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

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  1. chemistry

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

  2. 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

  3. 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-

  5. 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

  6. 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?

  7. Chem

    In a 1.0x10^-6 M solution of HNO3(aq) at 25 degrees C, identify the relative molar amounts of species from most to least. HNO3 H3O+ H2O OH- NO3-

  8. 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

  10. 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?

  11. CHEMISTRY

    In a 1.0x10^-6 M soltution of HNO3(aq), identify the relative molar amounts of these species. H2O , HNO3, H3O+,NO3-, OH-

  12. Chemistry

    In a 1.0x10^-6 M soltution of HNO3(aq), identify the relative molar amounts of these species. H2O , HNO3, H3O+,NO3-, OH-

  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

  15. 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

  16. 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 pool. For this

  17. 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

  18. 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.

  20. 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+

  21. 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.

  22. 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.

  23. 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

  25. 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

  26. 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..

  27. Chemistry

    Identify the relative molar amounts of the species in 0.10 M NaBr(aq). NaBr, Na+, Br-, H3O+, OH-, H2O

  28. Chemistry

    Identify the relative molar amounts of the species in 0.10 M NaBr(aq). NaBr, Na+, Br-, H3O+, OH-, H2O

  30. 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

  31. 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)

  32. Chemistry

    In a 1.0 x10-6 M of HNO3 (aq) at 25 degrees celsius identify the relative molar amounts of theses species HNO3- H3O+ OH- NO3- H2O

  33. 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

  35. chemistry

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

  36. 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

  37. 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.

  38. CHEM 1412 general

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

  40. ap chem

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

  41. 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).?

  42. 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

  43. 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

  45. 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?

  46. 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?

  47. 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?

  48. 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)

  50. Chemistry

    Hi, I posted yesterday with this lab question. "Calculate the molar amounts of NaOH used in the reaction with the HCl solution and with the HC2H3O2. I think I got the answer to that with the help that I received. I had 5 mL of HCl, and I was using .100 M

  51. 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 M equation used:

  52. 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.

  53. 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?

  55. 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 are

  56. 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

  57. 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

  58. Chemistry

    How many moles are in 1.64 g hclo

  60. 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?

  61. 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

  62. 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?

  63. chemistry

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

  65. Chemistry

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

  66. Chemistry

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

  67. 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

  68. chem

    balance the following equation please. comes from two half cell. HClO(aq)+ H^+(aq)+ e -> Cl^- (aq) +H2O(l)

  70. chemistry..

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

  71. chemistry

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

  72. Chemistry

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

  73. 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.

  75. 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

  76. 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

  77. Chemistry

    calculate the overall equilibrium constant, 𝐾overall, for the reaction CH3COOH(aq)+ClO−(aq)↽−−⇀CH3COO−(aq)+HClO(aq)

  78. 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

  80. 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) C2H5OH +

  81. 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

  82. chemistry

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

  83. 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?

  85. 8th Grade math PLEASE CHECK MY ANSWERES

    1.Write the number in standard form: 7.1x10^4 A)710 B)7,100 C)71,000 D)710,000*** 2.Write the number in standard form: 5.01x10^-3 A)5,010 B)0.501 C)0.0501 D)0.00501*** 3.Multiply (2.0x10^4)(3.0x10^3)=? A)6.0x10^7*** B)6.0x10^12 C)6.0x10^5 D)6.0x10^43 Add.

  86. Chemistry--need help!

    1. All the following act as a Lewis acid in water except a. SO3 b. BH3 c. Sn4+ d. Na2O *** I think c or d. 2. Which acts as a Lewis acid but neither Arrhenius nor Brønsted-Lowry? a. Fe3+(aq) b. NH3(aq) c.HCOOH(aq) d. HClO(aq) 3. An unknown solution forms

  87. 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?

  88. Buffers

    A buffer containing 0.30 M HCLO and 0.30 M NaClO has a pH of 7.53. What will the pH be after .010 mol of NaOH is added to 100 ml of the buffer. Answer options: 7.83 7.53 8.23 7.03

  90. 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 to

  91. 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

  92. 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)

  93. 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

  95. Chemistry

    Consider the following reaction that describes the solubility equilibria of solid Zn(OH)2 in aqueous solution (Ksp of Zn(OH)2 4.0x10^-17. Calculate molar solubility of Zn(OH)s in an acidic solution of pH5.0.

  96. Chemistry

    Consider the following reaction that describes the solubility equilibria of solid Zn(OH)2 in aqueous solution (Ksp of Zn(OH)2 4.0x10^-17. Calculate molar solubility of Zn(OH)s in an acidic solution of pH5.0.

  97. Chemistry

    Write the HA reaction for each acid below. Account for the following activity order by drawing the important resonance contributing structures (those having only one negative (-) formal charge) for A-. HA + H2O H3O+ + A- stronger HClO4>HClO3>HClO weaker

  98. Chemistry

    Which of the following are Arrhenius bases? (a) H3AsO4 (b) Ba(OH)2 (c) HClO (d) KOH Which of the following are Arrhenius bases? (a) CH3COOH (b) HOH (c) CH3OH (d) H2NNH2

  100. 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

  101. Science

    A biologist made population counts of four different species of animals in an ecosystem. What can you infer from these numbers about possible predator-prey relationships between the species? Species A 155 Species B 17 Species C 2,467 Species D 19 ·

  102. science (check!)

