1. Chemistry

    Calculate the pH of the the solution that results from titrating 50 mL of 0.6 M NaOCl(aq) with 0.3 M HBr At 0.00 mL of HBr: At 70 mL of HBr: At 100 mL HBr: At 120 mL of HBr
  2. Chemistry

    Let’s assume you have 250 ml of a 1.3M KOH solution and you want to neutralize it with the acid HBr. It takes 350 ml of the HBr solution to do so. What must have been the molarity of the HBr solution? HBr(aq) + KOH(aq) => KBr(aq) + H2O(l) The
  3. Chemistry

    A 38.5 mL sample of HBr is titrated with 112 mL of 1.05 mol/L KOH. The density of the HBr solution is 1.75 g/mL. Calculate the percentage by mass of the HBr in the sample. How come we don't use density*volume to find the moles of HBr?
  4. Chemistry

    1. Calculate the pH for each of the following cases in the titration of 25.0 mL of 0.240 M pyridine, C5H5N(aq) with 0.240 M HBr(aq): (a) before addition of any HBr (b) after addition of 12.5 mL of HBr (c) after addition of 22.0 mL of HBr (d) after addition
  5. chemistry

    If 17.5 mL of 0.553 M KOH is needed to neutralize 25.0 mL of an HBr solution what is the molarity od HBr solution
  6. Chemistry

    A 16.6 mL portion of an HBr solution of unknown strength is diluted to exactly 247 mL. If 102.1 mL of this diluted solution requires 87.8 mL of 0.37 M NaOH to achieve complete neutralization, what was the strength of the original HBr solution?
  7. chemistry

    A 20.00 ml stock sample of HBr is diluted to 50 mL. If 18.76 ml of 0.1345 M KOH was required to reach the equivalence point, what is the concentration of the stock HBr solution? Is my answer correct? Titration problems can be solved with the MV=MV
  8. Chemistry

    If a chemist has a stock solution of HBr that is 10.0 M and would like to make 450.0 mL of 3.0 M HBr, how would he or she do it?
  9. Chemistry

    What volume of 14.1M HBr is required to make 250mL of 1.25M HBr solution by dilution with water?
  10. chemistry

    what volume of a 0.272 M solution of HBr is needed for a reaction that requires 49.5 g of HBr? Answer in units of L.
  11. chemistry

    Calculate the pH for each of the following cases in the titration of 25.0 mL of 0.180 M pyridine, C5H5N(aq) with 0.180 M HBr(aq): 1)before addition of any HBr 2)after addition of 12.5 ml of HBr: 3)after addition of 16 ml of HBr: 4)after addition of 25 ml
  12. Chemistry

    A 100.0mL solution containing aqueous HCl and HBr was titrated with 0.1290M NaOH. The volume of base required to neutralize the acid was 47.56mL. Aqueous AgNO3 was then added to precipitate the Cl- and Br- ions as AgCl and AgBr. The mass of the silver
  13. Chemistry

    According to the balanced equation below, how many moles of KBr will be made from 30.0 mL of 1.00 M HBr solution? HBr(aq) + KOH(aq) --> H2O(I) + KBr(aq)
  14. Chemistry

    The heat evolved in the reaction of hydrobromic acid with potassium hydroxide was determined using a coffee coup calorimeter. The equation for the reaction is: HBr(aq) + KOH(aq) -------------> KBr(aq) + H2O(l) When 25.0 mL of 1.00 M HBr at a temperature
  15. Chem-E / Chemistry

    Calculate the rate of heat required to bring 1.80mol/hr of HBr gas from 37.0 C to 434.0C at atmospheric pressure (Heat capacity of HBr is described by eq.) Cp (kJ/mol * C) = a + bT + cT^2 + dt^3 T is in C and HBr - a = 2.910x10^-2, b= -2.27x10^-7, c=
  16. chemistry

    the equilibrium constant for the synthesis of HBr(g0 from hydrogen and bromine gas is 2.18*10 exponent 6 at 730 degrees celcius.if 3.75 mol of HBr(g) is put into a 15L reaction vessel,calculate the concentration of H2,Br2 and HBr at equilibrium
  17. CHEMISTRY

