Which of the following statements is/are true? (Select all that apply) OThe higher the concentration of OH in a solution, the lower the pH. OThe higher the concentration of OH in a solution, the lower the pOH. O An acidic solution has a pH of geater than 7. The concentration of H30* in pure water is 1.00 x 107 M. OA Bronsted acid is a proton donor in an acid-base reaction.

Which of the following statements is/are true? (Select all that apply) OThe higher the concentration of OH in a solution, the lower the pH. OThe higher the concentration of OH in a solution, the lower the pOH. O An acidic solution has a pH of geater than 7. The concentration of H30* in pure water is 1.00 x 107 M. OA Bronsted acid is a proton donor in an acid-base reaction.

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter13: Acids And Bases

Section: Chapter Questions

Problem 2ALQ: Differentiate between the terms strength and concentration as they apply to acids and bases. When is...

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Differentiate between the terms strength and concentration as they apply to acids and bases. When is HCl strong? Weak? Concentrated? Dilute? Answer the same questions for ammonia. Is the conjugate base of a weak acid a strong base?
For which of the following solutions must we consider the ionization of water when calculating the pH or pOH? (a) 3108M HNO3. (b) 0.10 g HCl in 1.0 L of solution. (c) 0.00080 g NaOH in 0.50 L of solution. (d) 1107M Ca(OH)2. (e) 0.0245 M KNO3
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?
Write an equation that describes the equilibrium that exists when nitric acid dissolves in water. Identify each of the four species in solution as either Brnsted acids or Brnsted bases. Does the equilibrium favor the products or the reactants?
You are asked to calculate the H+ concentration in a solution of NaOH(aq). Because sodium hydroxide is a base, can we say there is no H+. since having H+ would imply that the solution is acidic?
Consider a solution prepared by mixing a weak acid HA. HCl, and NaA. Which of the following statements best describes what happens? a. The H+ from the HCl reacts completely with the A from the NaA. Then the HA dissociates somewhat. b. The H+ from the HCl reacts somewhat with the A from the NaA to make HA, while the HA is dissociating. Eventually you have equal amounts of everything. c. The H+ from the HCl reacts somewhat with the A from the NaA to make HA while the HA is dissociating. Eventually all the reactions have equal rates. d. The H+ from the HCl reacts completely with the A from the NaA. Then the HA dissociates somewhat until too much H+ and A are formed, so the H+ and A react to form HA, and so on. Eventually equilibrium is reached. Justify your choice, and for choices you did not pick, explain what is wrong with them.
The weak base, CIO (hypochlorite ion), is used in the form of NaCIO as a disinfectant in swimming pools and water treatment plants. What are the concentrations of HCIO and OH and the pH of a 0.015 M solution of NaCIO?
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A student prepares 455 mL of a KOH solution, but neglects to write down the mass of KOH added. His TA suggests that he take the pH of the solution. The pH is 13.33. How many grams of KOH were added?
Both HF and HCN ionize in water to a limited extent. Which of the conjugate bases. F“ or CN”, is the stronger base? See Table 14.2.
12.62 Write the formula of the conjugate acid of each of the following bases, (a) OH-, (b) NHj, (c) CHjNHt, (d) HPO/-, (e) CO.,2’
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