Which of these compounds will be most soluble in aqueous 0.1 M NaOH? The solubility of a compound is enhanced by favourable non-covalent interactions with the water. A deprotonation reaction is possible for one of these compounds that leads to an ionic compound. Ions have very strong non-covalent interactions with water. Select one: O₂N CO₂H

Which of these compounds will be most soluble in aqueous 0.1 M NaOH? The solubility of a compound is enhanced by favourable non-covalent interactions with the water. A deprotonation reaction is possible for one of these compounds that leads to an ionic compound. Ions have very strong non-covalent interactions with water. Select one: O₂N CO₂H

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

Chapter15: 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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What are the major species in solution after NaHSO4 is dissolved in water? What happens to the pH of the solution as more NaHSO4 is added? Why? Would the results vary if baking soda (NaHCO3) were used instead?
Weak base B has a pKb of 6.78 and weak acid HA has a pKa of 5.12. a Which is the stronger base, B or A? b Which is the stronger acid, HA or BH+? c Consider the following reaction: B(aq)+HA(aq)BH+(aq)+A(aq) Based on the information about the acid/base strengths for the species in this reaction, is this reaction favored to proceed more to the right or more to the left? Why? d An aqueous solution is made in which the concentration of weak base B is one half the concentration of its acidic salt, BHCl, where BH+ is the conjugate weak add of B. Calculate the pH of the solution. e An aqueous solution is made in which the concentration of weak acid HA twice the concentration of the sodium salt of the weak acid, NaA. Calculate the pH of the solution. f Assume the conjugate pairs B/BH+ and HA/A are capable of being used as color-based end point indicators in acidbase titrations, where B is the base form indicator and BH is the acid form indicator, and HA is the acid form indicator and A is the base form indicator. Select the indicator pair that would be best to use in each of the following titrations: (1) Titration of a strong acid with a strong base. (i) B/BH+ (ii) HA/A (2) Titration of a weak base with a strong acid. (i) B/BH+ (ii) HA/A
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.
24. A solution of volume 0.500 L contains 1.68 g NH3 and 4.05 g (NH4)2SO4. (a) What is the pH of this solution? (b) If 0.88 g NaOH is added to the solution, what will be the pH? (c) How many milliliters of 12 M HCl must be added to 0.500 L of the original solution to change its pH to 9.00?
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 mol and at 25 °C has a pKa of 5.4.
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…
A solution of ammonium sulfate was prepared by dissolving 55.44g of (NH4)2SO4 in enough water to prepare a 2.00L solution. What is the concentration of ammonium ions in this solution?
Methanoic acid is also called formic acid. It has the chemical formula HCOOH(l). It is a colourless fuming liquid that is mainly used as a preservative. It exhibits the following equilibrium in water:HCOOH(aq) + H2O(l) → HCOO–(aq) + H3O+(aq) 1) A 4.50 g tablet of magnesium hydroxide neutralizes 400.0 mL of stomach acid, HCl. What is the concentration of HCl in the stomach? PLEASE HELP WITH THIS ITS EXTREMELY URGENT
k= 6.33 × 10−3 L·mol−1·s−1. If the initial concentration of XY is 0.150 mol·L−1, how long will it take for the concentration to decrease to 6.25 × 10−2 mol·L−1 ?
A chemical system is set up by placing some solid ammonium chloride in an ammonia solution. The equilibrium established can be represented as follows: NH4*(aq) + H2O(e) 2 H30*(aq) + NH3(aq) The pH of the solution is taken, then a small amount of NaOH(aq) is added and the pH is taken again. What can be said about the change in pH for the solution? The pH significantly increases because a strong base has been added to the solution. The pH significantly decreases because a strong base has been added to the solution. There is very little change to the pH of the solution. If anything the pH of the solution decreases slightly. There is very little change to the pH of the solution. If anything the pH of the solution increases slightly.
Apart from the identity of the central atom, what is the major difference between NH4+ and CH4? How does this difference affect the relative solubility of the compounds in water?

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