0.250g of phthalic acid is dissolved in 40.00cm^3 of 0.100 mol dm^-3 NaOH. It requires 11.80 cubic centimeters of 0.100 mol\dm^-3 HCL fo neutralisation( to phenolphthalein) The mole ratio in which phthalic acid reacts with sodium hydroxide ihn 1:2 (a)

40,047 results
  1. Chemistry

    Commercial vinegar was titrated with NaOH solution to determine the content of acetic acid, HC2H3O2. For 20.0 milliliters of the vinegar 26.7 milliliters of 0.600-molar NaOH solution was required. What was the concentration of acetic acid in the vinegar if

  2. Chemistry

    A 1.00 g sample of limestone is allowed to react with 100 cm^3 of 0.200 mol/dm^3 HCl. The excess acid required 24.8 cm^3 of 0.100 mol/dm^3 NaOH solution. Calculate the percentage of calcium carbonate in the limestone

  3. Chemistry

    Ethanoic acid can be reacted with alcohols to form esters, an equilibrium mixture being formed. CH3CO2H + ROH CH3CO2R + H2O The reaction is usually carried out in the presence of an acid catalyst. In an experiment to determine Kc a student placed together

  4. CHEMISTRY

    A 1.575 g sample of ethanedioic acid crystals, H2C2O4. xH20 was dissolved in water and made up to 250cm^3 . One mole of the acid reacts with two moles of NaOH. In a titration, 25.0 cm^3 of this solution of acid reacted with exactly 15.6 cm^3 of 0.160 mol/

  5. Chemistry

    1.) Watch the animation, and observe the titration process using a standard 0.100 M sodium hydroxide solution to titrate 50.0 mL of a 0.100 M hydrochloric acid solution. Identify which of the following statements regarding acid-base titrations are correct

  6. Chemistry

    1.025g of an impure sample of a weak acid HX(mol mass = 82) is dissolved in 60ml of water and titrated with 0.25M NaOH. When half of the acid was neutralized the pH was found to be 5.0 and at the equivalence point the pH is 9.0. Find the % purity of this

  7. 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

  8. science

    the teacher instructed three students A,B,and C respectively to prepare a 50% (mass by volume) solution of sodium hydroxide (NaOH). 'A' dissolved 50 g of NaOH in 100 ml of water B dissolved 50g of NaOH in 100g of water while C dissolved 50g of NaOH in

  9. Chemistry

    A certain headache relief tablet is composed of monoprotic acetylsalicylic acid(C9H8O4(s)) and an inert filler. A 4.00 g tablet was crushed and dissolved to make 40.0 mL of solution. The solution was then titrated with 0.900 mol/L NaOH(aq). The volume of

  10. Chemistry

    Determine the molar mass of the unknown acid.? A 0.167-g sample of an unknown acid requires 27.8 mL of 0.100 M NaOH to titrate to the equivalence point. Elemental analysis of the acid gives the following percentages by mass: 40.00% C; 6.71% H; 53.29% O.

  11. chemistry

    Anthroquinone (C14H8O2), an important intermediate in the dye industry, is produced from the reaction of benzene with phthalic anhydride (C8H4O3), followed by dehydration with sulfuric acid. The overall reaction is... C8H4O3 + C6H6 --> C14H8O2 + H20 b)

  12. CHEMISTRY FOR DR. BOB or anyone else

    A hypothetical weak acid HA, was combined with NaOH in the following proportions: 0.20 mol HA, 0.08 mol NaOH. The mixture was then diluted to a total volume of 1L, and the pH measured. (a) If pH=4.80, what is the pKa of the acid (b) how many additional

  13. chemistry

    Which of the following mixtures will be a buffer when dissolved in a liter of water? a. 0.1 mol Ca(OH)2 and 0.3 mol HI b. 0.3 mol NaCl and 0.3 mol HCl c. 0.4 mol NH3 and 0.4 mol HCl d. 0.2 mol HBr and 0.1 mol NaOH e. 0.2 mol H3PO4 and 0.1 mol NaOH i think

  14. science

    C respectively to prepare a 50% (mass by volume) solution of sodium hydroxide (NaOH). 'A' dissolved 50 g of NaOH in 100 ml of water B dissolved 50g of NaOH in 100g of water while C dissolved 50g of NaOH in water to make 100ml of ...

