What is the pH of a 5.62\times 10-2 M aqueous solution of potassium fluoride, KF?pH =This solution is .

Given that the concentration of potassium fluoride (KF) is 5.6×10-2 M, and KF dissociates into one…

Answered: What is the pH of a 5.62\times 10-2 M…

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter15: Solutions Of Acids And Bases

Section: Chapter Questions

Problem 15.125QE

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What is the freezing point of vinegar, which is an aqueous solution of 5.00% acetic acid, HC2H3O2, by mass (d=1.006g/cm3)?
Using the diagrams shown in Problem 10-117, which of the solutions would have the greatest buffer capacity, that is, greatest protection against pH change, when the following occurs? a. A strong acid is added to the solution. b. A strong base is added to the solution.
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.
What is a salt? List some anions that behave as weak bases in water. List some anions that have no basic properties in water. List some cations that behave as weak acids in water. List some cations that have no acidic properties in water. Using these lists, give some formulas for salts that have only weak base properties in water. What strategy would you use to solve for the pH of these basic salt solutions? Identify some salts that have only weak acid properties in water. What strategy would you use to solve for the pH of these acidic salt solutions? Identify some salts that have no acidic or basic properties in water (produce neutral solutions). When a salt contains both a weak acid ion and a weak base ion, how do you predict whether the solution pH is acidic, basic, or neutral?
Which of the diagrams in Problem 10-135 represents the substance that is the weakest electrolyte?
A solution of sodium cyanide, NaCN, has a pH of 12.10. How many grams of NaCN are in 425 mL of a solution with the same pH?
Four different substances of the generalized formula HA were dissolved in water, with the results shown in the diagrams. Which of the diagrams represents the substance that is the strongest electrolyte?
Two strategies are also followed when solving for the pH of a base in water. What is the strategy for calculating the pH of a strong base in water? List the strong bases mentioned in the text that should be committed to memory. Why is calculating the pH of Ca(OH)2 solutions a little more difficult than calculating the pH of NaOH solutions? Most bases are weak bases. The presence of what element most commonly results in basic properties for an organic compound? What is present on this element in compounds that allows it to accept a proton? Table 13-3 and Appendix 5 of the text list Kb values for some weak bases. What strategy is used to solve for the pH of a weak base in water? What assumptions are made when solving for the pH of weak base solutions? If the 5% rule fails, how do you calculate the pH of a weak base in water?
Consider a 0.020 M hypochlorous acid solution (K, = 3.0 x 10-8). pH = =
What is the pOH for a solution at 25 °C that has a H3O+ concentration of 6.57 ×10-6 M? A 34.1 % (NH4 )2SO4 (molar mass = 132.1 g mol−1) has a density of 1.15 g mL−1. What is the molarity of this solution? (the answer should be entered with 3 significant figures; do not enter units; give answer in normal notation--examples include 1.23 and 120. and -123 and 123. and 12.3) Determine the boiling point of a solution that contains 78.5 g of compound W (molar mass = 132.5 g mol–1) dissolved in 1088.6 g benzene (C6H6; molar mass = 84.156 g mol–1; Kb = 2.53 °C m–1; boiling point of pure benzene = 80.1 °C). (the answer should be entered with 3 significant figures; do not enter units; give answer in normal notation--examples include 1.23 and 120. and -123 and 123. and 12.3) NEED HELP ASAP NO WORK NEEDED
Consider the following chemical equilibrium for the weak base CN in water: CN- (aq) + H₂O(1) = HCN (aq) + OH(aq). Which of the following statements is correct when more water is evaporated from system? Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a b C d pH will go up; [OH-] will go up; net amount of OH will go up pH will go down; [OH-]will go up; net amount of OH will go down pH will go down; [OH-]will go down; net amount of OH will go down pH will go up; [OH-] will go up; net amount of OH will go down
Use the References to access important The pH scale was designed to make it convenient to express hydrogen ion concentrations that are small in aqueous solutions. The definiton of pH is in terms of base 10 logarithms pH = -log[H+] where [H] is the hydrogen ion concentration. a. If the hydrogen ion concentration in a solution is 5.58 x 10-3 mol/L, the pH is b. If the pH of a solution is 3.007, the hydrogen ion concentration is mol/L.

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What is the pH of a 5.62\times 10-2 M aqueous solution of potassium fluoride, KF?pH = This solution is .