b). What is the conjugate base of NH4?c) The Ka for NH4* is 5.5x10-10. What is the pKa for its conjugate base? pKa=d) AlCl3, when dissolved in water, forms a(n) (basic or acidic) solution (Circle one).Calculate the pH at the equivalence point for the titration of 0.120 M hydrofluoric acid (HF) with0.120 M NaOH. The K, of HF is 6.8×104. (Know how to do both acid and base)

b) Conjugate base is formed when a species releases a proton (H+).NH4+ →−H+ NH3so, conjugate base of…

Answered: b). What is the conjugate base of NH4?…

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...

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An analytical chemist is titrating 225.8 mL of a 0.5300 M solution of butanoic acid (HC,H,CO,) with a 0.8200 M solution of KOH. The p K, of butanoic acid is 4.82. Calculate the pH of the acid solution after the chemist has added 40.67 mL of the KOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of KOH solution added. Round your answer to 2 decimal places. pH = ||
With the same initial solution of 0.75 moles formate and 0.85 moles formic acid to make a buffer solution. The Ka of formic acid is 1.8x10-4. You add 60.7g hydrobromic acid to this solution, what is the new pH?
An analytical chemist is titrating 111.5 mL of a 0.2600M solution of acetic acid (HCH,CO,) with a 0.5100M solution of NaOH. The p K, of acetic acid is 4.70. Calculate the pH of the acid solution after the chemist has added 10.45 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 = |
When a 18.3 mL sample of a 0.460 M aqueous hydrocyanic acid solution is titrated with a 0.330 M aqueous barium hydroxide solution, (1) What is the pH at the midpoint in the titration? (2) What is the pH at the equivalence point of the titration? (3) What is the pH after 19.1 mL of barium hydroxide have been added?
An analytical chemist is titrating 231.8 mL of a 0.9900M solution of acetic acid (HCH, CO,) with a 1.200M solution of NaOH. The p K, of acetic acid is 4.70. Calculate the pH of the acid solution after the chemist has added 131.2 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. alo pH %3| Ar Explanation Check © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use Privacy Center | Accessibility CA
#18. The sample of 25.00 mL of 0.020 M NH3 is titrated with 0.016 M HCl. (a) Show the reaction between NH3 and H+. (b) Find the volume of 0.016 M HCl needed to reach the equivalence point. (c)Show the reaction of hydrolysis of product from the step (a). (d) Calculate the pH at the equivalence point(Ka of NH4+ is 5.6 x 10–10)
a An analytical chemist is titrating 69.9 mL of a 0.2200M solution of cyanic acid (HCNO) with a 0.8900M solution of KOH. The pK of cyanic acid is 3.46. Calculate the pH of the acid solution after the chemist has added 5.93 mL of the KOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of KOH solution added. Round your answer to 2 decimal places. pH 0 X Ś
GW 18b 1. A 20.0 mL sample of a 0.240 M hydrofluoric acid (HF) solution is titrated with 0.200 M NaOH. Determine: (a) pH of the acid solution before any base is added; (b) volume (in mL) of base needed to get to the equivalence point; (c) pH halfway to equivalence point; (d) pH at equivalence point; (e) pH when 0.100 mL NaOH is added beyond the equivalence point. (K₂ of HF = 7.1 × 104)
Calculating the pH of a weak base titrated with a strong acid An analytical chemist is titrating 104.1 mL of a 0.1200M solution of propylamine (C,H,NH,) with a 0.2600M solution of HNO3. The p K, of propylamine is 3.46. Calculate the pH of the base solution after the chemist has added 53.1 mL of the HNO, solution to it. Note for advanced students: you may assume the final volume eguals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places. pH = Explanation Check O 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use Privacy | Accessibility APR 23 MacBook Air O00 000 F4
In this lab, we will experimentally determine the titration curve for the titration of a weak acid solution against a strong base solution. The weak acid we will use is potassium hydrogen phthalate, KHP, its chemical structure is shown below. KHP is an ionic compound composed of a potassium cation K+ and a hydrogen phthalate anion HP–. HP– is a weak acid and upon dissolving in water, can lower the pH of the solution. (a) Suggest the chemical reaction(s) when a solid sample of KHP is dissolved in water, writing out the chemical equations for them. (b) Sketch the structure of KHP from above and circle the hydrogen atom that is responsible for its acidity. (c) Calculate the pH of a solution made of 0.50 g of KHP and 50 mL of water. KHP has a molar mass of 204.2 g and at 25 °C has a pKa of 5.4.
When a 20.1 mL sample of a 0.367 M aqueous hydrocyanic acid solution is titrated with a 0.492 M aqueous barium hydroxide solution, (1) What is the pH at the midpoint in the titration? (2) What is the pH at the equivalence point of the titration? (3) What is the pH after 11.2 mL of barium hydroxide have been added?
-2 A chemistry graduate student is given 100. mL of a 0.80M chlorous acid (HCIO,) solution. Chlorous acid is a weak acid with K,=1.1 × 10 ´. What mass of KCIO, should the student dissolve in the HCIO, solution to turn it into a buffer with pH = 1.37? You may assume that the volume of the solution doesn't change when the KC10, is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. x10

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