1. Chemistry

    The Ka of HClO is 3.0x 10^-8 at 25°c. What is the percent ionization of HClO in a 0.015M aqueous solution of HCLO at 25°c?
  2. Chemistry

    Calculate the pH for each of the following cases in the titration of 50.0 mL of 0.240 M HClO(aq) with 0.240 M KOH(aq). The ionization constant for HClO can be found here.
  3. chemistry

    A solution of HClO is mixed and found to have a pH of 4.53. Find what the initial concentration of HClO was for this solution. Ka = 3.00 × 10−8 for HClO. Answer in units of mol/L please help this is due in 1 hour
  4. Chem

    A 20.00−mL sample of an unknown HClO 4 solution requires titration with 22.92mL of 0.2200M NaOH to reach the equivalence point. What is the concentration of the unknown HClO 4 solution? The neutralization reaction is: HClO 4 (aq)+NaOH(aq)¨H 2
  5. pH calculations

    A backyard pool as a pH of 7.4. At this level, the concentrations of hypochlorus acid and hypochlorite are approximetly equal. HClO(aq) <--> H^+ (aq) + ClO^- (aq) (a) Predict the effect of increasing pH has on the concentration of HClO(aq) in the
  6. chemistry

    Calculate the pH for each of the following cases in the titration of 50.0 mL of 0.150 M HClO(aq) with 0.150 M KOH(aq). The ionization constant for HClO is 4.0x10^-8. pH before the addition of any KOH? pH after the addition of 25 mL of KOH? Please show the
  7. Chemistry

    In a 1.0× 10–4 M solution of HClO(aq), identify the relative molar amounts of these species. (most to least) H2O HClO H3O OH- OCl-
  8. Chemistry

    In a 1.0× 10–4 M solution of HClO(aq), identify the relative molar amounts of these species from most to least: HClO, OCl, OH^-, H30^+, H20
  9. Chemistry

    Calculate the pH for each of the following cases in the titration of 50.0 mL of 0.230 M HClO (aq) with 0.230 M KOH (aq). The ionization constant (Ka) for HClO is 4.00 x 10^-8. (b) after addition of 25.0 mL of KOH (d) after addition of 50.0 mL of KOH
  10. chemistry

    In a 1.0x10^-4 M solution of HClO(aq), identify the relative molar amounts of these species:HClO, OH-, H3O+, OCl-, H2O
  11. college general chemistry 2

    a chemist titrates 70 ml of .7889M HClO solution with .6221M KOH. calculate pH at equivalence. pKa of HClO is 7.50 I am getting pH of 17.72 Is that right?
  12. Chemistry

    You have 1.0 liter of .45 M HCLO (aq). At 25 degrees Celsius, Ka= 3.5x10^8 for this acid. Calculate the pH of .45 M HCLO and the concentration of CLO- at equilibrium. Thank you very much for any amount of help you are willing to give me.
  13. Chemistry

    An industrial chemist studying bleaching and sterilizing prepares several hypochlorite buffers. Find the pH of the following buffers. (a) 0.090 M HClO and 0.090 M NaClO (b) 0.090 M HClO and 0.135 M NaClO (c) 0.135 M HClO and 0.090 M NaClO (d) One liter of
  14. Chemistry

    Calculate the pH for each of the following cases in the titration of 50.0 mL of 0.200 M HClO(aq) with 0.200 M KOH(aq). The ionization constant for HClO can be found here. A. Before any addition of KOH B. After addition of 25.0 mL of KOH C. After 30.0 mL of
  15. chemistry

    Ka for hypochlorous acid, HClO, is 3.0*10^(-8). Calculate the pH after 10.0, 20.0, 30.0, and 40.0 mL of 0.100M NaOH have been added to 40.00mL of 0.100M HClO.
  16. ap chem

    What is the pH at 25C of a 0.17 M solution of the acid HClO which has an ionization constant of 3.5 × 10−8?
  17. Chemistry

