chemistry

A 40.0 mL sample of 0.150 M Ba(OH)2 is titrated with 0.400 M HNO3. Calculate the pH after the addtion of the following volumes of acid, and plot the pH versus millimeters of HNO3 added.

a. 0.00 mL
b. 10.2 mL
c. 19.9 mL
d. 30.0 mL
e. 39.8 mL

  1. 👍 0
  2. 👎 0
  3. 👁 246
  1. First determine where the equivalence point is (how many mL HNOe are required).
    At zero mL, calculate pH from pure Ba(OH)2.
    All points from zero to the equivalence point, use an ICE chart to determine how much Ba(OH)2 remains, then determine pH from that. Remember to take into account the dilution of the base.
    At equivalence point, the pH is the pH of pure water since this is a strong acid/strong base titration.
    All points after the equivalence point, use an ICE chart to determine how much HNO3 is in excess and determine pH from that. Post your work if you get stuck.

    1. 👍 0
    2. 👎 0

Respond to this Question

First Name

Your Response

Similar Questions

  1. 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?

    asked by Lori on November 9, 2013
  2. Chemistry

    Calculate the pH at the halfway point and at the equivalence point for each of the following titrations. (a) 100.0 mL of 0.14 M HC7H5O2 (Ka= 6.4 multiplied by 10-5) titrated by 0.14 M NaOH halfway point equivalence point (b) 100.0

    asked by Andrew on June 1, 2012
  3. Chemistry

    A 2.52g sample of a compound containing only carbon, hydrogen, nitrogen, oxygen, and sulfur was burned in excess O to yield 4.36g of CO2 and 0.892g of H20. Another sample of the same compound of mass 4.14g, yielded g of SO3. A

    asked by Christina on September 6, 2010
  4. Chemistry

    A 0.450-gram sample of impure CaCO3(s) is dissolved in 50.0 mL of 0.150 M HCl(aq). The equation for the reaction is: CaCO3(s)+2HCl(aq) -> CaCl2(aq) + H2O(l) + CO2(g) The excess HCl(aq) is titrated by 9.75 mL of 0.125 M NaOH(aq).

    asked by Katherine on April 10, 2012
  5. Economics (40)

    A market research firm conducts telephone surveys with a 42% historical response rate. What is the probability that in a new sample of 400 telephone numbers, at least 150 individuals will cooperate and respond to the questions? In

    asked by Mia on May 9, 2014
  1. chemistry

    A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3. Determine the pH of the solution before the addition of any KOH. The Kb of NH3 is 1.8 × 10-5. I thought that I would need a second volume to find the moles of NH3?

    asked by Sydney on November 6, 2014
  2. Chemistry-Dr.Bob222

    A 25.0 mL sample of 0.125 M pyridine is titrated with 0.100 M HCl. Calculate the pH at 0 mL of added acid.

    asked by Nevaeh on April 19, 2016
  3. Chemistry

    Calculate the molar concentration of acetic acid (CH3COOH) in a 5.00-mL sample of vinegar (density is 1.00 g/mL) if it is titrated with 25.00 mL of NaOH.

    asked by Jake on March 4, 2009
  4. Chemistry

    A water chemist obtained a 250 ml sample from a nearby lake and fixed the oxygen on-site with alkaline solutions of MnSO4 and KI-NAN3. Returning to the laboratory, a 200 ml sample was analyzed by acidifying the sample with conc

    asked by Dalal on March 20, 2018
  5. Chemistry Titration Lab HELP!

    Hi everyone! I just got a new lab that I MUST complete today, and it's about titration- I have absolutely no clue how to do it, it just doesn't make sense to me! I hope that someone can help explain to me how to do it so I can

    asked by Angel on June 11, 2008
  6. Chemistry

    1-A sample of potassium hydrogen oxalate, KHC2O4, weighing 0.717 g, was dissolved in water and titrated with 18.47 mL of an NaOH solution. Calculate the molarity of the NaOH solution. 2-A 35 mL drinking water sample, whose pH is

    asked by Hiba on June 11, 2020

You can view more similar questions or ask a new question.