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A is a solution of trioxonitrate(v)acid (nitric acid) HNO3 of unknown concentration.B is a standard solution of sodium hydroxide containing 4.00g per dm3 of solution a). Suggest with a reason,a suitable indicator for the reaction b) Write a balanced equation

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  1. Chemistry

    A is a solution of trioxonitrate(v)acid (nitric acid) HNO3 of unknown concentration.B is a standard solution of sodium hydroxide containing 4.00g per dm3 of solution a). Suggest with a reason,a suitable indicator for the reaction b) Write a balanced
  2. chemistry

    A is a solution of trioxonitrate(v) acid, HNO3, of unknown concentration. B is standard solution of sodium hydroxide containing 4.00g per dm3 of solution. 25cm3 portions solution B required an average of 24.00cm3 of solution A for neutralization, using
  3. Chemistry

    A is a solution of trioxonitrate (v)acid, HNO3 of unknown concentration.B is standard solution of sodium hydroxide containing 4.00g per dm3 of solution. 25 cm3 portion solution B required an average of 24.00cm3 of solution A for neutralization using 2drops
  4. chemistry

    A nitric acid solution of unknown concentration is used to titrate 0.771g of sodium tyrosinate (NaC9H10NO3). If the endpoint is reached when 32.79mL of nitric acid has been added, what is the concentration of the unknown nitric acid solution?
  5. Chemistry practical

    Table reading for A is a solution of trioxonitrate (iv) acid of unknown concentration B is a standard solution of sodium hydroxide NaoH containing 4.00, 25cm3 portion of solution A for complete neutralization 1 state with a reason a suitable indicator 2
  6. CHEMISTRY

    A is a solution of trioxonitate acid of an unknown concentration, B is a standard solution of sodium hydroxide containing 4.00g per dm3 of solution 25cm3 portion of solution B require an average of 24cm3 of solution A for complete neutralization. Write a
  7. CHEMISTRY

    A is a solution of trioxonitate acid of an unknown concentration, B is a standard solution of sodium hydroxide containing 4.00g per dm3 of solution 25cm3 portion of solution B require an average of 24cm3 of solution A for complete neutralization. Write a
  8. Chemistry, pH, Buffers

    Please help!! Given this data: mass of unknown acid 1.4671g Volume of NaOH used in titration 18.47mL Concentration of the NaOH used 0.2403M pH of the original acid solution 2.16 pH of the final acid solution 3.49 Show me how do I calculate the Ka of the
  9. 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
  10. College Chemistry

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

    Hi could someone please help me in the next 5 minutes with this question: Given this data: mass of unknown acid 1.4671g Volume of NaOH used in titration 18.47mL Concentration of the NaOH used 0.2403M pH of the original acid solution 2.16 pH of the final
  12. Chemistry

    A is a solution of trioxonitrate (V) acid. HNO of unknown concentration B is standard solution of sodium hydroxide containing 4.00g per dm3 of solution 25cm3 portion solution B required an average of 24.00cm3 of solution A for neutralization. Using 2 drop
  13. Chemistry

    1) What volume of 1.25 mol/L hydrobromic acid, HBr(aq) will neutralize 75.0 ml of 0.895 mol/L magnesium hydroxide Mg(OH)2(aq)? 2) a 25.00 mL sample of a nitric acid solution , HNO3(aq) is neutralized by 18.55mL of a 0.1750 mol/L sodium hydroxide, NaOH(aq)
  14. Chemistry

    1) What volume of 1.25 mol/L hydrobromic acid, HBr(aq) will neutralize 75.0 ml of 0.895 mol/L magnesium hydroxide Mg(OH)2(aq)? 2) a 25.00 mL sample of a nitric acid solution , HNO3(aq) is neutralized by 18.55mL of a 0.1750 mol/L sodium hydroxide, NaOH(aq)
  15. chemistry(Urgent Please help)

    A student is asked to standardize a solution of barium hydroxide. He weighs out 0.945 g potassium hydrogen phthalate (KHC8H4O4, treat this as a monoprotic acid). It requires 33.9 mL of barium hydroxide to reach the endpoint. A. What is the molarity of the
  16. Chemistry

    A solution containing nitric acid (HNO3) is to be used in the neutralization titration of a sodium hydroxide (NaOH) solution. a. If the pH of the nitric acid solution is 2.30, what is the normality of the nitric acid? b. If 27.00 ml of the nitric acid
  17. chemistry

    A commercial sample of concentrated aqueous nitric acid (HNO3) is 18.2% nitric acid base mass and has a density of 1.12 g/mL. (a) What is the molarity (M) of the HNO3 solution? (b) What is the molality (m) of the HNO3 solution? -------- I know that.... (a)
  18. chemistry

