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- Complete each of these reactions by filling in the blanks. Predict whether each reaction is product-favored or reactant-favored, and explain your reasoning. (a) _________ (aq) + Br(aq) NH3(aq) + HBr(aq) (b) CH3COOH(aq) + CN(aq) ________ (aq) + HCN(aq) (c) ________ (aq)+H2O () NH3(aq) + OH(aq)Most naturally occurring acids are weak acids. Lactic acid is one example. CH3CH(OH)CO2H(s)+H2O(l)H3O+(aq)+CH3CH(OH)CO2(aq) If you place some lactic acid in water, it will ionize to a small extent, and an equilibrium will be established. Suggest some experiments to prow that this is a weak acid and that the establishment of equilibrium is a reversible process.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: 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…
- ■ What is the product of the following reaction OH CrO3/H2SO4 ■ What are the reaction conditions to produce an acid from this reactant: OHYou 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…Give the products in the following acid-base reactions. Identify the conjugate acid-base pairs.
- When the reaction below reaches equilibrium, does the equilibrium lie on the left or the right side? Briefly explain.ClO– + CH3CO2H ⇌ HClO + CH3CO2–Predict the position of equilibrium and calculate the equilibrium constant, Keq, for each acid-base reactionComplete the following acid-base reaction: HC≡CH + NaH =