    The heat evolved in the reaction of hydrobromic acid with potassium hydroxide was determined using a coffee coup calorimeter. The equation for the reaction is: HBr(aq) + KOH(aq) -------------> KBr(aq) + H2O(l) When 25.0 mL of 1.00 M HBr at a temperature
  18. Chemistry

    A sample of solid Ca(OH)2 is stirred in water at 30°C until the solution contains as much dissolved Ca(OH)2 as it can hold. A 100.-mL sample of this solution is withdrawn and titrated with 5.00 X 10^-2 M HBr. It requires 48.8 mL of the acid solution for
  19. Chemistry

    In a .57 M solution of HOC6H5, .0684% of the acid has been dissociated. a) find the concentrations of all aqueous species in the solution at equilibrium b) find the pH of the solution c) What concentration of HBr would produce a solution with the same pH
  20. chemistry

    A 50.0 mL sample of 0.50 M HBr is titrated with 0.25 M KOH. What is the pH after the addition of 60.0 mL of KOH? A) 4.1 B) 13.4 C) 1.7 D) 2.0 E) 7.7 I'm confused on the process of solving this problem. My work so far: .050L X .50 mol/1L= .025 mol HBR .060L
  21. Chemistry

    Assuming equal concentrations , rank these solutions by pH. RbOH(aq), NH3(aq), HF(aq) HBr(aq), Ca(OH)2(aq). I know the most acidic solution has the lowest pH and the most basic solution has the highest pH. But how am i supposed to know the pH if i don't
  22. Chemistry

    For the following reaction, Kp = 3.5 104 at 1495 K. H2(g) + Br2(g) 2 HBr(g) What is the value of Kp for the following reactions at 1495 K? (a) HBr(g) 1/2 H2(g) + 1/2 Br2(g) (b) 2 HBr(g) H2(g) + Br2(g) (c) 1/2 H2(g) + 1/2 Br2(g) HBr(g)
  23. Chemistry

    1. Hydrogen bromide(HBr) is a strong, highly corrosive acid and what is the pOH of a 0.0375M HBr solution? a)12.57 b)12.27 c)1.73 d)1.43 I can't fogure out what the answer should be as I don't know whether 0.0375M is the [H^+] or [OH^-] If 0.0375M is the
  24. Chemistry

    56mL of a stock solution of hydrobromic acid, HBr, is added to 85mL of water, yielding a solution having a pH of 1.0. What was the molarity of the stock solution? I know Molarity = moles of solute/ liters of solution
  25. CHEMISTRY

    2HBr+Mg(OH)2 -> MgBr2+2H2O how many mL of a 0.2 M HBr solution is required to react with 40 mL of a 0.40 M Mg(OH)2 solution
  26. chemistry

    need help figure out how to do these problem: 1)Calculate the pH of this solution: 1.55 X 10^-2 M HBr 2)Determine the pH of this solution: pOH = 8.3 thanks
  27. General Chemistry

    find [H3O+] and [OH-] 1)a solution that is 5.8×10−2 M in [HBr] and 1.9×10−2M in [NO3]. 2)a solution that is 0.780% HNO3 by mass (Assume a density of 1.01 g/mL for the solution.)
  28. Chemistry

    A 635 mL solution of HBr is titrated with 0.51 M KOH. If it takes 1569 mL of the base solution to reach the equivalence point, what is the pH when only 141 mL of the base has been added to the solution?
  29. Chemistry

    A 635 mL solution of HBr is titrated with 0.51 M KOH. If it takes 1569 mL of the base solution to reach the equivalence point, what is the pH when only 141 mL of the base has been added to the solution?
  30. Chemistry