    Calculate the pH for each of the following cases in the titration of 50.0 mL of 0.140 M HClO(aq) with 0.140 M KOH(aq).HClO is a weak acid with a Ka of 4.0× 10–8. It reacts with strong base to produce ClO–. (e) after addition of 60.0 mL of KOH
  18. chem

    Calculate the pH for each of the following cases in the titration of 50.0 mL of 0.150 M HClO(aq) with 0.150 M KOH(aq). The ionization constant for HClO is 4.0*10^-8 a)before addition of any KOH b)after addition of 25.0 mL of KOH c)after addition of 40.0 mL
  19. chemistry

    Calculate the [OCl-] of a 7.03×10-2 M solution of the weak acid HClO (make an approximate calculation assuming that initial concentration is equal to the equilibrium concentration). Round your answer to 3 significant digits. HClO = OCl- + H+
  20. 152

    Ka for hypochlorous acid,HCLO, IS 3.0*10^-8. Calculate the pH after 10.0,20.0,30.0, and 40.0mL OF 0.100M NaOH have been added to 40.0mL of 0.100M HCLO..
  21. chemistry

    For the weak hypochlorous acid (HClO), which statement is true at the point halfway to the equivalence point? A. The total amount of HClO is equal to the pKa. B. The total amount of HClO is equal to ClO-. C. The total amount of H3O+ is equal to the amount
  22. 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)
  23. chemistry

    The Ka of hypochlorous acid (HClO) is 3.0 × 10-8 at 25°C. Calculate the pH of a 0.0385-M hypochlorous acid solution? i got help with this problem, but i don't get where one of the numbers came from (3.4 x 10^-5)??? i tried makeing 3.0 x 10^-8 the x but i
  24. Chemistry

    How many moles are in 1.64 g hclo
  25. Chemistry

    HClO(aq) + H2O (l) <> H3O+ (aq) + ClO-(aq) Calculate the value of ΔGrxn at 25 °C for hypochlorous acid when [ClO-]=[H3O+]=5.69x10^-5 M [HClO] = 1.340 M Previously calculated a ΔGºrxn of 42.20 kJ/mol Q = [5.69x10^-5] / [1.340] = .00004245
  26. Chemistry

    calculate the ph of titration of 50.0 ml of 0.140 m hclo (aq)
  27. chem

    Given that Ka for HClO is 4.0 × 10-8 at 25 °C, what is the value of Kb for ClO– at 25 °C? Given that Kb for CH3CH2NH2 is 6.3 × 10-4 at 25 °C, what is the value of Ka for CH3CH2NH3 at 25 °C?
  28. chemistry

    I^- H5IO6 BrO2 HClO I2 Which could not disproportionate?
  29. Chemistry

    the ka of hypochlorous acid hclo is 3.5 x 10^-8. What is Kb for the hypochlorite ion?
  30. Chemistry

    what is the pH of a solution created by adding 15.5 g of KClO to 228 mL of 1.08 M HClO(aq).?
  31. chemistry

    Which of the following has the HIGHEST pKa? 1. HClO3 2. HBrO 3. HClO 4. HIO 5. HClO4
  32. CHEM 1412 general

    What is the pH of a solution that is 0.0 100 M in HClO and 0.0300 M in NaClO
  33. chemistry..

    to drbob222 ok, the pka (hclo) = 7.54 the ph = 7.35 this problem was under "preparing a buffer" section
  34. chemistry

    Please identify the acid and the base in this equation. HClO + NaOH = NaClO + H2O Thank you!
  35. Chemistry

    What is the correct net equation for: LiOH(aq) + HClO(aq) → LiClO(aq) + H2O(l)?
  36. chemistry

    If you had 500.0 ml of a 0.10 M solution of HCLO, what mass of the corresponding Na+ (sodium salt) of the conjugate base would you need to make the buffer?
  37. chemistry

    What is the molarity of OH- in a 7.68×10-4 M NaClO solution that hydrolyzes according to the equation. ClO-(aq) + H2O(l) = OH-(aq) + HClO(aq) Constants: Kh=2.86×10-7 Can someone help me figure this one out?
  38. chemistry

