this question. Calculate the pH of a solution that is prepared by dissolving 0.168 mol of pentafluorobenzoic acid (C,FCOOH, K = 3.30x102) and 0.350 mol of HCIO, and CIO". Do not make an approximation unless the initial acid concentration is greater than 1000 xK. (Hint: The pH will be determined by the stronger acid of this pair.) hypochlorous acid (HCIO, K,=3.00x10) in water and diluting to 2.50 L. Also, calculate the equilibrium concentrations of C,F;COOH, C¿F;COO", %3D pH = [C,F;COOH] = M [C,F;CO0] = M [HCIO] = M

this question. Calculate the pH of a solution that is prepared by dissolving 0.168 mol of pentafluorobenzoic acid (C,FCOOH, K = 3.30x102) and 0.350 mol of HCIO, and CIO". Do not make an approximation unless the initial acid concentration is greater than 1000 xK. (Hint: The pH will be determined by the stronger acid of this pair.) hypochlorous acid (HCIO, K,=3.00x10) in water and diluting to 2.50 L. Also, calculate the equilibrium concentrations of C,F;COOH, C¿F;COO", %3D pH = [C,F;COOH] = M [C,F;CO0] = M [HCIO] = M

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

At 25oC, a 1-L buffer solution is prepared by mixing acetic acid and sodium acetate.A) If the solution is to be buffered at pH = 5, what should be the molar ratio of sodium acetate to acetic acid?B) If the buffer is found to be 1.50M in acetic acid and 1.75M in sodium acetate, what will be the pH of the solution?C) If 0.05 mol of NaOH was added to the solution in B, what will be the pH of the solution?D) If the pH of the solution in B is 4.55, how many moles of HCl was added to the solution?
A solution is prepared that is initially 0.095 M in methylamine (CH,NH,), a weak base, and 0.38M in methylammonium chloride (CH,NH,CI). Complete the reaction table below, so that you could use it to calculate the pH of this solution. Use x to stand for the unknown change in [OH ]. You can leave out the M symbol for molarity. ОН [CH,NH.] [cH,NH;] [on ] initial change final
Kk.84.
Metabolic acidosis. As we will see later in the course, pathological conditions arise where the blood pH falls because of excess acid production, a condition called metabolic acidosis. Excess protons in the blood decrease the amount of HCO3− and thus reduce the buffering capacity of blood. A rapid drop in pH could lead to death. Normal values for blood are: pH = 7.4, [HCO3−] = 24.0 mM, [CO2] = 1.20 mM.✓ 6 (a) If a patient has a blood pH = 7.03 and [CO2] = 1.2 mM, what is the [HCO3−] in the patient’s blood? The pKa of HCO3−= 6.1. (b) Suggest a possible treatment for metabolic acidosis. (c) Why might the suggestion for part (b) be of benefit to middle-distance runners?
Calculate the pH at the following points in a titration of 40. mL (0.040 L) of 0.145 M 4-chlorobenzoic acid (Ka = 1.0 ✕ 10−4) with 0.145 M KOH. (Assume Kw = 1.01 ✕ 10−14.) When 40. mL of KOH solution added?
A chemist titrates 110.0 mL of a 0.1235M butanoic acid (HC,H,CO,) solution with 0.0643 M KOH solution at 25 °C. Calculate the pH at equivalence. The pK, of butanoic acid is 4.82. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of KOH solution added. pH = ] ? %3D
Calculate the pH of a 1.07 M solution of a weak acid, AH, for instance CH3COOH, and 0.62 M of a salt derived by its conjugate base, ANa, like CH3COONa. The acid dissociation constant, Ka , is 2.27e-6. What is the pH if 38 mL of 0.149 M of a strong acid, like HCl, is added to 100 mL of the buffer solution? What if a strong base, like NaOH, is added with the same ammount instead ? pH ← please insert your values Add acid = _______ Add base = _________
A solution is prepared at 25 °C that is initially 0.47 Min dimethylamine ((CH,) NH), a weak base with K, =5.4 x 10 , and 0.25 M in dimethylammonium 9. chloride ((CH, NH,CI). Calculate the pH of the solution. Round your answer to 2 decimal places. pH = |
A solution is prepared that is initially 0.41 M in trimethylamine ((CH N, a weak base, and 0.40M in trimethylammonium bromide ((CH,)¸NHB"). Complete the reaction table below, so that you could use it to calculate the pH of this solution. Use x to stand for the unknown change in [OH]. You can leave out the M symbol for molarity. [CH.),N] [CH),NH] [on] initial change final olo X O O
A solution contains 0.397 M HA (K₂ = 8.08 - 10-6) and 0.719 M NaA. What is the pH of this solution? What is the pH of this solution after 0.167 mol of HCl are added to 1.00 L of this solution? What is the pH of this solution after 0.334 mol of HCl are added to 1.00 L of this solution?
An analytical chemist is titrating 243.8 mL of a 0.7000 M solution of butanoic acid (HC3H,CO2) with a 0.3800 M solution of NaOH. The pK of butanoic acid is 4.82. Calculate the pH of the acid solution after the chemist has added 278.5 mL of the NaOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of NaOH solution added. Round your answer to 2 decimal places. PH ☐ olo Ar
An analytical chemist is titrating 247.8 ml. of a 0.6300M solution of nitrous acid (HNO₂) with a 0.9300M solution of NaOH. The pK, of nitrous acid is 3.35. Calculate the pH of the acid solution after the chemist has added 118.8 ml. of the NaOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of NaOH solution added. Round your answer to 2 decimal places. pH- 0 G