  15. Chemistry

    An unknown solid acid is either citric acid or tartaric acid. To determine which acid you have, you titrate a sample of the solid with NaOH. The appropriate reactions are as follows: Citric acid: H3C6H5O7 (aq) + 3NaOH (aq) -> 3H2O (l) + Na3C6H5O7 (aq)

  16. For Dr.Bob222 (chem work)

    What is the pH of a solution of 120 ml 0.15M acetic acid to which we add 30mL 0.2M NaOH? CAN YOU CHECK MY WORK PLEASE? 0.15 mol/L * 0.12 L = 0.018 mol acetic acid 0.2 mol/L * 0.03 L = 0.006 mol NaOH 0.018 - 0.006 = 0.012 mol of acetic acid in excess pH =

  17. Chemistry

    A 0.2800 g sample of an unknown acid requires 28.22 ml of 0.1199 M NaOH for neutralization to a phenolphthalein end point. a.) How many moles of OH- are used? b.) How many moles of H+ are found in the acid? c.) What is the calculated equivalent molar mass

  18. Chemistry-Dr.Bob222

    A student completes a titration of an unknown diprotic acid. In this experiment, 0.79 g of the acid is dissolved in 250.0 mL of water. It requires 13.48 mL of 1.0 M NaOH to reach the second equivalence point. What is the molar mass of the acid?

  19. Chemistry

    A student completes a titration of an unknown diprotic acid. In this experiment, 0.79 g of the acid is dissolved in 250.0 mL of water. It requires 13.48 mL of 1.0 M NaOH to reach the second equivalence point. What is the molar mass of the acid?

  20. Dr Bob

    What is the pH of the solution that results from mixing 5 ml of 0.2 M NaOH and 100 mL of 0.05 M lactic acid? (Pka of lactic acid= 3.86) Responses Use the Henderson-Hasselbalch equation. The mixture you have indicated will react to form a buffer, the base

  21. Chem.

    To standardize a solution of NaOH, one uses a primary standard called potassium hydrogen phthalate (KHP). It is a monoprotic acid. It has a molar mass of 204.33g/mol. Suppose you weigh out .556g of KHP and dissolve it in water. It requires 14.48 mL of NaOH

  22. science

    the teacher instructed three students A,B,and C respectively to prepare a 50% (mass by volume) solution of sodium hydroxide (NaOH). 'A' dissolved 50 g of NaOH in 100 ml of water B dissolved 50g of NaOH in 100g of water while C dissolved 50g of NaOH in

  23. chemistry

    Titration was used to determine the molarity of acetic acid in vinegar. A primary standard solution of KHP was used to standardize the NaOH. 1. When performing this experiment, impure KHP was used to standardize the NaOH solution. If the impurity is

  24. Chemistry

    If you could help me it would be greatly appreciated, Thanx Question 1 In a titration, a 20mL sampl of NaOh(aq) was neutralized by 14.9 mL of 0.13 mol/L H2SO4(aq). The concentration of the base is A. 8.7 mol/L B. 0.35 mol/L C. 0.19 mol/L D. 0.048 mol/L

  25. chemistry

    A 125.0 mg sample of an unknown, monoprotic acid was dissolved in 100.0 mL of distilled water and titrated with a 0.050 M solution of NaOH. The pH of the solution was monitored throughout the titration, and the following data were collected. Determine the

  26. Chemistry

    Calculate the pH after 0.011 mol NaOH is added to 1.00 L of each of the four solutions. a) 0.100 M propanoic acid (HC3H5O2, Ka= 1.3 10-5) b) 0.100 M sodium propanoate (NaC3H5O2) c)pure H2O d) 0.100 M HC3H5O2 and 0.100 M NaC3H5O2

