Chemistry

10. A weak acid with an initial pH of 3.2 was titrated with a strong base. 15 mL of 0.1 M NaOH was added to the acid to reach the equivalence point at a pH of 8.6. What would you expect the approximate pH of the analyte to be after the first 5 mL of 0.1 M NaOH was added?

8.6

3.4

5.1

7.2

  1. 👍
  2. 👎
  3. 👁
  1. I would choose 5.1. If one third of the base is added (in which the whole 15ml was utilized to bring to a basic state of 8.6), it must be 5.1, as the other answers are mathematically impossible.

    1. 👍
    2. 👎

Respond to this Question

First Name

Your Response

Similar Questions

  1. science

    Which acid-base chemical reaction is irreversible?(1 point) strong acid added to water water on its own weak base added to water weak acid added to water Hydrochloric acid is a strong acid. Acetic acid is a weak acid. Which

  2. Chemistry

    Select the statements that correctly describe buffers.? 1) The pH of a buffer solution does not change significantly when any amount of a strong acid is added. 2) The Ka of a buffer does not change when any amount of an acid is

  3. chemistry

    Is this a buffer system? NH3/(NH4)2SO4? It is formed by mixing NH3 (weak base) and a strong acid (H2SO4), but according to my worksheet it is not a buffer system. Why is this so? Isnt it a buffer as long as it consists of a weak

  4. CHEMISTRY

    HOW CAN U TELL IF HNO3 +KNO3 IS A BUFFER SOLUTION A buffer solution must contain a weak acid and its conjugate base OR a weak base and its conjugate acid. HNO3 is a strong base and KNO3 is the salt of a strong base (KOH) and a

  1. Chemistry

    Which of the following statements are true about a strong base and a weak base at a pH of 11? A) HCl will not bring the pH of either solution to pH 7. B) Both bases require the same amount of HCl to reach pH 7 because they are

  2. chemistry

    Strong base is dissolved in 665 mL of 0.400 M weak acid (Ka = 3.69 × 10-5) to make a buffer with a pH of 3.94. Assume that the volume remains constant when the base is added. HA(aq) + OH-(aq) -> H2O(l) + A-(aq) Calculate the pKa

  3. Chemistry: Equilbrium

    2. Which of the following statements are true about a strong base and a weak base at a pH of 11? HCl will not bring the pH of either solution to pH 7. Both bases require the same amount of HCl to reach pH 7 because they are both

  4. Chemistry

    A substance of Ka of 1 x 10^–5 would be classified as a ____. A.strong acid B.weak acid C.strong base D.weak base I think it is B...?

  1. chemistry- check!

    1. A pure salt solution can be any of the following except a. basic b. buffered *** c. alkaline c. acidic 2. You can make a buffer with all the following except a. weak acid + conjugate base b. weak base + salt of weak base c.

  2. Chemistry

    A weak acid with a Ka of 1.8 × 10–5 is titrated with a strong base. During the titration,12.5 mL of 0.10 M NaOH is added to 50.0 mL of 0.100 M acetic acid. What is the pH after the addition of the NaOH? A. 7.22 B. 5.13 C. 4.26

  3. chemistry

    A. Strong Base 1.) What is the concentration of a solution of KOH for which the pH is 11.89? 2.) What is the pH of a 0.011M solution of Ca(OH)2? B. Weak Acid 1.) The pH of a 0.060M weak monoprotic acid HA is 3.44. Calculate the Ka

  4. Chemistry

    HOBr (aq) H+ (aq) + OBr- (aq), Ka = 2.3 x 10^-9 Hypobromous acid, HOBr, is a weak acid that dissociates in water, as represented by the equation. (a) Calculate the value of [H+] in a solution of HOBr that has a pH of 4.95. Ans:

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