    What is the molarity of OH- in a 7.68×10-4 M NaClO solution that hydrolyzes according to the equation. ClO-(aq) + H2O(l) = OH-(aq) + HClO(aq) Constants: Kh=2.86×10-7 Can someone help me figure this one out?
  39. Chem

    Balance the following redox reactions in acidic solution by the half-reaction method Br–(aq) + I–(aq) + HClO(aq) = Br2(l) + IO3 + Cl–(aq)
  40. chemistry

    Rank the following compounds in order of increasing acid strength (1 = weakest, 4 = strongest) HClO HClO3 HClO2 HClO4
  41. CHEMISTRY!!

    1) How would you prepare 20 mL of a solution having pH = 2.00 by dilution of 0.10 M HCl? 2) The Ka, for hypochlorous acid, HClO, is 7.2 x l0^–4 at 25°C. What is pKa? Write the equation for the reaction to which Ka applies.
  42. Chemistry

    What is the pH of a 0.42 M NH4NO3 aqueous solution? What is the percent ionization?
  43. Chemistry

    What will happen if a small amount of hydrochloric acid is added to a 0.1 M solution of HF? A) The percent ionization of HF will increase. B) The percent ionization of HF will decrease. C) The percent ionization of HF will remain unchanged. D) Ka for HF
  44. Chemistry (really need quick help)

    Balance the following equations. (Use the lowest possible coefficients. These may be zero.) (a) As(s) + ClO3-(aq) ---> H3AsO3(aq) + HClO(aq) (acidic solution) I am using half-reactions but I don't really get this at all. Can someone explain?
  45. chemistry

    For a week acid whose ionization constant is 1.75 x 10(-5), the pH of its solution is 3.0. Determine its degree of ionization and its percent ionization.
  46. AP Chem

    A lab manual states that to prepare a certain buffer requires mixing 25 ml of 0.200 M HClO (Ka=3.00 x 10^-8) with 50 ml of 0.2 M NaClO What is the Ph of this buffer?
  47. more chemistry

    What volume of 0.115 M M HClO 4 \rm HClO_4 solution is needed to neutralize 58.00mL mL of 8.75×10−2 M M NaOH \rm NaOH
  48. Chem II Oxidation Reduction

    Sb+1 + HClO ------> Sb2O5 + Cl-1 I'm not doing something right. I think I have the charges correct, this is what I have so far . . . . 2Sb^+1 -----> Sb^+5 + 4e- 2(2e- + Cl^+1 ------> Cl^-1 then when I start subbing everything back and start trying
  49. Chemistry

    When all the following solutes act as acids, the one with the weakest conjugate base is a. H2SO3. b. H2CO3. c. HClO4. d. HClO. e. HF. 4. (Points: 1) A sample of ammonia (Kb = 1.8 * 10^-5) is titrated with 0.1 M H2SO4. At the equivalence point, the pH is
  50. Chemistry Please HELP!

    calculate the mass of each product formed if 10.0 g of the first reactant is reacted with 10.0 g of the second reactant: NCl3 + 3 H2O → 3 HClO + NH3 (Please show me full working out)
  51. College Chemistry

    what is the approximate pH of a solution labeled 0.050 M HClO? I realized my mistake on my last post but this isnt a strong acid nor a strong base so how do i solve this?
  52. Chemistry

    What is the molarity of OH- in a 7.83×10-3 M NaClO solution that hydrolyzes according to the equation. ClO-(aq) + H2O(l) = OH-(aq) + HClO(aq) The information they give is that constants Kh=2.86E-7 I know how to solve the problem when the constant Kw is
  53. Chemistry

    3HClO2(aq) +2Cr3+(aq) + 4H2O(l) -> 3HClO(aq) + (Cr2O7)2–(aq) + 8H+(aq) At pH 0.00, with [Cr2O72–] = 0.80 M, [HClO2] = 0.15 M, and [HClO] = 0.20 M, the cell voltage is found to be 0.15 V. Calculate the concentration of [Cr3+] in the cell Ecell = 0.31
  54. CHEM-102

