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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Chemistry: An Atoms-Focused Approach
Ch. 8 - Prob. 8.1VPCh. 8 - Prob. 8.2VPCh. 8 - Prob. 8.3VPCh. 8 - Prob. 8.4VPCh. 8 - Prob. 8.5VPCh. 8 - Prob. 8.6VPCh. 8 - Prob. 8.7VPCh. 8 - Prob. 8.8VPCh. 8 - Prob. 8.9VPCh. 8 - Prob. 8.10VP
Ch. 8 - Prob. 8.11QACh. 8 - Prob. 8.12QACh. 8 - Prob. 8.13QACh. 8 - Prob. 8.14QACh. 8 - Prob. 8.15QACh. 8 - Prob. 8.16QACh. 8 - Prob. 8.17QACh. 8 - Prob. 8.18QACh. 8 - Prob. 8.19QACh. 8 - Prob. 8.20QACh. 8 - Prob. 8.21QACh. 8 - Prob. 8.22QACh. 8 - Prob. 8.23QACh. 8 - Prob. 8.24QACh. 8 - Prob. 8.25QACh. 8 - Prob. 8.26QACh. 8 - Prob. 8.27QACh. 8 - Prob. 8.28QACh. 8 - Prob. 8.29QACh. 8 - Prob. 8.30QACh. 8 - Prob. 8.31QACh. 8 - Prob. 8.32QACh. 8 - Prob. 8.33QACh. 8 - Prob. 8.34QACh. 8 - Prob. 8.35QACh. 8 - Prob. 8.36QACh. 8 - Prob. 8.37QACh. 8 - Prob. 8.38QACh. 8 - Prob. 8.39QACh. 8 - Prob. 8.40QACh. 8 - Prob. 8.41QACh. 8 - Prob. 8.42QACh. 8 - Prob. 8.43QACh. 8 - Prob. 8.44QACh. 8 - Prob. 8.45QACh. 8 - Prob. 8.46QACh. 8 - Prob. 8.47QACh. 8 - Prob. 8.48QACh. 8 - Prob. 8.49QACh. 8 - Prob. 8.50QACh. 8 - Prob. 8.51QACh. 8 - Prob. 8.52QACh. 8 - Prob. 8.53QACh. 8 - Prob. 8.54QACh. 8 - Prob. 8.55QACh. 8 - Prob. 8.56QACh. 8 - Prob. 8.57QACh. 8 - Prob. 8.58QACh. 8 - Prob. 8.59QACh. 8 - Prob. 8.60QACh. 8 - Prob. 8.61QACh. 8 - Prob. 8.62QACh. 8 - Prob. 8.63QACh. 8 - Prob. 8.64QACh. 8 - Prob. 8.65QACh. 8 - Prob. 8.66QACh. 8 - Prob. 8.67QACh. 8 - Prob. 8.68QACh. 8 - Prob. 8.69QACh. 8 - Prob. 8.70QACh. 8 - Prob. 8.71QACh. 8 - Prob. 8.72QACh. 8 - Prob. 8.73QACh. 8 - Prob. 8.74QACh. 8 - Prob. 8.75QACh. 8 - Prob. 8.76QACh. 8 - Prob. 8.77QACh. 8 - Prob. 8.78QACh. 8 - Prob. 8.79QACh. 8 - Prob. 8.80QACh. 8 - Prob. 8.81QACh. 8 - Prob. 8.82QACh. 8 - Prob. 8.83QACh. 8 - Prob. 8.84QACh. 8 - Prob. 8.85QACh. 8 - Prob. 8.86QACh. 8 - Prob. 8.87QACh. 8 - Prob. 8.88QACh. 8 - Prob. 8.89QACh. 8 - Prob. 8.90QACh. 8 - Prob. 8.91QACh. 8 - Prob. 8.92QACh. 8 - Prob. 8.93QACh. 8 - Prob. 8.94QACh. 8 - Prob. 8.95QACh. 8 - Prob. 8.96QACh. 8 - Prob. 8.97QACh. 8 - Prob. 8.98QACh. 8 - Prob. 8.99QACh. 8 - Prob. 8.100QACh. 8 - Prob. 8.101QACh. 8 - Prob. 8.102QACh. 8 - Prob. 8.103QACh. 8 - Prob. 8.104QACh. 8 - Prob. 8.105QACh. 8 - Prob. 8.106QACh. 8 - Prob. 8.107QACh. 8 - Prob. 8.108QACh. 8 - Prob. 8.109QACh. 8 - Prob. 8.110QACh. 8 - Prob. 8.111QACh. 8 - Prob. 8.112QACh. 8 - Prob. 8.113QACh. 8 - Prob. 8.114QACh. 8 - Prob. 8.115QACh. 8 - Prob. 8.116QACh. 8 - Prob. 8.117QACh. 8 - Prob. 8.118QACh. 8 - Prob. 8.119QACh. 8 - Prob. 8.120QACh. 8 - Prob. 8.121QACh. 8 - Prob. 8.122QACh. 8 - Prob. 8.123QACh. 8 - Prob. 8.124QACh. 8 - Prob. 8.125QACh. 8 - Prob. 8.126QACh. 8 - Prob. 8.127QACh. 8 - Prob. 8.128QACh. 8 - Prob. 8.129QACh. 8 - Prob. 8.130QA