    A biologist made population counts of four different species of animals in an ecosystem. What can you infer from these numbers about possible predator-prey relationships between the species? Species A:155 Species B:17 Species C:2467 Species D:19 A.Species

  103. Science

    A biologist made population counts of four different species of animals in an ecosystem. What can you infer from these numbers about possible predator-prey relationships between the species? Species A:155 Species B:17 Species C:2467 Species D:19 A.Species

  105. AP Chemistry

    A vessel contains 500. milliliters of a 0.100-molar H2S solution. For H2S, Ka1 = 1.0 X 10-7 and Ka2 = 1.3 X 10-13 (a) What is the pH of the solution? (b) How many milliliters of 0.100-molar NaOH solution must be added to the solution to create a solution

  106. science

    Please help A researcher performed an analysis of the elemental composition of several fish species living in the same body of water. The amount (in parts per million) of iron (Fe), calcium (Ca), potassium (K), sodium (Na), and magnesium (Mg) found in each

  107. chemistry

    Adding a complex ion forming species to a solution will increase the solubility of a slightly soluble species. Calculate the Molar solubility (s) of AgI in a 1.75 M ammonia solution. The Ksp for AgI is 8.3 x 10-17 and the Kf for Ag(NH3)2+ is 1.5 x 107. I

  108. chemistry

    1. Calculate the volume of carbon dioxide at 273 K and 1.01 * 10^5 Pa which would be produced when 1.25g of calcium carbonate reacts completely with HCL. and 2. When 41.18 cm^3 of a solution of silver ions with concentration of .2040 mol dm^-3 is added to

  110. Science

    2. Study the amino acid sequences of the same protein taken from four different species of plants. Which pair of plants is most closely related? Species 1: -A-P-A-C-W- Species 2: -G-P-G-S-F- Species 3: -A-P-A-C-F- Species 4: -N-K-M-H-H- A. Species 2 and 4

  111. Chemistry

    what is Kc at 25 celsius for the following equilibrium? CH3BH3^+ +H2O CH3NH2 + H3O^+ Kb=4.4x10^-4 I got 4.0x10^4 / 1.0x10^-14 = 4.0x10^-10 (correct)?

  112. Chemistry

    0.1825 g of Fe(NH4)2(SO4)2•6H2O is dissolved in 250.00 mL of solution; this is Solution A. 5.00 mL of Solution A is transferred to another flask, and it is diluted to a total of 100.0 mL to make another solution, which is Solution B. Next, 3.00 mL of

  113. Chemistry

    3. 0.1825 g of Fe(NH4)2(SO4)2•6H2O is dissolved in 250.00 mL of solution; this is Solution A. 5.00 mL of Solution A is transferred to another flask, and it is diluted to a total of 100.0 mL to make another solution, which is Solution B. Next, 3.00 mL of

  115. Chemistry

    3. 0.1825 g of Fe(NH4)2(SO4)2•6H2O is dissolved in 250.00 mL of solution; this is Solution A. 5.00 mL of Solution A is transferred to another flask, and it is diluted to a total of 100.0 mL to make another solution, which is Solution B. Next, 3.00 mL of

  116. Chemistry

    A 100 milliliter sample of 0.100-molar NH4Cl solution was added to 80 milliliters of a 0.200-molar solution of NH3. The value of Kb for ammonia is 1.79 x 10^-5. (a) What is the value of pKb for ammonia? (b) What is the pH of the solution described in the

  117. Chemistry

    A 100 milliliter sample of 0.100-molar NH4Cl solution was added to 80 milliliters of a 0.200-molar solution of NH3. The value of Kb for ammonia is 1.79 x 10^-5. (a) What is the value of pKb for ammonia? (b) What is the pH of the solution described in the

  118. AP Chemistry

    A 100. milliliter sample of 0.100-molar NH4Cl solution was added to 80.0 milliliters of a 0.200-molar solution of NH3. The value of Kb for ammonia is 1.79 X 10-5. (a) What is the value of pKb for ammonia? {b) What is the pH of the solution described in the

  120. chemistry

    Which weak acid would be best to use when preparing a buffer solution with a pH of 8.50? 1) an acid with Ka=3.3x10^-9 2) an acid with Ka=5.0x10^-4 3) an acid with KA=6.3x10^-6 4) an acid with Ka=5.0x10^-7 5) an acid with Ka=4.0x10^-5 6) an acid with

  121. Chemistry Math

    Ka for a 0.100 M hydrofluoric acid solution where whose pH is 2.23 is a. 3.5x10-4 b. 3.5x10-2 c. 8.0x10-1 d. 8.0x10-2 ^I'm not sure how to solve.

  122. Chemistry

    A solution is prepared by dissolving 571.6 g of H 2SO4 in enough water to make 1000.0 mL of solution. The solution has a density of 1.3294 g/mL. (molar mass of H2SO4 = 98.08). What is the molar concentration of the solution?

  123. science

    The graph below shows the percent of seeds from two plant species that sprout when grown in water containing different amounts of salt Which of the following best summarizes the effect of saltwater on these plant species?

  125. HELP!

    A biologist made population count of four different species of animals in an ecosystem. What can you infer from these numbers possible predator-prey relationship[s between species? Species A : 155 Species B : 17 Species C : 2,467 Species D : 19

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