  27. Chemistry

    A 0.1873 g sample of a pure, solid acid, H2X was dissolved in water and titrated with 0.1052 M NaOH solution. The balanced equation for the neutralization reaction occurring is H2X(aq) + 2NaOH(aq) ¨ Na2X(aq) + 2H2O(l) If the molar mass of H2X is 85.00

  28. Chemistry

    1.In a titration, 50.0 mL of an acetic acid solution required 20.0 mL of a standard solution of 0.200 mol/L NaOH(aq). The concentration of the acetic acid solution is a. 0.08 mol/L. b. 0.50 mol/L. c. 0.05 mol/L. d. 1.0 mol/L. e. 0.30 mol/L. How do I solve

  29. Chemistry

    A sample of 1.018 g of KHP (potassium hydrogen phthalate, molar mass = 204.22 g/mol) was dissolved in ~ 25 mL distilled water and titrated with a NaOH solution of unknown concentration. If 28.69 mL of base was used to reach the endpoint, what was the

  30. Chemistry [sumone help me please :(]

    0.250g of phthalic acid is dissolved in 40.00cm^3 of 0.100 mol dm^-3 NaOH. It requires 11.80 cubic centimeters of 0.100 mol\dm^-3 HCL fo neutralisation( to phenolphthalein) The mole ratio in which phthalic acid reacts with sodium hydroxide ihn 1:2 (a)

  31. Chemistry urgent for my LAB today (22.09.11)

    0.250g of phthalic acid is dissolved in 40.00cm^3 of 0.100 mol dm^-3 NaOH. It requires 11.80 cubic centimeters of 0.100 mol\dm^-3 HCL fo neutralisation( to phenolphthalein) The mole ratio in which phthalic acid reacts with sodium hydroxide ihn 1:2 (a)

  32. Organic Chemistry

    A student purified a 3.88 g sample of phthalic acid by recrystallization from water. The published solubility of phthalic acid in 100 mL of water is 0.54 g at 14ºC and 18 g at 99ºC. What is the smallest volume (in milliliters) of boiling water the

  33. Chemistry

    A 0.2800 g sample of an unknown acid requires 28.22 mL of 0.1199 M NaOH for neutralization to a phenolphthalein point. a.) How many moles of OH- are used? b.) How many moles of H+ are found in the acid? c.) What is the calculated equivalent molar mass of

  34. Chemistry II

    A 12.00 mL sample of sulfuric acid from an automobile battery requires 34.62 mL of 2.42 M sodium hydroxide solution for complete neutralization. What is the molarity of the sulfuric acid? H2SO4 + 2NaOH ==> Na2SO4 + 2H2O molarity NaOH x liters NaOH = mols

  35. biology

    suppose 23mL of NaOH was required. How much Carbonic Acid was neutralized? 1L of .01 NaOH contains ____ mol NaOH? lmL of .01 NaOH contains _____mol NaOH? 23mL of .01 NaOH contains _____ mol NaOH? 2 mol of NaOH react with 1 mol H2CO3 2.3 x 10^-4 mol of NaOH

  36. CHEM

    Which of the following mixtures will result in the formation of a buffer solution when dissolved in 1.00 L of water? i) 0.50 mol NaOH and 0.50 mol HCl. ii) 0.50 mol NaCl and 0.25 mol HCl. iii) 0.50 mol NaF and 0.25 mol HF. iv) 0.50 mol NaOH and 0.25 mol

  37. General Chemistry

    Starting out with 50 mL of 0.20 M NaHCO3, calculate how many mL of 0.50 M NaOH solution to add to make 100 mL of approximately 0.10 M (total) buffer solution with a pH of 10.35. By adding NaOH, some of the NaHCO3 gets converted to the conjugate Na2CO3.

  38. organic chemistry

    How many milliliters of boiling water are required to dissolve 25 g of phthalic acid? If the solution were cooled to 14 degree Cellucius, how many grams of phthalic acid would recrystallize out?