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- The amount of oxygen, O2, dissolved in a water sample at 25 C can be determined by titration. The first step is to add solutions of MnSO4 and NaOH to the water to convert the dissolved oxygen to MnO2. A solution of H2SO4 and KI is then added to convert the MnO2 to Mn2+, and the iodide ion is converted to I2. The I2 is then titrated with standardized Na2S2O3. (a) Balance the equation for the reaction of Mn2+ ions with O2 in basic solution. (b) Balance the equation for the reaction of MnO2 with I in acid solution. (c) Balance the equation for the reaction of S2O32 with I2. (d) Calculate the amount of O2 in 25.0 mL of water if the titration requires 2.45 mL of 0.0112 M Na2S2O3 solution.arrow_forwardThere are many ionic compounds that dissolve in water to a very small extent. One example is lead(II) chloride. When it dissolves an equilibrium is established between the solid salt and its component ions. Suppose you stir some solid PbCl2 into water. Explain how you would prove that the compound dissolves but to a small extent? Is the dissolving process product-favored or reactant-favored? pbcl2(s)pb2+(aq)+2cl(aq)arrow_forwardSeparate samples of a solution of an unknown soluble ionic compound are treated with KCl, Na2SO4, and NaOH. A precipitate forms only when Na2SO4 is added. Which cations could be present in the unknown soluble ionic compound?arrow_forward
- You pour 150.0 mL of a 0.250 M lead(ll) nitrate solution into an empty 500-mL flask. What is the concentration of nitrate ions in the solution? What volume of 0.100 M sodium phosphate must be added to precipitate the lead(ll) ions from the solution?arrow_forwardA student is asked to identify the metal nitrate present in an aqueous solution. The cation in the solution can be either Na+, Ba2+, Ag+, or Ni2+. Results of solubility experiments are as follows: unknown + chloride ions—no precipitate unknown + carbonate ions—precipitate unknown + sulfate ions—precipitate What is the cation in the solution?arrow_forwardCitric acid, which can be obtained from lemon juice, has the molecular formula C6H8O7. A 0.250-g sample of citric acid dissolved in 25.0 mL of water requires 37.2 mL of 0.105 M NaOH for complete neutralization. What number of acidic hydrogens per molecule does citric acid have?arrow_forward
- Consider an experiment in which two burets, Y and Z, are simultaneously draining into a beaker that initially contained 275.0 mL of 0.300 M HCl. Buret Y contains 0.150 M NaOH and buret Z contains 0.250 M KOH. The stoichiometric point in the titration is reached 60.65 minutes after Y and Z were started simultaneously. The total volume in the beaker at the stoichiometric point is 655 mL. Calculate the flow rates of burets Y and Z. Assume the flow rates remain constant during the experiment.arrow_forwardA student mixes four reagents together, thinking that the solutions will neutralize each other. The solutions mixed together are 50.0 mL of 0.100M hydrochloric acid, 100.0 mL of 0.200 M of nitric acid, 500.0 mL of 0.0100 M calcium hydroxide, and 200.0 mL of 0.100 M rubidium hydroxide. Did the acids and bases exactly neutralize each other? If not, calculate the concentration of excess H+ or OH ions left in solution.arrow_forward
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