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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 2drops

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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 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
  5. 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
  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 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
  8. 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)
  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, 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
  12. 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
  13. 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
  14. 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
  15. 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
  16. 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
  17. 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
  18. chemistry

    35.0 mL of an aqueous solution of HNO3 of unknown concentration is titrated with a standard solution made up of 0.453 m NaOH
  19. 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
  20. Chemistry

    I really need help with this question. If 2 trials using 10.0 mL of a solution with an unknown concentration were titrated using close to 20mL of a standard solution each trial, what approximate volume of the standard solution would be needed to titrate
  21. Chemistry

    Consider a solution containing 4.35 mM of an analyte, X, and 1.09 mM of a standard, S. Upon chromatographic separation of the solution peak areas for X and S are 3251 and 10075, respectively. Determine the response factor for X relative to S. F=? To
  22. chemistry

    When the glucose solution described in part A is connected to an unknown solution via a semipermeable membrane, the unknown solution level rises. Based on this information, what can be said about these two solutions? a.) The unknown solution had the lower
  23. chemistry

    When the glucose solution described in part A is connected to an unknown solution via a semipermeable membrane, the unknown solution level rises. Based on this information, what can be said about these two solutions? a.) The unknown solution had the lower
  24. chemistry

    A is a solution containing 5.00 g of HNO3 in 500 cm\(^3) of solution. B is a solution of NaOH of unknown concentration. 21.30cm3 of A was titrate it with 25.0 cm3 portions of B using methyl orange as an indicator. calculate the: (i) concentration ot A In
  25. 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
  26. 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.
  27. 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)
  28. Chemistry

    A 0.110-L sample of an unknown HNO3 solution required 52.1 mL of 0.150 M Ba(OH)2 for complete neutralization. What was the concentration of the HNO3 solution?
  29. chemistry

    A 0.115-L sample of an unknown HNO3 solution required 31.1 mL of 0.100 M Ba(OH)2 for complete neutralization. What was the concentration of the HNO3 solution?
  30. Chemistry

    In a titration experiment, 15.0 mL of 0.10 M Ba(OH)2 is required to titrate a 10.0 mL of an unknown solution of HNO3. Calculate the concentration of the HNO3 solution using the data. 2HNO3 + Ba(OH)2 ® Ba(NO3)2 + 2H2O
  31. 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
  32. 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.
  33. Chemistry

    An aqueous solution of an unknown solute is tested with litmus paper and found to be acidic. The solution is weakly conducting compared with a solution of NaCl of the same concentration. Which of the following substances could the unknown be: KOH,NH3,HNO3,
  34. science

    solution A was prepared by dissolving 0.63g of HNO3 in 100cm3 solution. Solution B is a sodium calcium hydroxide solution of unknown concentration. state a balanced chemical equation for the reaction
  35. 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
  36. 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) %
  37. 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);
  38. 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)
  39. 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
  40. 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
  41. 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?
  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

    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
  44. 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
  45. college chemistry

    Suppose you have a 0.200 M solution of the nitrogen-containing weak base NX. Suppose you wish to titrate 25 mL of this 0.200 M NX solution with a 0.100 M solution of the strong acid HNO3. Given that the Kb value of NX is 6.50x10-5, complete each of the
  46. 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?
  47. 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
  48. Chemistry, #4

    Calculate the concentration of an aqueous HNO3 solution that has a pH=5.08. pH = 5.08. Convert that to (H^+). Since HNO3 is a strong acid and it is 100% ionized, (H^+) = (HNO3).
  49. chemistry

    A chemist added 3.15 grams of HNO3 to a solution of the same acid with concentration of 9 mol/L. dilutes the resulting solution up to the 100ml volume. The resulting solution will have what concentration?
  50. 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?
  51. Chemistry

    A is a solution of HNo3 of unknown concentration while is a solution of sodium hydroxide containing 4.00 g/dmcube of solution 5.00cm cube of B using methyl orange as an indicator.from the result and information provide above write a balanced equation for
  52. AP Chemistry

    A 5.0 M solution of HNO3 is titrated with 0.3 M NaOH. Identify the species that have the highest concenttrations in the solution being titrated halfway to the equivalence point. A 25.15 ml of 0.35 m HNO3 was titrated with an unknown concentration of NaOH.
  53. Chemistry

    How would each of the following affect the Cr(VI) concentration determined in this experiment? Justify the answers with an explanation. In the experiment, absorption spectroscopy was used to obtain the concentration of Cr(VI) ions. 1) A student adds more
  54. Chemistry: Check my answers please!