  39. 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

  40. chemistry

    What mass of sodium hydroxide pellets must be poured into a waste drum containing 20.0 L o 3.0 mol/L sulphuric acid to completely neutralize the waste acid solution? Write a balanced chemical equation for this reaction. okay, so here is the work I already

  41. Chemistry

    A 0.355 g sample of a solid, monoprotic acid having a molar mass of 121 g/mol requires 18.47 mL NaOH for neutralization. Calculate the molarity of the NaOH solution. I got 0.159 M NaOH

  42. 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

  43. Chemistry

    1. A good indicator will have a(n)____ close to this volume and pH. I think it's endpoint but it's wrong. 2. (part a) What is the pH of the solution created by combining 1.70 mL of the 0.10 M NaOH(aq) with 8.00 mL of the 0.10 M HCl(aq)? with 8.00 mL of the

  44. chemistry

    In a titration, 3.4 g of an acid (HX) requires 21.5 mL of 0.85 M NaOH(aq) for complete reaction. What is the molar mass of the acid? Answer in units of g/mol. im not really sure how to even start... but i calculated the moles of NaOH which i got to be .018

  45. Chemistry

    A solid weak acid is weighed, dissolved in water and diluted to exactly 50.00 ml. 25.00 ml of the solution is taken out and is titrated to a neutral endpoint with 0.10 M NaOH. The titrated portion is then mixed with the remaining untitrated portion and the

  46. Chemistry

    When we mix NaOH and H2SO4 we get the equation OH-(aq) + H+(aq) --> H2O(l) and if we mix H2CO3 and NaOH we get the equation 2OH-(aq) + H2CO3 --> 2H2O(l) + CO3-2(aq) Why aren't the two equations the same? ie only one mol of NaOH reacts in the first equation

  47. Chemistry

    An organic acid has a percentage composition by mass of C 41.4%, H 3.4%, and O 55.2%. A solution containing 0.250g of the acid, which is dibasic required 26.60 cm cubed of NaOH solution (0.20 mol.dm -3) for neutralisation. Calculate the empirical formula,

  48. chemistry

    A 43 mL sample of a solution of sulfuric acid is neutralized by 24 mL of a 0.053 M sodium hydroxide solution. Calculate the molarity of the sulfuric acid solution. Answer in units of mol/L. Here is my work so far. I thought I have successfully solved the

  49. Chem

    A sample contains an unknown amount of tartaric acid, H2C4H4O6. If 0.3888 g of the sample requires 37.74 mL of 0.1000 M NaOH to neutralize the H2C4H4O6 completely, what is the percentage of H2C4H4O6 in the sample? The molar mass of H2C4H4O6 is 150.09

  50. CHEMISTRY

    .4g sample of monobasic acid requires 16cm3 of .1 mol dm 3 of NAOH for complete neutralization what is relative mass of acid

  51. chemistry

    In a titration, 4.1 g of an acid (HX) requires 32.8 mL of 0.74 M NaOH(aq) for complete reaction. What is the molar mass of the acid? Answer in units of g/mol.

  52. chemistry 101

    If 15g of NaOh is dissolved in 285 g of water, calculate the following. Assume the density of the solution is 1.06 g/cc. a) Calculate the moles of NaOH in the solution? My answer is 15gNaOH/40g NaOH= .0375 mole NaOH b) Waht is the mass % w/w of the

  53. CHEMISTY

    A 25.0 mL sample of perchloric acid solution required 45.3 mL of 0.101 sodium hydroxide solution for complete neutralization. what was the concentration of the perchloric acide solution? work: 0.0453 L NaOH x ( .101 mol NaOH/ 1L NaOH) x (1 mol HClO4/ 1 mol

  54. chem lab (webwork)

    What is the pH of the solution created by combining 1.80 mL of the 0.10 M NaOH(aq) with 8.00 mL of the 0.10 M HCl(aq)? with 8.00 mL of the 0.10 M HC2H3O2(aq)? mL NaOH pH wHCl pH wHC2H3O2 1.80 Complete the table below: What are the pH values if you take

  55. chemistry

    A 2.5 g sample of NaOH (Mw = 40.00) was dissolved in water to give a solution of final volume 250 cm3. (i) With reasons, state whether NaOH is a strong or a weak base. Give the conjugate acid of NaOH and decide whether this conjugate acid is acid, alkaline

