posted by .

Sodium hypochlorite, NaClO, is added as a disinfectant to the water supply. You
are analyzing a sample from the supplier to verify its purity and you prepare to titrate 250.0 mL of a solution containing 1.86 g of NaClO with a 1.00 M HCl solution.
What is the pH of the solution at the equivalence point?

  • Chemistry -

    I must admit this is a new one on me; however, I assume we have HClO at the equivalence point.
    moles NaClO = 1.86/about 74 = about 0.025
    moles HClO = 0.025 at equivalence point.
    How much 1M HCl is required to titrate the sample? That will be M = mmols/mL or
    mL = mmols/M = 25 mmoles/1M = 25 mL. The initial volume was 250 mL so the final volume is 250+ 25 = 275 mL.
    (HClO) = mmoles/total volume = 25/275 = 0.0909M
    ..........HClO ==> H^+ + ClO^-

    Ka = (H^+)(ClO^-)/(HCl0)
    Substitute from the ICE chart above into the Ka expression and solve for (H^+), then convert to pH by pH = -log(H^+).
    Post your work if you need additional assistance.

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. Chemistry Help Please

    Titration of a Sample of Household bleaches: The oxidizing agent in a household bleach is determined by placing 100 mL of distilled water in a 250 mL Erlenmeyer flask and adding 10 mL of the 10% (w/w) KI solution, swirling the contents …
  2. Chemistry

    Commercial bleach contains 5.25% (by mass) of NaClO in water. It has a density of 1.08 g/mL. Calculate the molarity of this solution. (Hints: assume you have 1 L of solution (mass 1080 g); molar mass of NaClO is 74.4 g/mol)
  3. Ap Chemistry

    I'm doing the calculations on the lab "Oxidizing Power of Laundry Bleach," and I'm stuck on one part. This is what I have so far: My average volume of sodium thiosulfate is 6.94 ML. I then converted that into moles and got 6.94X10^-4 …
  4. Chemistry

    A solution household bleach contains 5.25% NaClO, by mass. Assuming that the density of bleach is the same as water(1.0g/ml). Calculate the volume in mL of household bleach that should be diluted with water to make 500.0 ml of a pH= …
  5. Chemistry

    CONCENTRATION OF NaClO IN COMMERCIAL BLEACH. Bleach comes as 6%(mass/volume) solution of NaClO. Calculate the Molarity of NaClO in bleach to three significant figures ( you need molar mass of NaClO)
  6. 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 …
  7. chemistry

    Household bleach contains (NaClO)2 that decomposes in water, NaClO + h2o = Na+ + OH- + Cl2 + O2 If 15ml bleach containing 5.85℅ NaClO is allowed to decomposes completely, then hoe many mL of o2 at 22C and 755mmHg can be liberated. …
  8. Chemistry

    Solutions of sodium hypochlorite, NaClO are sold as bleach. They are prepared by the following reaction: 2NaOH + Cl2 --> NaCl + NaClO + H2O If you have 2.32 mol of NaOH and 2.74 mol of Cl2 ga available to react, answer the following …
  9. Chemistry

    List the grams of bleach solution necessary to provide 0.931g of NaClO(laundry bleach is 8.25% NaClO by weight) and the mL of bleach solution that contains the necessary amount... NaClO=74.442 g/mol. Need 0.931 grams of NaClO. Density …
  10. Chemistry

    I have 25 million gallons of water at a pH of 6.5. I add 17.4 million gallons of 12.5% by wt sodium hypochlorite (NaClO) at a pH of 12.5 to this water. What will my pH of my final solution be?

More Similar Questions