    You need to determine the concentration of a sulfuric acid solution by titration with a standard sodium hydroxide solution. You have a 0.1896 M standard solution. You take a 25.00 mL sample of the original acid solution and dilute it to 250.0 mL. You then
  19. 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
  20. CHEMISTRY

    A solution of trioxonitrate (V) acid contained 0.67g in 100cm3. 31.0cm3 of this solution neutralized 25cm3 of a sodium trioxocarbonate (IV) solution. Calculate the concentration of the trioxocarbonate (IV) solution. (HNO3 = 63, Na2CO3 = 106)
  21. algebra

    Two acid solutions are available to a chemist. One is 10% nitric acid solution, the other is 4% nitric acid solution. How much of each type of solution should be mixed together to form a 600 ml of a 6% nitric acid solution?
  22. Chemistry

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

    Traffic in the cities releases NOx gases into the atmosphere (in the form of NO and NO2). NOx gases contribute to rainwater acidification by dissolving and transforming into a strong acid (HNO3, nitric acid) according to the reaction below: 4 NO + 3 O2 + 2
  24. chem

    An aqueous solution of nitric acid has a density of 1.084 g mL-1 and a measured concentration of 2.580 molar. What is the percent weight of nitric acid in the solution.
  25. Chemistry

    Help me with this; For the second part of the analysis,you will be provided with hydrated crystal of oxalic acid (H2C204. 2H2O). weigh out accurately about 1.575g of oxalic acid in a weighing bottle. Dissolve the acid in a beaker, then transfer the
  26. Chemistry

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

    In an acid base titration,25.0 ml of nitric acid, HNO3, were neautralized by 28.0 mL of 0.209 mol/L calcium hydroxide, Ca(OH)2. What is the concentration of the nitric acid?
  28. Chemistry

    An 8 Molar (aqueous) solution contains H2O and HNO3. The solution has an S.G. of 1.24 at 25oC. HNO3 is a strong acid that completely dissociates in water. a) Calculate the mass of I Litre of solution. b) Calculate the mass concentration (g/L) of HNO3 in
  29. chemistry

    An aqueous solution of nitric acid is standardized by titration with a 0.121 M solution of calcium hydroxide. If 24.5 mL of base are required to neutralize 15.4 mL of the acid, what is the molarity of the nitric acid solution?
  30. Chemistry

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

    If a rate of 80.0 mL of an aqueous solution of potassium hydroxide concentration of 0.25 mol / L are partially neutralized by 20.0 mL of an aqueous solution of nitric acid concentration of 0.50 mol L. Determine pH of the final solution. kOH + HNO3 -> H2O +
  32. Chemistry

    The nitric acid was purchased as a solution that has 70% HNO3. That volume (mL) of this solution is necessary for preparing 250 mL Solution 2.0 mol L-1? The density of HNO3 (aq) 70% is 1.42 g cm-3
  33. Chemistry 12

    In s 0.30 mol/L HNO3(aq) solution. a) what is the concentration of nitric acid molecules. b)what is the hydroxide ion concentration?
  34. chemistry

    You were given 25.00 ml of an acetic acid solution of unknown concentration. You find that it requires 29.60 ml of a 0.1050 M NaOH solution to exaclty neutralize this sample. A) What is the molarity of the acetic acid solution? B) what is the percentage of
  35. chemistry

    Suppose that 50mL of a solution of sulfuric acid of unknown concentration was titrated with a 0.100M solution of sodium hydroxide. If it took 45.5 mL of titrant to reach the equivalence point, what was the concentration of the unknown solution of sulfuric
  36. Chemistry

    1. What is the pH of a 1.0 x 10-3 M solution of boric acid, H3BO3? The Ka value for boric acid is 6 x 10-10. (choices: 3, 7, between 7 and 12, between 3 and 7) 2. You want to use a 0.500 M HNO3 solution to titrate an unknown concentration of KOH solution.
  37. Chemistry 12

    9. According to Arrhenius, which of the following groups contain: i)only acids ii)only bases a. NaOH, H2CO3, KCl b. MgCl2, H2SO4, HCl c. HNO3, HCl, H3PO4 d. Mg(OH)2, AgBr, HF e. KOH, NH4OH, Ba(OH)2 10. Enough water is added to 100 g of sodium hydroxide in
  38. Chemistry-please help

    "Use a 10% w/v nitric acid solution." How to prepare 10% w/v nitric acid solution? Do I just weigh 10g of conc nitric acid (65%) and dilute to 100ml with water?
  39. chemisty

