Be sure to answer all parts.What is the [H3O+] and the pH of a benzoic acid-benzoate buffer that consists of 0.20 M C6H5COOHand 0.41 M C6H5COONa? (K of benzoic acid = 6.3 × 10−5) Be sure to report your answer to thecorrect number of significant figures.[H3O+] =pH =× 10M

Answered: Be sure to answer all parts. What is…

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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The answer I got was 13.33 but that's not correct
The temperature for each solution is carried out at approximately 297 K where Kw=1.00 x 10-14- a) 0.20 g of hydrogen chloride (HCl) is dissolved in water to make 4.5 L of solution. What is the pH of the resulting hydrochloric acid solution? Express the pH numerically to two decimal places. b) 0.70 g of sodium hydroxide (NaOH) pellets are dissolved in water to make 3.0 L of solution. What is the pH of this solution? Express the pH numerically to two decimal places.
10 An analytical chemist is titrating 180.7 mL of a 0.5200M solution of piperidine (C5H₁0NH) with a 0.8300M solution of HIO3. The p K² of piperidine is 2.89. Calculate the pH of the base solution after the chemist has added 37.7 mL of the HIO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HIO3 solution added. Round your answer to 2 decimal places. G 4 = 0 X 3
An analytical chemist is titrating 149.0mL of a 0.2200M solution of piperidine C5H10NH with a 0.3200M solution of HNO3 . The pKb of piperidine is 2.89 .Calculate the pH of the base solution after the chemist has added 113.4mL of the HNO3 solution to it. Round your answer to 2 decimal places.
Calculate the pH of a buffer solution made by combining 0.069 M formic acid (HCO₂H, K₂ = 1.8x10-4) and 0.046 M lithium formate. Report your answer with the correct number of significant figures.
An unknown concentration of formic acid (HCOOH, Ka = 1.8 x 10^-4 M) is titrated with NaOH. If a 0.150 M solution of NaOH requires 35 mL of NaOH to neutralize 15.0 mL of the formic acid,calculate the concentration of the acid.Calculate the pH of the solution at the titration’s end point.
A chemist titrates 140.0 mL of a 0.4430 M hydrochloric acid (HCI) solution with 0.4963 M NaOH solution at 25 °C. Calculate the pH at equivalence. 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 NaOH solution added. PH =0 × 9
Determine the pH at the equivalence point in titration of 25.0 mL of 0.690 M HCOOH with 0.18 M NaOH. The Ka of HCOOH is 1.8 × 10−4.HCOOH (aq) + NaOH (aq) → NaHCOO (aq) + H2O (l)
25.00 mL of a 0.22M C6H5COOH(KA = 6.3x10-5) is titrated with a 0.15 M NAOH solution. What is the pH of the solution after 23.4 mL of NaOH is added? A Moving to another question will save this response. «< Question 3 of 7 24:01 hulu & 5 Σ
The weak base trimethylamine has a chemical formula (CH3)3N and a Kb = 6.4×10-5. Determine the pH of the titration of 100.0 mL of a 0.263 M solution of trimethylamine after 83.5 mL of 1.0 M HCl has been added.
A chemist titrates 250.0 mL of a 0.2431M dimethylamine ((CH3)₂NH) solution with 0.4945M HNO3 solution at 25 °C. Calculate the pH at equivalence. The p K₂ of dimethylamine is 3.27. 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 HNO3 solution added. pH = X Ś alla 18 Ar

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Be sure to answer all parts. What is the [H3O+] and the pH of a benzoic acid-benzoate buffer that consists of 0.20 M C6H5COOH and 0.41 M C6H5COONa? (K of benzoic acid = 6.3 × 10−5) Be sure to report your answer to the correct number of significant figures. [H3O+] = pH = × 10 M