXED WITH AN EQUAL VALUE 0.1 SODIUM SOLUTION OF SODIUM SALT WHAT IS THE PH OF THE FINAL MIXTURE.

  90. Chemistry

    My question talks about a buffer with HA and NaA, where NaA is the sodium salt of the acid. What does the equation for this look like? HA + NaA --> H+ + NaA2 ??

  91. chemistry

    a) What is fellesioneffekten? Veronal is a barbiturate (structure see above). Barbiturates is a substance class which occur in a variety of drug classes, including sleep medications (hypnotikasedativa), in painkillers (anesthetics) and anticonvulsants. A

  92. 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.

  93. chemistry-confirm please

    Only a chemist can be trusted with the combination to the safe containing a ton of money. The combination is the pH of solution A, followed by the pH of solution C. (for example: is the pH of solution A is 3.47 and the pH of solution C is 8.15 the

  94. 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.

  95. 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...

  96. 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?

  97. 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?

  98. 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?

  99. 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?

  100. 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

Pages

  1. 1
  2. 2
  3. 3
  4. 4
  5. 5
  6. 6
  7. 7
  8. 8
  9. 9
  10. 10
  11. 11
  12. 12
  13. 13
  14. 14
  15. 15
  16. 16
  17. 17
  18. 18
  19. 19
  20. 20