    Ka for hypochlorous acid,HClO is 3.0x10^-8. Calculate the pH after 10.0, 20.0, 30.0, and 40.0mL of 0.100M NaOH have been added to 40.0mL of 0.100M HOCl.
  55. chemistry

    The Ka of hypochlorous acid (HClO) is 3.00×10-8 at 25.0°C. Calculate the pH of a 0.0385 M hypochlorous acid solution. a.1.41 b.7.52 c.-1.41 D.4.47 E. 8.94 I got B 7.52 but i feel like im wrong
  56. CHEMISTRY

    a) Write the formula for each component in a buffer solution of acetic acid and its’ salt. b) The Ka, for hypochlorous acid, HClO, is 7.2 x l0^–4 at 25°C. What is pKa? Write the equation for the reaction to which Ka applies.
  57. Chemistry

    Which one of the following pairs of reactants would react together in a Lewis Acid/Lewis Base reaction? a. KOH and HNO2 b. NaOH and HCl c. CH3COOH and HF d. Ag+ and NH3 e. HClO and NH3
  58. chemistry

    The Ka of hypochlorous acid (HClO) is 3.00×10-8 at 25.0°C. Calculate the pH of a 0.0385 M hypochlorous acid solution. A.1.41 B.7.52 C.-1.41 D.4.47 E.8.94 I chose B
  59. Chemistry

    Ag2S is an insoluable black solid. Would more solid dissolve, or precipitate once the following are added to the solution. 1. KS-----I know [S] increases, shift to reactants side, precipitate 2. HClO 3. LiOH 4. NH4OH
  60. chemistry

    What is the percent ionization of a 1.38 mol/L weak acid if its Ka = 2.7 x 10-6? Answer to two (2) decimal places. I know what steps to use but have difficulty applying them to the quesiton Can someone please complete the question for me since there are
  61. CHEMISTRY

    I have these equations in our book , but I've tried a few times to solve it in half reaction method , but I couldn't yet : 1) KMnO4 + KIO3 => MnO2 + KIO4 ( in a basic solution ) 2) MnO4- + Cl- => Mn^+2 + HClO ( in a acidic solution ) I think these
  62. A few chemistry

    I got the rest of the homework, but these are confusing me so much...ugghhhh. 1. The pH of a .400 M solution of iodic acid, HlO3, is .726 at 25 degrees C. What is the Ka(acid constant) at this temperature? 2. The pH of a .150 M solution of HClO is found to
  63. chem help

    a. Determine the percent ionization for a 1.00M phosphoric acid solution at 25.0 oC given the following (assume the small x approximation is valid) H3PO4(aq) H2PO4(aq)H+(aq) ΔGf (kJ/mol) -1142.6| -1130.2 | 0 b. Assuming ΔGf does not change with
  64. Chemistry

    Which solution will have the lowest pH? a. 0.10 M HClO2, pKa = 1.96 b. 0.10 M HCN, pKa = 9.21 c. 0.10 M HF, pKa = 3.19 d. 0.10 M HClO, pKa = 7.538 e. 0.00010 M HCl Does the lower the pka stronger the acid, means the lower the ph, so the answer is A?
  65. Chem

    What simplifying assumptions do we usually make in working problems involving equilibria of salts of polyprotic acids? Why are they usually valid? Answer by selecting all true statements. Are the answers: a,b,d,and f A)If the two ionization constants are
  66. Chemistry

    I just to know how to identify the substance that is reduced, the substance that is oxidized, the oxidizing agent and the reducing agent in each reaction. As (s) + ClO3-(aq) → H3AsO3 (aq) + HClO(aq) CN-(aq) + MnO4-(aq) → CNO-(aq) + MnO2(s)
  67. chemistry

    a) Calculate the percent ionization of 0.125M lactic acid (Ka=1.4x10^-4) b) Calculate the percent ionization of 0.125M lactic acid in a solution containing 0.00075 M sodium lactate.
  68. Chemistry

