A technician finds the molar mass to be 134.8 g/mol and the pK, to be 4.65 after processing a data set for a solid acid unknown. Based on the previous information and the list of acid unknowns in the Laboratory Manual, what is the best call the student can make for the identity of the solid acid unknown? picolinic acid para-aminobenzoic acid. glutamic acid monohydrate D potassium hydrogen phosphate, monobasic O A. O B. OC. O D.

A technician finds the molar mass to be 134.8 g/mol and the pK, to be 4.65 after processing a data set for a solid acid unknown. Based on the previous information and the list of acid unknowns in the Laboratory Manual, what is the best call the student can make for the identity of the solid acid unknown? picolinic acid para-aminobenzoic acid. glutamic acid monohydrate D potassium hydrogen phosphate, monobasic O A. O B. OC. O D.

Introductory Chemistry For Today

8th Edition

ISBN:9781285644561

Author:Seager

Publisher:Seager

Chapter9: Acids, Bases, And Salts

Section: Chapter Questions

Problem 9.142E

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A substance that functions to prevent rapid, drastic changes in the pH of a body fluid by changing strong acids and bases into weak acids and bases is called an: a.salt. b.buffer. c.enzyme. d.coenzyme.
Unknown Acid Acid name Acetic acid Group #5 Group #6 Group #7 Mean Standard Deviation % Error STATISTICAL ANALYSIS: Calculate mean values for molar mass, pKa, and Ka. Calculate % error and standard deviation: Unknown acid # 1 Molar Mass of unknown acid (calculated), g/mol Group #1 Group #2 Group #3 Group #4 Reaction Initial conc. / M: Change in conc. at equilibrium / M: Equilibrium conc. / M: Acetic acid | Molar Mass, g/mol: 60.05 | pka = 4.76 Accepted Values Molar mass, g/mol 60.05 Ka = Part II 1. Using initial molarity of acid and measured pH of the acid before titration, build a RICE table and calculate the Ka of the acid. You can use examples 1, 2 (pp. 3-4) from the Manual (posted on Canvas) Initial Molarity of [HA], M 0.219 Initial pH of Acid pka = HA(aq) + H₂O(1) [HA] -X 58.8 57.4 60.4 61.0 58.4 59.2 59.7 59.3 1.13 0.01 [HA] + X 台 pH: H3O+ (aq) = 0 +X 2. Use the Henderson-Hasselbauch equation to perform the same calculation. +X pka 4.76 Ka = pka 4.78 5.00 4.64 4.89 4.62 4.68 4.82…
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Provide explanation of correct and incorrect option. please do not provide solution based on AI.
A 0.100M succinic acid solution (diprotic acid: Kal = 6.21E-5, Ka2 = 2.31E-6) at pH 5, calculate the [H₂A], [HA], and [A²-]. A) [H2A] = 0.0999, [HA-] = 6.21E-5, [A2-] = 1.43E-9 B) [H2A] = 0.0116, [HA-] = 0.0718, [A2-] = 0.0166 C) [H2A] = 6.9E-8, [HA-] = 4.31E-4, [A2-] = 0.996 D) [H2A] = 0.0266, [HA-] = 0.0631, [A2-] = 0.0103
When ammonium (NH4*) is placed in water, a chemical reaction occurs and an equilibrium is established as shown below. NH4+ (aq) + H₂O (1) ≥ NH3 (aq) + H3O+ (aq) The pK, of NH4* is 9.25. Predict whether the acid form (NH4*) or the base form (NH3) is predominant at pH = 7.4. Explain your answer.
please explain the process and answer Mouthwash acts to clean and disinfect mouths. Two important considerations when designing a mouthwash solution are the pH, which should ideally not be too acidic (where saliva has a normal pH range of 6.2–7.6 and below pH 5.5 erosion may occur), and the resistance of the solution to changes in pH. One example of a buffering system used in mouthwash is based on the compound H3PO4 which has PKa values of 2.1, 7.2 and 12.3. i. Hand-draw the structure of the main phosphorus species at pH 7.0, as well as a balanced equilibrium equation showing the structures of the two main phosphoric acid species at pH 7.0.
Given for 9: A healthy individual has a blood with [H*]= 4.87× 10*. 9. What is his/her blood pH? Answer: Computation:
of 13 > A diprotic base (B) has pKg values of 3.33 (pKp1) and 6.66 (pKp2). Which of the equalities is true when the pH is 7.34? Which of the equalities is true when the pH is 10.67? [BH*] = [B] (BH? *) = [BH*) %3D %3D (BH *) = [BH*] O (BH? *1 = [B] [BH? *] = [B] %3D [BH*] = [B] %3! !! What is the predominant species of B at pH 4.40? What is the predominant species of B at pH 9.18? BH? BH? BH* BH+ What is the predominant species of B at pH 12.80? BH? BH
Gastric juice is made up of substances secreted from parietal cells, chief cells, and mucous-secreting cells. The cells secrete HCI, proteolytic enzyme zymogens, mucin, and intrinsic factor. The pH of gastric juice is acidic, between 1–3. If the pH of gastric juice is 1.1, what is the amount of energy (AG) required for the transport of hydrogen ions from a cell (internal pH of 7.4) into the stomach lumen? Assume that the potential difference across the membrane separating the cell and the interior of the stomach is –60.0 mV (inside of the cell is negative relative to the lumen of the stomach). Assume that the temperature is 37 °C. The Faraday constant is 96.5 kJ/(V-mol) and the gas constant is 8.314 x 10-3 kJ/(mol·K). Express your answer in kilojoules per mole. AG = kJ/mol
I Normal 1 No Spac.. Heading 1 Heading 2 Title Styles Paragraph 5. Fill in the following table: [H3O"] РОН [OH'] ACID or BASE pH 7.21 9.84 x 10° M 3.25 2.64 x 102 M 2.49
Gastric juice is made up of substances secreted from parietal cells, chief cells, and mucous-secreting cells. The cells secrete HCI, proteolytic enzyme zymogens, mucin, and intrinsic factor. The pH of gastric juice is acidic, between 1–3. If the pH of gastric juice is 1.9, what is the amount of energy (AG) required for the transport of hydrogen ions from a cell (internal pH of 7.4) into the stomach lumen? Assume that the potential difference across the membrane separating the cell and the interior of the stomach is –70.0 mV (inside of the cell is negative relative to the lumen of the stomach). Assume that the temperature is 37 °C. The Faraday constant is 96.5 kJ/(V-mol) and the gas constant is 8.314 x 10-3 kJ/(mol·K). Express your answer in kilojoules per mole. A = 10.68 kJ/mol