    A nitric acid solution is neutralized using sodium hydroxide. How many grams of sodium hydroxide are needed to neutralize 5.50 L of 1.200 M nitric acid solution? HNO3 (aq) + NaOH (aq) → H2O (l) + NaNO3 (aq)
  40. Chem

    Which of the following are true regarding acid-base titrations? A They are used to determine the concentration of an unknown acid or base. B The acid or the base must be a standard solution with a known concentration C The standard solution is titrated
  41. 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
  42. Chemistry

    Expt #1- Molecular Weight of Unknown Acid Unknown Acid: #2 Mass of Unknown solid acid transferred:0.414g Volume of volumetric flask: 100.00 mL Concentration of NaOH: 0.0989 M Aliqot of acid titrated with NaOH: 25.00 mL Average volume of Naoh from
  43. 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);
  44. Chemistry 104

    Nitric acid, HNO3, is available commercially at a concentration of 16 M. What volume would you use to prepare 770 mL of a 0.19 M solution?
  45. Chemistryyy

    a) A standard solution of 0.243 M NaOH was used to determine the concentration of a hydrochloric acid solution. If 46.33 mL of NaOH is needed to neutralize 10.00 mL of the acid, what is the molar concentration of the acid? b) A 0.150 M sodium chloride
  46. science

    The concentration of commercially available concentrated nitric acid is 70% , or 15.9M In 100 grams of solution there are 1.11 mol of HNO3. Calculate the volume of 100 g of the Solution.
  47. Chemistry

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

    My professor gave us two homework questions that are a bit confusing, can you help me to get started on them. 1) You have 6g of water (Kf=1.86 C kg/mol). You add and dissolve 2.1 g of a different unknown substance. The freezing point of the solution is
  49. science

    6g of impure NaOH was dissolved in 100ml of a solution.0.25molar solution of the base utilize 27.6ml of the solution containing 6g of trioxonitrate(5)acid.calculate (a)molar concentration of acid (b) molar concentration of base (c) mass of the base (d) %
  50. general, organic and biochemistry

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

    600 mL of an unknown monoprotic acid was titrated with a standard solution of a 1.0 M base. If it took 40.0 mL of the base to neutralize the acid, what was the H+ ion concentration of the acid in moles per Liter?
  52. Chemistry

    A contains 1.60g of trioxonitrate(v) acid in 250cm³ of the solution. B contains 9.0gdm3 of XHCO3, 25cm³ portions of B required an average of 24.90cm³ of A for complete neutralization, calculate the: a) concentration of acid in A in mol/dm³. b)
  53. Chemistry

    How many resonance structures do these following acids have? H2CO3-carbonic acid H3PO4-phosphoric acid H2SO4-sulfuric acid HNO3-nitric acid CH3COOH- acetic acid CH2ClCOOH- chloroacetic acid CHCl2COOH- dichloroacetic acid CCl3COOH- trichloroacetic acid
  54. Chemistry 12

    15. The concentration of hydroxide ions in a solution of nitric acid 0.2 M is: a. 2 x 10-14 M b. 5 x 10-14 M c. 5 x 10-7 M d. 2 x 10-1 M 16. Aqueous solutions of strong acids and strong bases: a. are good electricity conductors b. make litmus paper become
  55. chemistry

    The density of 19.0% by mass of nitric acid, HNO3 is 1.11 g cm-3. Calculate the volume (dm3) of acid needed to prepare 2.00 dm3 of 3.00 mol dm-3 HNO3 solution. (FW HNO3 = 63 g/mol)
  56. Chemistry

    A 23.16 ml volume of an H2A acid solution of unknown concentration with 2 drops of phenolphthalein required 14.24 ml of 0.135 M NaOH to reach the endpoint. What is the molar concentration of the acid solution?
  57. Chemistry

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

    A solution of sodium carbonate of concentration 0.100moldm-3 is used to standardize a solution of hydrochloric acid. 25cm3 of the standard solution of sodium carbonate require 35cm3 of the acid for neutralization. Calculate the concentration of the acid.
  59. chemistry

    A nitric acid solution containing 71.0% by mass of the acid has a density of 1.42g/ml how many grams of nitric acid are present in 1.0L of this solution
  60. Chemistry

    A solution of trioxonitrate(v)acid contains 0.63g in 100cm³. 28.0cm³of this solution neutralized 25cm³of sodiumtrioxocarbonate(iv) solution. Calculate the molar concentration and mass concentration of sodiumtrioxocarbonate(iv)
  61. chemistry

