A beaker with 1.70x102 mL of an acetic acid buffer with a pH of 5.000 is sitting on a benchtop. The total molarity of acid and conjugate base in this buffer is 0.100 M. A student adds 8.90 mL of a 0.370 M HCI solution to the beaker. How much will the pH change? The pKa of acetic acid is 4.740. Express your answer numerically to two decimal places. Use a minus (- ) sign if the pH has decreased. > View Available Hint(s) ApH = Submit

A beaker with 1.70x102 mL of an acetic acid buffer with a pH of 5.000 is sitting on a benchtop. The total molarity of acid and conjugate base in this buffer is 0.100 M. A student adds 8.90 mL of a 0.370 M HCI solution to the beaker. How much will the pH change? The pKa of acetic acid is 4.740. Express your answer numerically to two decimal places. Use a minus (- ) sign if the pH has decreased. > View Available Hint(s) ApH = Submit

Introductory Chemistry For Today

8th Edition

ISBN:9781285644561

Author:Seager

Publisher:Seager

Chapter9: Acids, Bases, And Salts

Section: Chapter Questions

Problem 9.116E

See similar textbooks

Similar questions

Which of these buffers involving a weak acid HA has the greater resistance to change in pH? Explain your answer. (i) [HA] =0.100 M = [A] (ii) [HA] = 0.300 M = [A]
Fifty cm3 of 1.000 M nitrous acid is titrated with 0.850 M NaOH. What is the pH of the solution (a) before any NaOH is added? (b) at half-neutralization? (c) at the equivalence point? (d) when 0.10 mL less than the volume of NaOH to reach the equivalence point is added? (e) when 0.10 mL more than the volume of NaOH to reach the equivalence point is added? (f) Use your data to construct a plot similar to that shown in Figure 14.10 (pH versus volume NaOH added).
Two acids, each approximately 0.01 M in concentration, are titrated separately with a strong base. The adds show the following pH values at the equivalence point: HA, pH = 9.5, and HB, pH = 8.5. (a) Which is the stronger acid, HA or HB? (b) Which of the conjugate bases, A or B, is the stronger base?
A 0.2481 M solution of KOH is used to titrate 30.00 mL of 0.269 M hydrobromic acid. Assume that volumes are additive. (a) Write a balanced net ionic equation for the reaction that takes place during the titration. (b) What are the species present at the equivalence point? (c) What volume of KOH is required to reach the equivalence point? (d) What is the pH of the solution 1. before any KOH is added? 2. halfway to the equivalence point? 3. at the equivalence point?
A beaker with 1.50×102 mL of an acetic acid buffer with a pH of 5.000 is sitting on a benchtop. The total molarity of acid and conjugate base in this buffer is 0.100 M. A student adds 6.70 mL of a 0.390 M HCl solution to the beaker. How much will the pH change? The pKa of acetic acid is 4.740.
A beaker with 1.0 x 10^2 mL of an acetic acid buffer with a pH of 5.000 is sitting on a benchtop. The total molarity of acid and conjugate base in this buffer is 0.100 M. A student adds 8.80 mL of a 0.360 M HCl solution to the beaker. How much will the pH change? The pKa of acetic acid is 4.740.
A beaker with 155 mL of an acetic acid buffer with a pH of 5.000 is sitting on a benchtop. The total molarity of acid and conjugate base in this buffer is 0.100 M. A student adds 7.80 mL of a 0.450 M HCl solution to the beaker. How much will the pH change? The pKa of acetic acid is 4.740. Express your answer numerically to two decimal places
A beaker with 165 mL of an acetic acid buffer with a pH of 5.000 is sitting on a benchtop. The total molarity of acid and conjugate base in this buffer is 0.100 M . A student adds 4.50 mL of a 0.370 M HCl solution to the beaker. How much will the pH change? The pKa of acetic acid is 4.740. Express your answer numerically to two decimal places. Use a minus ( −− ) sign if the pH has decreased.
A student titrates 20.0 mL of 1.84 M HCl with a weak base (Kb = 2.33 x 10−6). The weak base and HCl react in a 1:1 ratio. a.Determine the molarity of the weak base if 32.7 mL of base was required to reach equivalence. b.Would the pH at equivalence be less than 7, greater than 7, or equal to 7? Justify your answer. c.A buffer is created using 100 mL of the weak base and 100 mL of 1.35 M salt containing the conjugate acid. Determine the pH of the buffer.
A beaker with 135 mL of an acetic acid buffer with a pH of 5.000 is sitting on a benchtop. The total molarity of acid and conjugate base in this buffer is 0.100 mol L−1. A student adds 8.60 mL of a 0.380 mol L−1 HCl solution to the beaker. How much will the pH change? The pKa of acetic acid is 4.760. Express your answer numerically to two decimal places. Use a minus ( − ) sign if the pH has decreased.
An acid–base buffer is able to resist changes in pH due to the addition of small amounts of strong acid or base to the system. An acid–base buffer typically contains a weak acid and its conjugate base. A buffer is prepared by mixing 33.2 mL of 0.209 M NaOH with 138.1 mL of 0.231 M acetic acid. What is the pH of this buffer? (The pKa for acetic acid is 4.75.) Calculate the pH of this buffer after the addition of 0.192 g of solid NaOH.
A beaker with 1.00×102 mLmL of an acetic acid buffer with a pH of 5.000 is sitting on a benchtop. The total molarity of acid and conjugate base in this buffer is 0.100 M�. A student adds 6.50 mLmL of a 0.490 M� HClHCl solution to the beaker. How much will the pH change? The pKap�a of acetic acid is 4.740. Express your answer numerically to two decimal places. Use a minus ( −− ) sign if the pH has decreased.