  56. chemistry first yera

    A 0.4 g sample of monobasic acid requires 16cm3 of 0.1 mol per dm3 of NaOH for complete neutralization . what is the relative mass of the acid?? Plz ans me urgent

  57. Chemistry

    3) 0.3382 g of an unknown diprotic acid, when dissolved in water, required 32.34 mL of 0.1046 M KOH to reach the endpoint. Calculate the molar mass of the unknown acid. Also, for this problem I keept getting 99 close to 100 g/mol, but the answer has to be

  58. chemistry

    0.1276 of a monoprotic acid (molar mass 110g/mol) was dissolved in 25ml of water.The pH of the solution was found to be 5.87 after the addition of 10.0ml of 0.0633 M NaOH.The Ka of acid is.......................

  59. Chemistry(Please check)

    Which of the following mixtures will be a buffer when dissolved in 1 liter of water? 0.10 mol Ba(OH)2 and 0.20 mol HCl 0.30 mol KCl and 0.30 mol HCl 0.40 mol NH3 and 0.40 mol HCl 0.20 mol HNO2 and 0.10 mol NaOH 0.20 mol HBr and 0.10 mol KOH My answer is

  60. ENGINEERING

    a vinegar contains acetic acid,CH3COOH.Titration of 5.00g of vinegar with 0.100M of NAOH requires 33.00cm to reach the equivalence point.a)what is the weight percentage of CH3COOH in vinegar?

  61. 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

  62. 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

  63. Chem

    You are titrating an unknown weak acid you hope to identify. Your titrant is a 0.0935 mol/L NaOH solution, and the titration requires 22.3 mL to reach the equivalence point. How many moles of acid were in your sample?

  64. chemistry

    You are titrating an unknown weak acid you hope to identify. Your titrant is a 0.0935 mol/L NaOH solution, and the titration requires 39.9 mL to reach the equivalence point. How many moles of acid were in your sample?

  65. Chemistry

    what is the resultig pH if 0.005 mol of NaOH is added to 100.0mL of buffer containing 0.010 mol acetic acid (CH3COOH,pKa = 4.74)and 0.010 mol sodium acetate (NaCH3COO)? (Assume the final volume is 100 mL) So i worked it out, i just need to double check the

  66. 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?

  67. Chem

    25.0 mL of 0.100 M acetic acid (Ka= 1.8 x 10^-5) is titrated with 0.100 M NaOH. Calculate the pH after the addtion of 27.00 mL of 0.100M NaOH. my work CH3COOH + H2O H3O^+ + CH3COO^- 25mL x 0.100 mmol/ml = 2.5mmol CH3COOH 27mL x 0.100 mmol/ml = 2.7mmol NaOH

  68. chemistry

    A chemist wishes to prepare 250mL of a buffer that is pH = 4.50. Beginning with 100mL of 0.12 mol L^(-1) acetic acid and a supply of 0.10 mol L^(-1) NaOH, explain how this could be done. How much 0.20 mol L^(-1) NaOH must be added to this buffer to raise

  69. chemistry

    530 mL solution 10% HCl has been spilt onto the bench. It cannot be diluted or washed away. How much of the granular NaOH from the container seen in a must be used to neutralise the acid? [Using NaOH: MM = 40 g/mol] 1. I have NaOH + HCl --> NaCl + H2O. 10%

  70. 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

  71. chemistry

    hi, I am trying to find the solubility of Sodium Acetate by using 0.100 mol Hydroxide(base) and 0.837 mol acetic acid( vinegar). The theoretical solubility of sodium acetate is 82.3g/100ml at 25C. Doing calculations we would want NAOH concentration of

  72. Chemistry

    A .682 g sample of an unknown weak monoprotic acid, HA, was dissolved in sufficient water to make 50mL of solution and was titrated with a .135 M NaOH solution. After the addition of 10.6mL of base, a pH of 5.65 was recorded. The equivalence point was