    25 mL of nitric acid of an unknown molarity are used. the end point of the titration was reached using the basic solution. what is the molarity of the nitric acid?
  62. chemistry

    sorry to keep bugging you, but if it makes you feel better i am understanding it more. what if you have the same numbers, but you are trying to find the concentration of an UNKNOWN acid. all you have is: Volume of Unknown Acid Volume of Stock Solution
  63. science

    A solution of trioxonitrate(V) acid contained 0.67g in 100cm^3. 31.0cm^3 of this solution neutralized 2.5cm^3 of a sodium trioxocarbonate(IV) solution. calculate the concentration of the trioxocarbonate(IV) solution.
  64. Chemistry

    If it requires 23.4 milliliters of 0.65 molar barium hydroxide to neutralize 42.5 milliliters of nitric acid, solve for the molarity of the nitric acid solution. Show all of the work used to solve this problem. Unbalanced equation: Ba(OH)2 + HNO3 ->
  65. Science

    If it requires 23.4 milliliters of 0.65 molar barium hydroxide to neutralize 42.5 milliliters of nitric acid, solve for the molarity of the nitric acid solution. Show all of the work used to solve this problem. Unbalanced equation: Ba(OH)2 + HNO3 ->
  66. Chemistry

    I have a .283M of Nitric acid in 5500 kg of water. How much of 68% Nitric acid do I need to add to make the nitric acid solution 0.3M?
  67. Chemistry

    Hi! I really really need help in this question: what observation is expected when: 1. an acid (nitric acid, HNO3) is added to a solution containing carbonate or bicarbonate ions? 2. silver ion is added to a solution containing chloride (or bromide or
  68. Chemistry- PLEASE HELP

    Hi! I really really need help in this question: what observation is expected when: 1. an acid (nitric acid, HNO3) is added to a solution containing carbonate or bicarbonate ions? 2. silver ion is added to a solution containing chloride (or bromide or
  69. Chem

    Using the standardized NaOH solution, the student weighs out 0.2550g of a solid unknown acid and finds that 28.50mL of the NaOH solution is required to reach an end point with the acid. Calculate the molar mass of the unknown acid, assuming the acid is
  70. Chem

    Using the standardized NaOH solution, the student weighs out 0.2550g of a solid unknown acid and finds that 28.50mL of the NaOH solution is required to reach an end point with the acid. Calculate the molar mass of the unknown acid, assuming the acid is
  71. Chemistry

    You wish to prepare 0.18 M HNO3 from a stock solution of nitric acid that is 18.9 M. How many milliliters of the stock solution do you require to make up 1.00 L of 0.18 M HNO3? Answer and..... HOW DO I DO IT?
  72. chemistry

    A 116.9 g sample of nitric acid solution that is 70.0% HNO3 contains how many moles of HNO3? how did you get the answer
  73. CHEMISTRY

    A 116.9 g sample of nitric acid solution that is 70.0% HNO3 contains how many moles of HNO3? how did you get the answer
  74. Chemistry

    Hi! My name's Isabow! can someone please help with this question? Thanks in advance :3
  75. chemistry

    A 116.9 g sample of nitric acid solution that is 70.0% HNO3 (by mass) contains how many moles of HNO3? how did you get the answer
  76. chemistry

    detail how to dilute a stock solution of nitric acid, 81 m HNO3, to prepare 675 ml of a 2.5 M solution
  77. Chemistry

    A is a solution of HNO3 of unknown concentration. B is a standard solution of Naoh 25cm3 portion of solution B required an average of 24.00cm3 of solution A for complete neutralization. (1) suggests with reason a suitable indicator for the reaction
  78. Chemistry

    You have 500 mL of a 5.0 M solution of nitric acid HNO3 (63.01 g / mol) dissolved in water. How many grams of nitrogen does the solution contain?
  79. Chemistry titrations

    25.00mL of an unknown sulfuric acid solution is titrated to the second equivalence point with 21.02mL of 0.420M potassium hydroxide solution. What is the concentration of the sulfuric acid solution?
  80. Science

    A is a solution of trioxonitrate nitrate (v) (HNO3) of unknown concentration, B is a standard solutions of NAOH containing 4.00g/dm3 of solutions 25.0cm potion of solutions B required an average of 24.00cm of solutions A for complete neutralization
  81. Chemistry

    You wish to prepare 0.18 M HNO3 from a stock solution of nitric acid that is 18.9 M. How many milliliters of the stock solution do you require to make up 1.00 L of 0.18 M HNO3?
  82. Chemistry

    40.0 ml of an acetic acid of unknown concentration is titrated with 0.100 M NaOH. After 20.0 mL of the base solution has been added, the pH in the titration flask is 5.10. What was the concentration of the original acetic acid solution? (Ka(CH3COOH) = 1.8
  83. Chemistry

