Chemistry: An Atoms-Focused Approach
14th Edition
ISBN: 9780393912340
Author: Thomas R. Gilbert, Rein V. Kirss, Natalie Foster
Publisher: W. W. Norton & Company
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Chapter 15 Solutions
Chemistry: An Atoms-Focused Approach
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- 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?arrow_forwardCommon Acids and Bases Use the data in Table 18.8 to answer the following questions. Which substance is the most basic? Which substance is closest to neutral? Which has a concentration of H+=4.01010M ? Which has a pOH of 11.0? How many times more basic is antacid than blood?arrow_forwardExplain why the pH does not change significantly when a small amount of an acid or a base is added to a solution that contains equal amounts of the acid H3PO4 and a salt of its conjugate base NaH2PO4.arrow_forward
- A sample of vinegar has a hydronium-ion concentration of 3.0 103 M. What is the pH of the vinegar?arrow_forwardPhthalic acid H2C8H4O4, is a diprotic acid. It is used to make phenolphthalein indicator. Ka1=0.0012, and Ka2=3.9106. Calculate the pH of a 2.9 M solution of phthalic acid. Estimate [HC8H4O4-] and (C8H4O42-].arrow_forwardAt 25C, a 0.327 M solution of a weak acid HX has a pH of 5.12. What is G for the dissociation of the weak acid?arrow_forward
- A chemist wanted to determine the concentration of a solution of lactic acid, HC3H5O3. She found that the pH of the solution was 2.60. What was the concentration of the solution? The Kd of lactic acid is 1.4 104.arrow_forwardTile pH of a solution of household ammonia, a 0.950 M solution of NH3 is 11.612. Determine Kb for NH3 from these data.arrow_forwardThe pH of human blood is steady at a value of approximately 7.4 owing to the following equilibrium reactions: CO2(aq)+H2O(l)H2CO3(aq)H2CO3(aq)+H+(aq) Acids formed during normal cellular respiration react with the HCO3 to form carbonic acid, which is in equilibrium with CO2(aq) and H2O(l). During vigorous exercise, a persons H2CO3 blood levels were 26.3 mM whereas his CO2 levels were 1.63 mM. On resting, the H2CO3 levels declined to 24.9 mM. What was the CO2 blood level at rest?arrow_forward
- Using the acid ionization constant information given in Table 10-3, indicate which acid is the stronger in each of the following acid pairs. a. H3PO4 and H2PO4 b. H3PO4 and H2CO3 c. HPO42 and H2PO4 d. HC2H3O2 and HCNarrow_forwardAcetic acid and sodium hydrogen carbonate, NaHCO3, are mixed in water. Write a balanced equation for the acid-base reaction that could, in principle, occur. Using Table 16.2, decide whether the equilibrium lies predominantly to the right or to the left.arrow_forwardExplain why the ionization constant, Ka, for H2SO4 is larger than the ionization constant for H2SO3.arrow_forward
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