Chemistry

Why is the equivalence point of a weak acid-strong base titration above 7.0? How can the data reflect this?

The titration of a weak acid with a srong base produces a salt of the two. The anion is hydrolyzed in water solution but the cation is not.
A^- + HOH ==> HA + OH^-
The production of OH^- shows that a water solution of this salt will be basic. The data will reflect that because you probably used an indicator that changed color above 7.0.

  1. 👍 0
  2. 👎 0
  3. 👁 74

Respond to this Question

First Name

Your Response

Similar Questions

  1. chemistry

    if 0.4M NaOH is titrated with 0.4M HF, how do we calcualte the ph at equivalence. The book assumes each is 1L, but why do we use 1L * chemistry - Dr.Jim, Thursday, November 11, 2010 at 5:31am HF is a weak acid, so you need the

    asked by flame on November 11, 2010
  2. Chem+ASAP+2 fill in the blank questions+ASAP!!!

    PLease check this. They are fill in the blank and I just need to know if they are right. Thanks! 9. Compared to a strong acid-strong base titration curve, a weak acid-strong base titration curve has a (higher, lower) __higher___

    asked by David on August 8, 2006
  3. titrations

    I have to find the correct acid-base indicator to use for the following titrations (methyl orange with end point @ pH 4, bromthymol blue with end point @ pH 7, or phenopthanlein with end point @ pH 9). I have several problems

    asked by Taylor on May 5, 2007
  4. CHEMISTRY

    How can we determine the equivalence point ( or end point ) in the curves in titration ( strong acid/weak base and weak acid/strong base )

    asked by MAD on September 12, 2014
  5. Chemistry

    In the titration of a weak acid with a strong base, the pH at the equivalence point is affected mostly by a.hydrolysis (reaction with water) of the weak acid b.the dissociation of water molecules c.the presence of excess base

    asked by Cheryl on May 26, 2011
  6. AP Chemistry

    A solution is prepared by titrating a 100.0 mL sample of 0.10 M HF (Ka = 7.2 × 10-4) with 0.10 M NaOH a. Does the solution contain a strong acid with a strong base, a strong acid with a weak base, a weak acid with a strong base,

    asked by Anonymous on March 23, 2016
  7. AP Chemistry

    A solution is prepared by titrating a 100.0 mL sample of 0.10 M HF (Ka = 7.2 × 10-4) with 0.10 M NaOH a. Does the solution contain a strong acid with a strong base, a strong acid with a weak base, a weak acid with a strong base,

    asked by jesse on March 23, 2016
  8. chemistry

    1. An aqueous solution of weak base B of unknown concentration is tritrated with a known concentration of strong acid, HA. (a) Write the balanced chemical equation for this acid-base reaction, identifying the conjugate acid/base

    asked by Phuong on April 8, 2011
  9. Chemistry

    Plot the titration of a weak base with a strong acid. Show the titration curve using .106M NH3 and .225M HCl for a 50.00mL sample of the ammonia. No idea where to start here. I'm supposed to plot the curve from 2mL increments

    asked by Andrew on October 22, 2014
  10. chemistry

    ) At the equivalence point in the titration of a strong acid with a strong base, do you expect the pH to be acidic, basic, neutral? Explain your answer. If the titration involves a strong acid with a strong base, the pH = 7 at the

    asked by Anonymous on March 3, 2009
  11. chemistry

    A 1.0 M acetic acid solution (CH3COOH, pKa = 4.7) is neutralized by dissolving NaOH(s) (a strong base) in the solution. Estimate the pH at the equivalence point of the neutralization process: 4.7 7.0 9.3 Which one of the following

    asked by bekah on March 31, 2014

More Similar Questions