    40.0 ml of an acetic acid of unknown concentration is titrated with 0.100 M NaOH. After 20.0 mL of the base solution has been added, the pH in the titration flask is 5.10. What was the concentration of the original acetic acid solution? [Ka(CH3COOH) = 1.8
  84. college Chemistry

    Hydrobromic acid is a strong acid. If you have 1 L of a 7.5 M solution of Hydrbromic acid? A) What is the concentration of H_3O^+? B) What is the PH of this solution? C) If you dilute 1 liter of 7.5M in HBR solution to a volume of 2 L what is the new
  85. Chemistry

    A solution is prepared by adding 47.3 mL of concentrated hydrochloric acid and 16.3 mL of concentrated nitric acid to 300 mL of water. More water is added until the final volume is 1.00 L. Calculate [H+], [OH -], and the pH for this solution. [Hint:
  86. Chemistry

    A solution is prepared by adding 50.3 mL of concentrated hydrochloric acid and 16.6 mL of concentrated nitric acid to 300 mL of water. More water is added until the final volume is 1.00 L. Calculate [H+], [OH -], and the pH for this solution. [Hint:
  87. chemistry

    1. if 15.0mL of 4.5 M NaOH are diluted with water to a volume of 500mL, what is the molarity of the resulting solution? 2. in a acid-base titration, 33.65mL of an 0.148 M HCL solution were required to neutralize 25.00mL of a NaOH solution. What is the
  88. chemistry

    You need to prepare 500.00 mL of a 0.15 M solution of nitric acid . Concentrated nitric acid comes from the chemical copmanies as a 15.8 M liquid. How much (in mL) of this 15.8 M solution will you need to dilute to 500.00 mL to get the desired 0.15 M
  89. chemistry

    You need to prepare 500.00 mL of a 0.25 M solution of nitric acid . Concentrated nitric acid comes from the chemical copmanies as a 15.8 M liquid. How much (in mL) of this 15.8 M solution will you need to dilute to 500.00 mL to get the desired 0.25 M
  90. Chemistry

    At 298.K and 1.00 atm, assume that 22 mL of NO gas reacts with 18 mL of oxygen gas and excess water to produce nitric acid according to the following equation: 2 NO(g) + 3/2 O2 (g)+ H2O(l)?? 2 HNO3(g). If all of the nitric acid produced by this reaction is
  91. chemistry

    Which masses of HNO3 nitric acid and water should be mixed to prepare 1000 grams of UAM 8% solution in mass of HNO3?
  92. Chemistry

    A nitric acid solution is found to have a pH of 2.70. Determine [H3O+],[OH-], and the number of moles of HNO3 required to make 5.50L of the solution.
  93. Chemistry

    A sample of 25.00 mL of vinegar is titrated with a standard 1.02 M NaOH solution. It was found that a volume of 19.60 mL of the standard NaOH solution is used to completely neutralize the acetic acid in the solution. Calculate the concentration of the
  94. SCIENCE

    A nitric acid solution at 25% by weight has a density of 1.21 KG / L Calculate the volume needed to be taken to obtain 2 L of a 2.5 M solution of nitric acid
  95. chemistry

    How many milliliters of concentrated nitric acid, HNO3, 70 % (wt/wt) are required to prepare 1 liter of 0.250 M solution? The molar mass and density of HNO3 are 63.0 g/mol and 1.36 g/cm respectively.
  96. Science(Chemsitry)

    HNO3 used as a reagent has specific gravity of 1.42g/ml and contains 70% by strength HNO3. Calculate a)Normality Of Acid b)Volume of acid that contains 63g pure acid c)Volume of water required to make 1N solution from 2ml conc.HNO3
  97. Titration/Acid-base chem

    a .4000 M solution of nitric acid is used to titrate 50.00 mL of .237 M barium hydroxide (Assume that volumes are additive). a) Write a balanced net ionic equation for the reaction that takes place during titration. b) what are the species present at the
  98. Chemistry

    A solution of 0.2M nitric acid is to be prepared from a 4.5M solution. How much nitric acid needs to be diluted in a50ml volumetric flask?
  99. science

    Hydrochloric acid is a strong acid. Acetic acid is a weak acid. Which statement about hydrochloric acid and acetic acid is correct?(1 point) The dissociation constant for hydrochloric acid is greater than the dissociation constant for acetic acid. The
  100. Chemistry

    Calculate the molar concentration of a solution of nitric acid if 20.00 mL of the acid requires12.63 mL of 0.155 M NaOH to reach the equivalence point.

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