    How would each of the following affect the Cr(VI) concentration determined in this experiment? Justify the answers with an explanation. In the experiment, absorption spectroscopy was used to obtain the concentration of Cr(VI) ions. 1) A student adds more
  55. 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
  56. 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 +
  57. 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.
  58. 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
  59. analytical chemistry

    DrBob222, it is me again. Continue the question 5mL of a solution A (unknown concentration) was transferred into sic 25mL volumetric flask. The following volumes of a standard solution of A with with a concentration 75ppm were added to the flask: 0mL,
  60. 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
  61. 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
  62. 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?
  63. 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?
  64. Chemistry

    The densities of three solutions with known concentrations ( 20% , 50%, and 70%), and one unknown solution were determined. If the densities of 20%, 50% and 70% solutions are 0.69 and 0.58 and 0.49 g/mL, respectively, and the denisty of the unknown
  65. analytical chemistry

    Any help is greatly appreciated 5mL of a solution A (unknown concentration) was transferred into sic 25mL volumetric flask. The following volumes of a standard solution of A with with a concentration 75ppm were added to the flask: 0mL, 0.5mL, 1mL, 1.5mL,
  66. 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
  67. science chemistry

    Brandon prepares a potassium hydroxide solution (KOH) that he uses during a titration to determine the unknown concentration of a hydrochloric acid solution calculate the mass of potassium hydroxide that is need to prepare 250 cm^3 of a standard 0,125
  68. 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
  69. Chemistry

    Cadmium and a solution of cadmium(II) nitrate are used with tin and a solution of tin(II) nitrate to construct a galvanic cell. 1) The reaction run initially at standard state with 100-mL samples of each solution is allowed to proceed until 8.0 g of tin
  70. Chemistry.

    hi again, thanks to the previous help i got the first part of the question. the second part builds on the first part as we used that stock solution for titration of the next. we are now given: Concentration of Standard Acid Soultion (M) = 0.100 M Volume of
  71. Chemistry

    a potassium dichromate is prepared by 0.3525grams of K2Cr2O7 is enough water to yield 250.0mL of solution. a student then measures 10.00mL of an unknown solution of Fe2+ into an erlenmeyer flask and dilutes with 90mL of 1.0M hydrochloric acid. she then
  72. 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
  73. 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
  74. chemistry

    The densities of three solutions with known concentrations ( 20% , 50%, and 70%), and one unknown solution were determined. If the densities of 20%, 50% and 70% solutions are 0.69 and 0.58 and 0.49 g/mL, respectively, and the denisty of the unknown
  75. Chemistry

    A standard solution with a FeSCN2+ concentration of 1.55x10^-4M has a percent transmittance (%T) of 18.8%. Another solution of unknown FeSCN2+ concentration has a percent transmittance of 44.8%. A) Calculate the absorbance (A) of each solution. B) Using
  76. Please help with Chemistry?????

    A standard solution with a FeSCN2+ concentration of 1.55x10^-4M has a percent transmittance (%T) of 18.8%. Another solution of unknown FeSCN2+ concentration has a percent transmittance of 44.8%. A) Calculate the absorbance (A) of each solution. B) Using
  77. Nuhu Bamali Poly zaria Nig

    Chemistry volumetric analysis. B is a solution of Na2CO3 containing 5g/dm3. A is a solution of oxalic acid of uknown concentration 25cm3 of 25.25,25.0 and 24.80 respectively (I) Calculate the average volume of acid used (II) The molar concentration of
  78. AP CHEM

    Please help me with thses AP CHEM homework problems and show the steps to how to find the solutions: Solid Liquid Titrations: Determine the concentration of the indicated liquid unknown given the mass of a solid standard and the buret data for the
  79. 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)
  80. Chemistry

    During a titration experiment, a 150.0 mL solution of 0.05 M sulfuric acid (H2SO4) is neutralized by 300.0 mL solution with an unknown concentration of sodium hydroxide (NaOH). What is the concentration of the sodium hydroxide solution? The answer I got
  81. Chemistry