  73. Chemistry

    Find the Molecular weight of unknown acid #5... Mass of acid #5 = 1.200g Volume (acid was mixed in) = 100ml (distilled water) Conectration of NaOH = 0.989 M Aliquot of acid titrated with NaOH = 25ml = 0.025 L Average volume of NaOH from titration = 9.3ml =

  74. chemistry

    if the pH of a half-neutralized acid solution is 5.4, how would you find the [H+] of the the solution. There is 1.0 g of L-ascorbic acid which was dissolved in 100 ml of water. That solution was split in two and 50 ml of the solution was titrated with 0.2

  75. CHEM HELP! (Check work)

    H3CA is a vitally important intemediate in the metabolism of carbohydrates. The compound is widely distributed in plant and animal tissues and fluids. H3CA is a tiprotric acid, ie, it requires three moles of NaOH to fully neutralize one mole of H3CA. a.)

  76. Chemistry

    Consider a weak acid-strong base titration in which 25.0 mL of 0.100 M acetic acid is titrated with 0.100 M NaOH. a) Calculate the pH after the addition of 3.00mL of NaOH. b) What is the pH of the solution before the addition of NaOH (pKa of acetic

  77. Chemistry

    In this experiment NaOH is standardized to find out the percent by mass of the acetic acid in a sample of vinegar. A student had not allowed the NaOH pellets to dissolve completely before standardizing it with KHP, but when the student refilled the buret

  78. Chemistry

    How many milimetres of 0.114 M sulphuric acid solution provide the sulfuric acid required to react with the sodium hydroxide in 32.3 ml of 0.122 M NaOH according to the following equation? H2SO4 + 2 NAOH ---> Na2SO4 + 2 H20 A millimeter is a unit of

  79. Chemistry

    The titration of a 50.0 mL solution of the monoprotic bromoacetic acid (pKa = 3) takes 10 ml of 0.01 mol L-1 NaOH to reach the stoichiometric point. What was the initial concentration of bromoacetic acid? A) 0.02 mol/L B) 0.01 mol/L C) 0.002 mol/L D) 0.001

  80. Inorganic chemistry

    mol KHP = (0.7719g)(1 mol KHP/204.2g) = .0038mol Where are the moles of NaOH? I know that there are 0.02637 L of NaOH and I know M = mol/l I know there are 40g NaOH/mol NaOH There is 1 mol of NaOH in the balanced equation But I do not have grams of NaOH

  81. Chemistry

    Determine the molar mass of the unknown acid.? A 0.167-g sample of an unknown acid requires 27.8 mL of 0.100 M NaOH to titrate to the equivalence point. Elemental analysis of the acid gives the following percentages by mass: 40.00% C; 6.71% H; 53.29% O.

  82. Chemistry

    Thanks for your help; I am still have a few problems, could you check my work: Given: Volume of vinegar analyzed-5mL Con'c of NaOH-0.09890M Avg. Volume of NaOH from titration-43.75mL Density CH3COOH: 1.049g/mL Calculations: 1.Moles of NaOH required to

  83. ap chemistry

    A 0.456 gram sample of an unknown mono- protic acid (let’s call it HZ) was dissolved in some water (you pick the amount). Then the acidic solution was titrated to the equivalence point with 32.5 mL of 0.174 M KOH. What is the molecular weight of the

  84. CHEMISTRY FOR DR. BOB or anyone else

    A hypothetical weak acid HA, was combined with NaOH in the following proportions: 0.20 mol HA, 0.08 mol NaOH. The mixture was then diluted to a total volume of 1L, and the pH measured. (a) If pH=4.80, what is the pKa of the acid (b) how many additional

  85. Science

    25 cm of 1.0 mol dm− NaOH is added to 25 cm of 1.0 mol dm− HCl. The temperature rise is 6¢XC. Which reactants will also give a temperature rise of 6¢XC? A. 25 cm of 2.0 mol dm− NaOH and 25 cm of 2.0 mol dm− HCl. B. 50 cm of 1.0 mol dm− NaOH and