    The pH of an 0.0870 M solution of weak acid A is 2.20. The pH of an 0.0830 M solution of weak acid B is 4.07. The pH of an 0.0890 M solution of weak acid C is 5.13. Identify the three acids from among those listed below (the Ka values are listed in
  69. chemistry

    Given the table of Ka values on the right below, arrange the conjugate bases in order from strongest to weakest. Acid Ka HClO 3.5 e-8 HClO2 1.2 e-2 HCN 6.2 e-10 H2PO4- 6.2 e-8 A. ClO2-, ClO¬-, HPO42-, CN- B. ClO2-, HPO42-, ClO¬-, CN- C. CN-, HPO42-,
  70. Chemistry

    Calculate the percent ionization of cyanic acid, Ka=2.0x10^-4, in a buffer soln that is .50M HCNO and .10M NaCNO. Answer is .20%. So,I know that NaCNO-->Na+ + CNO- so [CNO-]=.10M from ICF chart. and then HCNO <=>H+ + CNO- where: [HCNO]= .5 and
  71. Chemistry

    A solution is prepared by mixing 13.00 ml of .0021 M aqueous Hg2(NO3)2 with 25 ml of .015M HCL. Assme that volumes are additive. a) Will precipitation occur? b) Calculate [HG2 2+], [CL-], and [NO3] after equilibrium is established.
  72. chemistry

    A 0.185 M solution of a monoprotic acid has a percent ionization of 1.55%. Determine the acid ionization constant (Ka) for the acid.
  73. Stupid Chemistry

    Ok, blonde moment here, Kb is the same as Ka but just for bases and Ka is for acids correct? right. Ka is the ionization constant for acids, Kb is the ionization constant for bases. BUT, we can change one into the other this way. KaKb = Kw. So if you are
  74. chemistry

    for chemical equilibrium, what is the difference between percent ionization and percent dissociation
  75. chem

    which of these are strong electrolytes, weak electrolytes and non electrolytes. H2SO4 FeCl2 HClO AgCl I put AgCl as a non H2So4 and HCl as strong FeCl2 as weak but the computer told me my answer is wrong Can some one help please?
  76. chemistry

    Calculate the percent ionization of a .31 molar solution of acetic acid. The ionization constant of acetic acid is 1.8 x 10^-5
  77. chemistry

    i have no idea how ionization works, yet i have to do a worksheet on it! help! how does ionization, and how do you tell which element has a higher ionization energy in relation to another? PLZ ANSWER SOON! I NEED HELP!
  78. chemistry

    25. Which of the two reactions, A or B is a neutralization reaction? Explain why. A. HBr + H2O = Br- = H3O+ B. HClO + NaOH = NaClO + H2O 26. A. Look at the reaction again. when this reaction is reversed. Br- + H3O+ = HBr = H2O what substance is the acid,
  79. chemistry

    What is the percent ionization of 0.025 M chlorous acid, HClO2 solution? Ka HClO2 = 1.1*10^(-2) Answer: 48% What I did: HClO2(aq) + H2O(l) -><- ClO2(aq) + H3O(aq) initial-change-end table results: x^(2)/(.025-x)=1.1*10^(-2) x=1.6*10^(-2) % ionization
  80. Chemistry

    What is the percent ionization for each of the following acids? a. 0.022 M HClO2 solution of pH= 3.88 Answer obtained: .60% pH = 10^(-3.88) = 1.32 x 10^-4 % ionization= [H+] formed divided by MHA (original acid concent) x 100 = (1.32x10^-4)/0.022 x 100 =
  81. Chemistry

    which of the following statements are true? a) For an acid H-O-A : the greater the electronegativity of A, the weaker the acid HA b) For an acid H-A : the weaker the H-A bond, the stronger the acid H-A c) HF is a stronger acid than HCl d) HClO4 is a weaker
  82. mvcc

    determine the molatiry of each of the ions present in the following aqueous solutions[assume 100% ionization] 2.25 M FeCl3
  83. chemistry

    how do you write the ionization reaction and the acid ionization constant expression for the third ionization of phosphoric acid in water? Can you explain the main concepts that are involved in this?
  84. chemistry final-urgent