    During a titration experiment, a 150.0 mL solution of 0.05 M sulfuric acid (H2SO4) is neutralized by 300.0 mL solution with an unknown concentration of sodium hydroxide (NaOH). What is the concentration of the sodium hydroxide solution?
  82. Chemistry

    What effect on the molar mass of the unknown acid would each of the following have-that is-would it make the calculated molar mass high, low, or would it have no effect? 1. Adding 5 drops of phenolphthalein instead of 1 drop. 2. Using a standard NaOH
  83. Analytical Chemistry

    5mL of a solution A (unknown concentration) was transferred into sic 25mL volumetric flask. The following volumes of a standard solution of A with with a concentration 75ppm were added to the flask: 0mL, 0.5mL, 1mL, 1.5mL, 2mL, and 2.5L. The excitation
  84. CHEMISTRY PLEASE HELP

    Cobalt was used as an internal standard to analyze a sample of titanium with atomic absorption spectroscopy. A mixture was prepared by combining a 4.00 mL Ti solution of unknown concentration with 3.00 mL of a 11.7 micrograms/mL solution of Co. The atomic
  85. CHEMISTRY

    Cobalt was used as an internal standard to analyze a sample of titanium with atomic absorption spectroscopy. A mixture was prepared by combining a 4.00 mL Ti solution of unknown concentration with 3.00 mL of a 11.7 micrograms/mL solution of Co. The atomic
  86. Chemistry

    Cobalt was used as an internal standard to analyze a sample of titanium with atomic absorption spectroscopy. A mixture was prepared by combining a 4.00 mL Ti solution of unknown concentration with 3.00 mL of a 11.7 micrograms/mL solution of Co. The atomic
  87. chemistry

    in HNO3 titration, you add few drops of phenolphthalein indicator to 50.0 mL of acid in a flask. you quickly add 20.00 mL of 0.0547 M NaOH but overshoot the end point, and the solutions turn deep pink. instead of starting over, you add 30.00 mL of acid,
  88. 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.
  89. chemistry

    10.0 mL of a Cu2+ solution of unknown concentration was placed in a 250 mL Erlenmeyer flask. An excess of KI solution was added. Indicator was added and the solution was diluted with H2O to a total volume of 75 mL. The solution was titrated with 0.20 M
  90. Chemistry

    A solution of trioxonitrate v contains 0•67g in 100cm^3. 31•00cm^3 of this solution neutralize 25cm^3 of Na2CO3 solution. Calculate the concentration of the Na2CO3 solution.
  91. 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
  92. chemistry

    A 30 ml sample of unknown strong base is neutralized after the addition of 12 ml of a 0.150 M HNO3 solution if the unknown base concentration is 0.0300 M give some possible identities for the unknown base
  93. chemistry

    30 ml of sample of unknown strong base is neutralized after the addition of 12 ml of a 0.150 M HNO3 solution if the unknown base concentration 0.0300 M give the possible identities for the unknown base
  94. Chemistry

    If you dilute 14.0mL of the stock solution to a final volume of 0.350L , what will be the concentration of the diluted solution? Before it, there was a question: How many milliliters of a stock solution of 5.60 M HNO3 would you have to use to prepare
  95. chemistry

    X is a solution,of dibasic of H2X. G is a solution containing 1.00g of NaOH in 250cm3 of solution . 24.60cm3 of solution F required 25.00cm3 of solution G . From your result and information provided above. (I)concentration of G in mol/dm3 (ii)
  96. 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
  97. 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
  98. chemistry

    if 10 ml of a 2M standard solution is used to neutralize 20mL of an unknown base what is the molarity of the unknown and is this standard solution an acid or base?
  99. chemistry

    A bottle of commercial hydrochloric acid solution So is labeled 37% composition by mass, density 1.19 kg/L. Calculate the concentration of solution So. 4.2 ml of So are diluted to 500ml solution called S. We titrate S with 200 ml of KOH solution of
  100. chemistry

    The concentration of HNO3 in a solution is 3.50 10-6 M. What is the [H3O+] in the solution? _______M What is the [OH-] in the solution? ________ M What is the pH of the solution? What is the pOH of the solution?

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