  86. Chemistry

    Greetings: I was wondering how to calculate the weight/volume % of vinegar using the formula ---------------w/v Per Cent = g/100 mL or grams per deciliter: WHAT WEIGHT DO I USE NaOH, Acetic ACID? the data include: volume of NaOH needed to neutralize

  87. chemistry

    hi, I am trying to find the solubility of Sodium Acetate by using 0.100 mol Hydroxide(base) and 0.837 mol acetic acid( vinegar). The theoretical solubility of sodium acetate is 82.3g/100ml at 25C. Doing calculations we would want NAOH concentration of

  88. Chemistry

    Hi,may I have your help? I have posted a titration question that I'm trying to solve. The correct answer to the problem is 0.128 M, however,I have arrived at the answer: 0.000128 M. Here's the question: If 38.30 mL of 0.250 M NaOH is used to titrate 25.0

  89. Chemistry

    I'm trying to find the solubility of Ca(OH)2 in .0125 mol/L aqueous NaOH. Here is my data: Vol of solution used per titration: 20mL Conc of HCl: .1201 mol/L Average Titre: 4.71 I need to calculte: 1. the TOTAL [OH-] in the saturated solution of Ca(OH)2 in

  90. Chemistry

    1)A solution prepared by adding 0.400 mol of acetic acid (pKa = 4.74) and 0.400 mol of sodium acetate to 100.0 mL of water. The pH of this buffer solution is initially 4.74. Predict the final pH when 55.0 mL of 1.10 M NaOH is added to solution 2) A

  91. chemistry

    1. When performing this experiment, a student mistakenly used impure KHP to standardize the NaOH solution. If the impurity is neither acidic nor basic, will the percent by mass of acetic acid in the vinegar solution determined by the student be too high or

  92. Chem

    What is the pH of the resulting solution if 30.00 mL of 0.100M acetic acid is added to 10.00mL of 0.100 M NaOH? For acetic acid, Ka=0.000018. I know that NaOH is a strong base and acetic acid is a weak acid. What is the equation: C6H5COOH+NaOH C6H5COOH

  93. chemistry

    So I did a titration lab at school with NaOH and HCl. i have to find: - volume used, NaOH - Moles of NaOH - Moles of HCl -Volume used unknown HCl - Molarity of HCl solution My concentration of NaOH stock solution was 0.100 mol/lL Final buret reading, NaOH:

  94. Chemistry

    1)A solution prepared by adding 0.400 mol of acetic acid (pKa = 4.74) and 0.400 mol of sodium acetate to 100.0 mL of water. The pH of this buffer solution is initially 4.74. Predict the final pH when 55.0 mL of 1.10 M NaOH is added to solution 2) A

  95. Chemistry

    A BS Medical Technology student was asked to determine the molecular weight of a diprotic acid using acid-base titration. This student performed four trials. Firstly, the student used potassium hydrogen phthalate (KHP, 204.22 g/mol) as standard to

  96. Chemistry

    If 0.250 moles of NaOH are dissolved in 125g of water, what is the %m/m of NaOH in this solution? I converted 0.250 mol to 10.0 g. Then using the equation mass solute/mass solution * 100 I came up with the final answer of 7.41 %m/m. Is that correct?

  97. Chemistry

    Please help! I'm trying to find the solubility of Ca(OH)2 in .001305 mol/L aqueous NaOH? Saturated solution of Ca(OH)2 in 0.01305 mol/L NaOH. [HCl] = 0.1213 M Volume of HCl = 9.81 mL Volume of Ca(OH)2/NaOH aliquot = 25ml Find: 1. the TOTAL [OH-] in the

  98. Chemistry

    SOMEBODY PLEASE HELP ME! This is my last question for the chemistry and thank you. :D A BS Medical Technology student was asked to determine the molecular weight of a diprotic acid using acid-base titration. This student performed four trials. Firstly, the

  99. 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

  100. Chemistry

    1.) It takes 2.085x10^1 mL of 1.30x10^-1 M NaOH to titrate 2.9660x10^-1 grams of solid monoprotic acid (HX). What is the molar mass of this acid. Express in scientific not. w/ 3 sig figs. Here is my work, but I'm not sure if it's right. Please check.

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