Answered: 9. Compare and explain the…

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Chemistry

9. Compare and explain the regiochemical outcomes of the following reactions: PBrs (xs.) مور OH OH HBr (xs.)

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter14: Acid- Base Equilibria

Section: Chapter Questions

Problem 1ALQ: What are the major species in solution after NaHSO4 is dissolved in water? What happens to the pH of...

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You found a bottle of aqueous solution in the laboratory cabinet. Unfortunately, the label has been eroded and you could not recognize it. To the best of your recollection, it may be one of the following solutions:  HCl  CH3COOH  CH3CH2COOH  A mixture of HF and NaF (both of substantial amount)  A mixture of H3PO4 and NaH2PO4 (both of substantial amount)  NH4Cl  NaHCO3 In order to identify the solution, you conduct the following experiments: Using a pH meter, you determine the pH of the solution to be 3.00. You dilute 20 mL of the solution with water to a total volume of 200 mL and measure the pH again, this time it reads 3.50. You take some volume of the solution, add phenolphthalein, and titrate it with NaOH solution until the mixture turns pink. You record the volume of the required titrant as Vt and the pH meter reads 9.05. In a separate flask, you take the same volume of the unknown solution as in step iii and titrate it with the same NaOH…
The odor of fish is due primarily to amines, especially methylamine(CH3NH2). Fish is often served with a wedge oflemon, which contains citric acid. The amine and the acidreact forming a product with no odor, thereby makingthe less-than-fresh fish more appetizing. Calculate the equilibrium constant for the reaction of citric acid with methylamine, if only the firstproton of the citric acid (Ka1) is important in the neutralizationreaction.
19. Consider the Ka values for the following acids: Cyanic acid, HOCN, 3.5 × 10 Formic acid, HCHO2, 1.7 × 104 Lactic acid, HC;H5O3, 1.3 × 104 Propionic acid, HC3H5O2, 1.3 × 10-5 Benzoic acid, HC;H5O2, 6.3 x 10-5 Given initially equimolar solutions of each weak acid, which solution will have the highest pH once equilibrium is established? a) НОCN b) HC;H5O2 c) HC3H5O2 d) HC3H5O3 e) HCHO2 f) same pH for all
You found a bottle of aqueous solution in the laboratory cabinet. Unfortunately, the label has been eroded and you could not recognize it. To the best of your recollection, it may be one of the following solutions:  HCl  CH3COOH  CH3CH2COOH  A mixture of HF and NaF (both of substantial amount)  A mixture of H3PO4 and NaH2PO4 (both of substantial amount)  NH4Cl  NaHCO3 In order to identify the solution, you conduct the following experiments: Using a pH meter, you determine the pH of the solution to be 3.00. You dilute 20 mL of the solution with water to a total volume of 200 mL and measure the pH again, this time it reads 3.50. You take some volume of the solution, add phenolphthalein, and titrate it with NaOH solution until the mixture turns pink. You record the volume of the required titrant as Vt and the pH meter reads 9.05. In a separate flask, you take the same volume of the unknown solution as in step iii and titrate it with the same NaOH…
You found a bottle of aqueous solution in the laboratory cabinet. Unfortunately, the label has been eroded and you could not recognize it. To the best of your recollection, it may be one of the following solutions: HCl CH3COOH CH3CH2COOH A mixture of HF and NaF (both of substantial amount) A mixture of H3PO4 and NaH2PO4 (both of substantial amount) NH4Cl NaHCO3 In order to identify the solution, you conduct the following experiments: i.Using a pH meter, you determine the pH of the solution to be 3.00. ii. You dilute 20 mL of the solution with water to a total volume of 200 mL and measure the pH again, this time it reads 3.50. iii. You take some volume of the solution, add phenolphthalein, and titrate it with NaOH solution until the mixture turns pink. You record the volume of the required titrant as Vt and the pH meter reads 9.05. iv. In a separate flask, you take the same volume of the unknown solution as in step iii and titrate it with the same NaOH solution, but this time…