    Find the pH: 1) A 0.001M solution of HCl 2) A 7.98 x 10^-2 M solution of HNO3 3) 1098L of a solution containing 8.543moles of HBr 4) 120mL of a solution containing 0.005 grams of hydrochloric acid. Please help me with these four. Out of 20 questions i only
  31. chemistry

    A 0.10-mol sample of H2(g) and a 0.10-mol sample of Br2(g) are placed in a 2.0-L container. The reaction H2(g) + Br2(g) <----> 2 HBr(g) is then allowed to come to equilibrium. A 0.20 mol sample of HBr is placed into a second 2.0-L sealed container at
  32. 9th grade science

    A strong acid, HBr, has been dissolved into a beaker of water. If the solution is known to be 0.000 001 M, what is the pH solution?
  33. CHEM 1411

    What volume (in mL) OF 0.0215M HBr solution is be required to titrate 0.235L of a 0.0150M Ca(OH)2 solution? Ca(OH)2+2HBr= CaBr2+2H2O
  34. chemistry

    A chemist has 12.0 M HBr and would like to use it to make 500.0 mL of 3.5 M HBr. describe how she should do this
  35. Chemistry

    A 26.8 mL sample of a solution of RbOH is neutralized by 15.71 mL of a 1.918 M solution of HBr. What is the molarity of the RbOH solution?
  36. Science

    A student wants to neutralize 1000 ml of .25m lioh with 0.75m hbr. How much hbr are they expected to use? Sho your work.
  37. chemistry

    for haloacetic acids, HBr has higher stronger acid strength then HF but doesnt HBr has low dipole then
  38. chemistry

    Part A 6.00×10−3 mol of HBr are dissolved in water to make 16.0L of solution. What is the concentration of hydroxide ions,[OH-], in this solution? Express your answer with the appropriate units.
  39. chemistry help asap

    Please check these thanks. 1. In a titration, 33.21 mL 0.3020M rubidium hydroxide solution is required to exactly neutralize 20.00 mL hydrofluroic acid solution. What is the molarity of the hydrofluroic acid solution? Answer: 0.502HF 2. A 35.00 mL-sample
  40. Chemistry

    Determine the entropy change when 1.80 mol of HBr(g) condenses at atmospheric pressure? I got that DeltaS fus = 12.922J/(k*mol) Delta S Vapour = 93.475J/(K*mol) the only thing I don't get is the entropy change when 1.80 mol of HBr(g) condenses at
  41. Chemistry

    Cynthia combines 1.7 grams of Silver hydroxide with 234 ml of a 1.2 M solution of HBr. Assume all the silver hydroxide dissolves once it is in solution(which is technically not the case, but for this example, just go with the flow of it). What will be the
  42. Science

    What is the pH of a 2.62 x 10^-2 M HBr solution? thanks
  43. Chemistry

    a 2.0M solution of Hbr will have what pH?
  44. science

    a solution of hcl of concentration 1.5 mole/liter is mixed with another solution of hbr of the same concentration. calculate: 1)ph of hcl solution alone 2)ph of the final mixture
  45. chemistry

    5.00×10−3mol of HBr are dissolved in water to make 15.0L of solution. What is the concentration of hydroxide ions, [OH−], in this solution?
  46. Chemistry

    If the reaction H2 + Br2 2HBr has a rate law that can be described by k[H2][Br2]1/2, which series of reactions is a possible mechanism for the reaction? a. Br2 2Br (fast) Br + H2 HBr + H (slow) HBr + H + Br → 2HBr (fast) b. Br2 2Br (slow) Br + H2
  47. 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
  48. Chem/science

    what is the ph of 2.62 x 10 ^-2 M HBr solution? I get 5.94 is that right? thanks andy
  49. chemistry

    If 30.0 mL of 4.8 10-2 M HBr is added to 21.5 mL of 3.6 10-2 M NaOH, what is the pH of the solution?
  50. College Chemistry