    Choose the element with the highest ionization energy element: Na, Mg, Al, P, S In my book: ionization energy increase from left to right and bottom to top. Na<Mg<Al<P<S S is highest ionization energy? my instructor review this problem and his
  85. chemistry (Bohr model)

    The second ionization energy of He is almost exactly four times the ionization energy of H, and the third ionization energy of Li is almost exactly nine times the ionization energy of H: IE (MJ mol-1) H(g) --> H +(g) + e- (1.3120) He+(g) --> He2+(g)
  86. Chemistry

    Calculate the percent ionizationof a 0.15 M benzoic acid solution in pure water Nd also in a solution containing 0.10M sodium benzoate. Why does the percent ionization differ significantly in the two solutions?
  87. Chemistry

    Which of the following can we predict from an equilibrium constant for a reaction? 1 The extent of a reaction 2 Whether the reaction is fast or slow 3 Whether a reaction is exothermic or endothermic a. 1 only b. 2 only c. 3 only d. 1 and 2 only e. 1 and 3
  88. chemistry

    Knowing that 1 mol of a certain monoprotico acid, HX, contained in 1 litre aqueous solution, this 50% ionized, point the value of its ionization constant.
  89. chemistry

    The pH of a 0.164 M aqueous solution of dimethylamine is 11.98. Write the ionization equation, calculate the values of Kb and pKa and comment on strength of the
  90. Chem

    Which group shows the correct order of first ionization energy? Ca > Na > K Al > Si > P K > Ca > Ge Na > P > Cl Cs < Rb < Na I know the closer the element is to the right side of the table, group 8, the higher the ionization
  91. Chemistry

    Which one of the following pairs of 0.100 mol L-1 solutions, when mixed, will produce a buffer solution? A. 50. mL of aqueous CH3COOH and 25. mL of aqueous CH3COONa B. 50. mL of aqueous CH3COOH and 25. mL of aqueous HCl C. 50. mL of aqueous NaOH and 25. mL
  92. math

    A bond has an average return of 6.8 percent and a standard deviation of 4.6 percent. What range of returns would you expect to see 68 percent of the time? a. 2.2 percent to 11.4 percent b. 4.6 percent to 11.4 percent c. 4.6 percent to 22.8 percent d. 11.4
  93. Chemistry

    Calulate the degree of ionization for NH3(aq) in 1.0 M solution, Kb = 3.236E-4. I've seen degree ionization for acids and not bases. Do I need to find the Ka [H+] value of the base to determine the degree of ionization?
  94. Chemistry

    How do these react? Some may have no reaction. a. aqueous chromium(III) nitrate plus magnesium metal b. aqueous lithium sulfate plus aqueous barium chloride c. solid lead metal plus aqueous potassium chloride d. aqueous lithium fluoride with aqueous
  95. Chem

    It is possible to determine the ionization energy for hydrogen using the Bohr equation. Calculate the ionization energy for an atom of hydrogen, making the assumption that ionization is the transition from n=1 to n=infinity. I don't know how to solve this
  96. university of the west indies

    The pH of a 0.164 M aqueous solution of dimethylamine is 11.98. Write the ionization equation, calculate the values of Kb and pKb and comment on strength of the base....
  97. Chemistry

    It is possible to determine the ionization energy for hydrogen using the Bohr equation. Calculate the ionization energy for an atom of hydrogen, making the assumption that ionization is the transition from n=1 to n=infinity. I don't know how to solve this
  98. Chemistry

    The pH of a 0.010 M aqueous solution of a weak monoprotic acid, HX, is 4.5. What is the value of the acid ionization constant?
  99. chemistry

    What is the percent ionization of a 1.38 mol/L weak acid if its Ka = 2.7 x 10^-6? Thanks again!
  100. Chemistry

    Calculate the concentration of H+ ions of an aqueous solution of nitrous acid ( HNO2) to 0.02 mol/L knowing that the degree of ionization of acid is 3%