A beaker with 1.40x10² 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 8.30 mL of a 0.490 M HCl solution to the beaker. How much will the pH change? The pK, of acetic acid is 4.740. ) Express your answer numerically to two decimal places. Use a minus ( sign if the pH has decreased.

A beaker with 1.40x10² 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 8.30 mL of a 0.490 M HCl solution to the beaker. How much will the pH change? The pK, of acetic acid is 4.740. ) Express your answer numerically to two decimal places. Use a minus ( sign if the pH has decreased.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

A solution of an unknown weak base (0.495 g in 100 mL of water) was prepared and titrated with standardized 0.113 M HCÌi and the pH of the solution was plotted as a function of titrant added (shown below). Titration of a Weak Base With 0.113 M HCI 12 10 10 20 30 40 50 60 70 80 90 Volume of HCl added (ml) Possible identities for the three liquid bases are shown in the table below. Base pyrole pyrimidine pyridine triethylamine 2.51 x 10-14 1.25 x 10-13 1.70 x 10-9 5.30 x 104 Density (g/mL) 0.967 1.02 0.982 0.762 Based on the data above, identify the weak base and explain your selection. The best explanations will account for all relevant experimental data. Additionally, suggest an indicator to use for this titration if it were to be done without a pH meter. Hd
Near the equivalence point in the titration of a strong acid with a strong base, one drop of base can cause the pH of the solution in the flask to change from 6.0 to 8.0. What is the relationship between the hydrogen ion concentrations at the two pH values? (A) The [H+] would be 100 times higher at pH 8.0 than 6.0. (B) The [H+] would be 200 times higher at pH 6.0 than 8.0. (C) The [H+] would be 2 times higher at pH 6.0 than 8.0. (D) The [H+] would be 2 times higher at pH 8.0 than 6.0. (E) The [H+] would be 100 times higher at pH 6.0 than 8.0.
A chemistry graduate student is given 250, ml, of a 1.30 M pyridine (C5H5N) solution, Pyridine is a weak base with Kg = 1.7 x10^-9. What mass of C5H5NHBr should the student dissolve in the C5H5N solution to turn it into a buffer with pH = 5.227 You may assume that the volume of the solution doesn't change when the C5H5NHBr is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.
A beaker with 195 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 MM. A student adds 7.70 mLmL of a 0.440 MM HClHCl solution to the beaker. How much will the pH change? The pKapKa of acetic acid is 4.740. Express your answer numerically to two decimal places. Use a minus ( −− ) sign if the pH has decreased.
A beaker with 2.00x102 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 0.380 M HCl solution to the beaker. How much will the pH change? The pK, of acetic acid is 4.740.
A chemistry graduate student is given 500. mL of a 1.80M hydrocyanic acid (HCN) solution. Hydrocyanic acid is a weak acid with K,= 4.9 x 10 – 10 What mass of KCN should the student dissolve in the HCN solution to turn it into a buffer with pH =9.70? You may assume that the volume of the solution doesn't change when the KCN is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. 国国回
How many moles of potassium hydroxide would have to be added to 125 mL of a 0.438 M hydrocyanic acid solution, in order to prepare a buffer with a pH of 9.090? moles
The stockroom contains 1M NaAc (Sodium Acetate), 1M HAc (Acetic Acid), distilled water and strong acids and bases. You need to create a buffer solution that has a pH of 4.75 such that when 1ml of 10M HCI is added to 100ml of your buffer, the resulting pH is 3.75 (+/-0.1). What concentrations of HAc and NaAc do you need to create the buffer solution?
A buffer is made with 0.50 M weak acid and 0.50 M sodium salt of the conjugate base. The pKa of the weak acid is 9.30 After the addition of a small amount of strong concentrated acid, the new equilibrium concentrations are 0.6 M weak acid and 0.4 M base. Calculate the new pH. Enter result with 2 decimal places, digits only.
A 5.145 g sample of a solid, weak, monoprotic acid is used to make a 100.0 mL solution. 27.00 mL of the resulting acid solution is then titrated with 0.09636 M NaOH. The pH after the addition of 16.00 mL of the base is 5.75, and the endpoint is reached after the addition of 45.85 mL of the base. (a) How many moles of acid were present in the 27.00 mL sample?4.42e-3 mol(b) What is the molar mass of the acid?314 g/mol(c) What is the pKa of the acid? (only confused on part c, answers for a and b are given)
A chemistry graduate student is given 100. mL of a 0.90M hydrocyanic acid (HCN) solution. Hydrocyanic acid is a weak acid with K,=4.9 × 10 10 What mass of KCN should the student dissolve in the HCN solution to turn it into a buffer with pH = 8.97? You may assume that the volume of the solution doesn't change when the KCN is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.