    What is the approximate pH of a solution labeled 6 x 10^-5 M HBr?
  51. chemistry

    18. Calculate ƒ´H for the following reaction using Hess law H2 (g) + Br2 (g) ¡÷ 2 HBr (g) Experimental information 2 H+ ¡÷ H2 ƒ´H -436.4 kJ 2 Br- ¡÷ Br2 ƒ´H -192.5 kJ 2 H+ + 2 Br- ¡÷2 HBr ƒ´H -144.8 kJ
  52. chemistry

    Could you help me complete these equations. I can balance them after NaOH (aq) + HI (aq) ---> LiHCO3 (aq) + HI (aq) ---> HCl (aq) + NaHCO3 (aq) --> Na2CO3 (aq) + HBr (aq) --> HNO3 (aq) + KHCO3 (aq) --> HBr (aq) + NH3 (aq) ---> HNO3 (aq) +
  53. Chemistry

    What volume of 0.105 M(molarity)is needed to completely neutralize 25.0 ml of 0.180 M(molarity)HBr according to the equation: KOH(aq)+ HBr(aq)-> KBr(Aq)+ H2O(L)
  54. Chemistry

    For H2(g) + Br2(g) -> 2HBr(g) k=64 <- Ice table: H2 Br2 HBr I 0.10 0.10 0 C -x -x +2x E Solve for HBr at equilibrium I do not know how to start this.
  55. chemistry

    predict the pH of an aqueous solution that is 0.00378 molar in HBr
  56. Chemistry

    Write the net ionic equation for the reaction that occurs when aqueous solutions of barium hydroxide and hydrobromic acid are combined. I know that the first part of the formula would be BaOH + HBr but I do not know what the product would be since HBr is
  57. chem

    what is the concentration of a solution with 5 grams of HBr dissolved in 2 liters of water?
  58. Chemistry/ Dr.Bob222

    DrBob222 I am beginning to understand about balancing equations well, thanks to your help, but there are still some other things, which I am having a hard time figuring out. Complete and balance the following chemical reactions between an acid and a metal.
  59. chemistry

    equilibrium constant = 2.180 x 10^6 @ 730 C. H2 (g) + Br (g) <=> 2HBr (g) (reversible) startin with 3.20 moles of HBr in a 21.3-L reaction vessel, calculate the concentrations of H2, Br2, and HBr at equilibrium idk how to start my ice table
  60. Chemistry

    calculate the pH and the pOH of an aqueous solution that is 0.035 M In HCI and 0.080 M in HBr?
  61. Chemistry

    Calculate the pH and the pOH of an aqueous solution that is 0.025 M in HCl(aq) and 0.075 M in HBr(aq) at 25°C.
  62. chemistry

    HBr is a molecular substance that is a strong acid in water. Write an equation for its ionization in water. Use minimal integer numbers to balance the reaction. Include physical states in your answer, e.g., start with HBr(l).
  63. Chemistry

    Calculate the pOH of an aqueous solution of 146.6 ml of 0.000625 M HBr(aq) after dilution to 850 ml.
  64. Chemistry 2

    Calcualte PH and POh of an aqueous solution that is 0.050 M in HCL and 0.085 M in HBr at 25 degrees C
  65. chemistry

    calculate the pH. A solution is formed mixing 12.0 mL of .120 M HBr with 22.0mL of .180 M HCl
  66. Chemistry

    Calculate the pOH of an aqueous solution of 146.6 ml of 0.000625 M HBr(aq) after dilution to 850 ml.
  67. Chemistry

    Calculate the pOH of an aqueous solution of 146.6 ml of 0.000625 M HBr(aq) after dilution to 850 ml.
  68. chemistry

    Which of the following is a weak electrolyte in aqueous solution? a. H2SO3 b. HNO3 c. HBr d. HClO4 e. NaOH
  69. CHEMISTRY URGENT!!!