You found a bottle of aqueous solution in the laboratory cabinet. Unfortunately, the label has been eroded and you could not recognize it. To the best of your recollection, it may be one of the following solutions:  HCl  CH3COOH  CH3CH2COOH  A mixture of HF and NaF (both of substantial amount)  A mixture of H3PO4 and NaH2PO4 (both of substantial amount)  NH4Cl  NaHCO3 In order to identify the solution, you conduct the following experiments: Using a pH meter, you determine the pH of the solution to be 3.00. You dilute 20 mL of the solution with water to a total volume of 200 mL and measure the pH again, this time it reads 3.50. You take some volume of the solution, add phenolphthalein, and titrate it with NaOH solution until the mixture turns pink. You record the volume of the required titrant as Vt and the pH meter reads 9.05. In a separate flask, you take the same volume of the unknown solution as in step iii and titrate it with the same NaOH…
You found a bottle of aqueous solution in the laboratory cabinet. Unfortunately, the label has been eroded and you could not recognize it. To the best of your recollection, it may be one of the following solutions: HCl CH3COOH CH3CH2COOH A mixture of HF and NaF (both of substantial amount) A mixture of H3PO4 and NaH2PO4 (both of substantial amount) NH4Cl NaHCO3 In order to identify the solution, you conduct the following experiments: 1. Using a pH meter, you determine the pH of the solution be 3.00. 2. You dilute 20 mL of the solution with water to a total volume of 200 mL and measure the pH again, this time it reads 3.50. 3. You take some volume of the solution, add phenolphthalein, and titrate it with NaOH solution until the mixture turns pink. You record the volume of the required titrant as Vt and the pH meter reads 9.05. ti =0.0 and tf=2.0. 4. In a separate flask, you take the same volume of the unknown solution as in step iii and titrate it with the same NaOH…
A. Write all the equilibrium reactions with the corresponding equilibrium constant values for a diprotic acid, H;S in an aqueous solution. Ka, = 9.5 x 10 Kaz =1.3 x 1014 B. Given the following compounds: H;S (34.065); NaHS (56.065); Na,S (78.065), calculate the pH of a buffer solution (with a usable pH range) prepared by mixing 1.00 g of the acid and 1.200 g of its conjugate base and diluting to 1.00 L. c. Calculate the new pH of the buffer solution in (b) if 5.00 mL of 1.07 M HCl were added to the buffer prepared in (B). D. In a laboratory where NaHS and HCI are the only available reagents, how many mL of 1.00 M HCl should be added to a 50.0 ml solution containing 1.00 mmol of NaHS to give a buffer solution with a pH of 7.022.
Please write the balanced chemical equations on the observations of heating NaHCO3 and bubbling the gas made by decomposition through the Ca(OH)2 solution in the presence of bromothymol (blue acid base indicator solution) Please write out in chemical equation form!
Consider the titration of the weak acid, benzoic acid, HC7H5O2. Its acid dissociation reaction is: HC7H5O2 (aq) + H2O (l) ↔ C7H5O2- (aq) + H3O+ (aq) A 25.00 mL sample of a solution of benzoic acid, concentration unknown, is titrated with 0.0500M NaOH solution. A plot of the titration is shown below. 1. what is the pKa (approximately) of benzoic acid? Its Ka? 2. on the plot, indicate the buffering region of the titration 3. From the pH at the equivalence point, estimate the pKb of benzoate ion (conjugate base to benzoic acid)______________[Remember, at the equivalence point, C7H5O2- (aq) + H2O (l) ↔ HC7H5O2 (aq) + OH- (aq) ]
5. Acetic acid was dissolved in water to a concentration of 0.10 mol.L-!. The pKa of acetic acid is 4.8. а. What are the chemical species in solution at equilibrium? b. What is the pH of the solution at equilibrium? What are the concentrations of each reactant and product (except water) at equilibrium? с.
2. Explain why the observed color change with bromcresol green for each of the four solutions is reasonable given the pH. a. NaC.pH=7 b. Na;CO, pH =10.8 c. NaC;H,O, .pH-8.9 d. NaHSO.pH-1.5 Part C: 1. What was the unknown weak acid? From your observed pH calculate the [H+] concentration in M(mols/L) for your unknown acid 2. Calculate the Ka for the unknown acid