    Determine the pH (to two decimal places) of the solution that is produced by mixing 30.3 mL of 1.00×10-4 M HBr with 829 mL of 5.77×10-4 M Ca(OH)2.
  70. chemistry

    HBr is mixed with water. Which is the best description of what you would expect to find in the solution? 1. Br1−, OH1−, and water molecules 2. HBr molecules and water molecules 3. H2Br+, OH1−, and water molecules 4. H3O+, Br1−, and
  71. AP Chemistry

    HBr is mixed with water. Which is the best description of what you would expect to find in the solution? 1. H3O+, Br1−, and water molecules 2. HBr molecules, H3O+, Br1−, and water molecules 3. Br+, OH1−, and water molecules 4. HBr
  72. Chemistry

    Find the pH of each mixture of acids. 0.115 M HBr and O.125 M HCHO2. I TRIED DOING THIS PROBLEM THE SAME WAY AS THE ONE BEFORE BUT IT DIDN'T WORK. THE PH SHOULD BE 0.939. I did HBr as stronger acid and got concentration of H+ and put it into the ka
  73. chemistry

    The mean activity coefficients of HBrin 5.0 and 20.0 mmol kg –1 are 0.930 and 0.879, respectively. Consider a hydrogen electrode in HBr(aq) solution at 25 °C operating at 1.15 atm. Calculate the change in the electrode potential when the molality of the
  74. chem

    labeling form highest to lowest IMF and why HBr, LiF,CH4 HBr- Dipole, covalent LiF-Dipoole, Ionic CH4, Hydrogen bonding, -4 Is this right?
  75. chem

    What does this species represent a transition state for? CH2CH3IH20+---C---Br-/\H Hreaction of 1-propanol with HBr.reaction of 1-bromopropane with OH-.addition of HOBr to 1-propene.addition of HBr to propene with peroxides.
  76. chemistry

    a solid sample of impure Ba(OH)2 is added to 400.0 mL of 0.5000 M of aqueous HBr, a strong acid. the remaining solution was acidic. it was then titrated to equivalence point with 120.0 mL of 0.5000 M of NaOH solution. what mass of pure Ba(OH)2 was present
  77. Chemistry

    Consider the following reaction: Al + HBr ---> AlBr3 + H2 . When 4 moles of Al reacts with 3 moles of HBr, how many moles of H2 are formed?
  78. Chemistry

    In a 1.0× 10–2 M solution of CH3NH3Br(aq), identify the relative molar amounts of these species. H2O, OH-, CH3NH3+, CH3NH2, H3O+, Br-, HBr
  79. Chem

    In a 1.0× 10–2 M solution of CH3NH3Br(aq), identify the relative molar amounts from highest to lowest for : -Br- -OH- -CH3NH3+ -HBr -CH3NH2 -H3O+ -H2O
  80. Chemistry Help

    How many milliliters of 0.534 M Ba(OH)2 solution are needed to completely neutralize 34.5 mL of 0.220 M HBr solution? The reaction is Ba(OH)2(aq) + 2HBr(aq) → BaBr2(aq) + 2H2O(l) I did 0.0345 * 0.220 = 0.00759 Moles of HCl =2*0.00759= 0.01518
  81. chemistry

    A solution containing 5.00g of solid Al2(CO3)3 dissolved in water to a total volume of 200. mL is combined with 140. mL of 1.0 M HBr. Write the total of ionic equation for the reaction described below and find the molar concentration of all ions remaining
  82. chemistry

    Write the net ionic equation for the following molecular equation. HBr is a strong electrolyte. HClO is a weak electrolyte. KClO(aq) + HBr(aq) KBr(aq) + HClO(aq)
  83. General Chemistry I

    A sample of a compound containing only Br and O reacts with an excess of H2 to give 6.601 g of HBr and 3.919 g of H2O. What is the empirical formula of this compound? a. BrO b. BrO2 c. Br2O d. BrO3 e. None of the above I already know the answer is (e), but
  84. chemistry

    (a) The measured pH of a 0.200 M HBr solution at 25°C is 0.806. Calculate the activity coefficient for H . (b) The measured pH of a 0.200 M HNO3 solution at the same temperature is 0.822. Calculate the activity coefficient for H in this solution.
  85. Chemistry

    A 20.0-mL sample of 0.300 M HBr is titrated with 0.150 M NaOH. What is the pH of the solution after 40.3 mL of NaOH have been added to the acid?
  86. chemistry

    give the pH of a solution containing .972 g HBr in 628 mL of a soluion. I did .972/80.9=.012 mol. what do i do next...i'm stuck!
  87. chemistry

    A 20.0 mL sample of 0.687 M HBr is titrated with a 0.216 M NaOH solution. The pH after the addition of 10.0 mL of NaOH is __________.
  88. chemistry

    The dipole moment of HCl is 1.0 D, whuch represents a charge separation of about .17 of an electron charge. If the dipole moment of HBr is .8 D what fraction of a positive charge is found at H nucleus in HBr? Please explain
  89. pH levels

    Rank the following solutions in order of decreasing [H3O^+]. .10 M HC2H3C2 .10 M HC6H5O .10 M HF ,10 M HBr I think the correct order is: HBr>HF>HC2H3C2>HC6H5O am i right?
  90. chemistry

    A mole of HBr, a strong acid, is made up to a liter of solution with pure water. At equilibrium... (a) [H+] = 1M (b) [H+] = 0M (c) pH = 0 (d) both a & c (e) we cannot say without exact pKa of hydrobromic acid.
  91. chemistry

    A 20.0 mL sample of 0.687 M HBr is titrated with a 0.216 M NaOH solution. The pH after the addition of 10.0 mL of NaOH is __________. A. 0.413 B. 0.386 C. 0.163 D. 0.579 E. 0.237
  92. Chemistry

    an acid base titration is conducted in which 20 ml of LiOH is added to 10ml of .200M HBr to reach the equivilance point. what is the molarity of the LiOH solution?
  93. Chemistry

    Methanol (CH4O) is converted to bromomethane (CH3Br) as follows: CH4O + HBr --> CH3Br + H2O If 12.23 g of bromomethane are produced when 5.00 g of methanol is reacted with excess HBr, what is the percent yield?
  94. Chemistry

    Arrange each group of compounds/ions in order of increasing pH. 1. Li2CO3 , OH^- , NH4Br , NaCl 2. CH4 , HBr , H2O , F^- Lastly, I'd like to check if my answers for the following three questions were listed correctly in order of pH levels increasing. 3.
  95. 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)
  96. 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)
  97. chemistry-check my work

    for each of the following pairs, determine which acid is the stronger acid. A. H2S, HS- B. H2SO3, H2SeO3 C. HBr, H2Se D. HIO4, HIO3 E. H2S, H2O a. H2S b. H2SO3 c. HBr d. HIO3 e. H2S
  98. chemistry

    17. Calculate H for the following reaction using Hess law H2 (g) + Br2 (g) → 2 HBr (g) Experimental information 2 H+ → H2 H -436.4 kJ 2 Br- → Br2 H -192.5 kJ 2 H+ + 2 Br- →2 HBr H -144.8 kJ
  99. Chemistry

    The resulting pH of a solution when 100 mL of 0.877 M NH3 is mixed with 100 mL of 0.481 M HBr is ___. For NH3, Kb = 1.8 × 10−5.
  100. Chemistry

    A 500.0-mL buffer solution is 0.100 M in HNO2 and 0.150 M in KNO2. Determine whether or not each of the following additions would exceed the capacity of the buffer to neutralize it. a. 250 mg NaOH b. 350 mg KOH c. 1.25 g HBr d. 1.35 g HI Can you explain to