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Introductory Chemistry (6th Edition)
- Write the net ionic equation in which the slightly soluble salt barium fluoride, BaF2, dissolves in dilute hydrochloric acid.arrow_forwardMany natural processes can be studied in the laboratory but only in an environment of controlled pH. Which of these combinations is the best to buffer the pH at approximately 7? Explain your choice. H3PO4/NaH2PO4 NaH2PO4/Na2HPO4 Na2HPO4/Na3PO4arrow_forwardWhat is the pH of a solution that consists of 0.20 M ammonia, NH3, and 0.20 M ammonium chloride, NH4Cl?arrow_forward
- Write the Ksp expression for each of these slightly soluble salts: CuBr HgI2 SrSO4arrow_forwardWrite the ionic equation for the dissolution and the Ksp expression for each of the following slightly soluble ionic compounds: (a) LaF3. (b) CaCO3. (c) Ag2SO4. (d) Pb(OH)2arrow_forwardA 1.0-L solution that is 4.2 M in ammonia is mixed with 26.7 g of ammonium chloride. a What is the hydroxide-ion concentration of this solution? b 0.075 mol of MgCl2 is added to the above solution. Assume that there is no volume change. After Mg(OH)2 has precipitated, what is the molar concentration of magnesium ion? What percent of the Mg2+ is removed from solution?arrow_forward
- Describe the effect on the pH of the following actions or explain why there is not an effect: (a) Adding sodium acetate, NaCH3CO2, to 0.100 M CH3CO2H (b) Adding NaNO3 to 0.100 M HNO3arrow_forwardWhen a diprotic acid, H2A, is titrated with NaOH, the protons on the diprotic acid are generally removed one at a time, resulting in a pH curve that has the following generic shape: a. Notice that the plot has essentially two titration curves. If the first equivalence point occurs at 100.0 mL NaOH added, what volume of NaOH added corresponds to the second equivalence point? b. For the following volumes of NaOH added, list the major species present after the OH reacts completely. i. 0 mL NaOH added ii. between 0 and 100.0 mL NaOH added iii. 100.0 mL NaOH added iv. between 100.0 and 200.0 mL NaOH added v. 200.0 mL NaOH added vi. after 200.0 mL NaOH added c. If the pH at 50.0 mL NaOH added is 4.0, and the pH at 150.0 mL NaOH added is 8.0, determine the values Ka1, and Ka2 for the diprotic acid.arrow_forwardA solution is 1.5 104 M Zn2 and 0.20 M HSO4. The solution also contains Na2SO4. What should be the minimum molarity of Na2SO4 to prevent the precipitation of zinc sulfide when the solution is saturated with hydrogen sulfide (0.10 M H2S)?arrow_forward
- Which compound in each pair is more soluble in water than is predicted by a calculation from Ksp? (a) AgI or Ag2CO3 (b) PbCO3 or PbCl2 (c) AgCl or AgCNarrow_forwardWhat do you suppose happens to the Ksp, value of a solid as the temperature of the solution changes? Consider both increasing and decreasing temperatures, and explain your answer.arrow_forwardFor the titration of 50. mL of 0.10 M ammonia with 0.10 M HCI, calculate the pH. For ammonia, NH3, Kp = 1.8 x 10-5. (a) Before the addition of any HCl solution. pH = Use correct number of significant digits; (b) After 20. mL of the acid has been added. pH = Use correct number of significant digits; (c) After half of the NH3 has been neutralized. pH Use correct number of significant digits; (d) At the equivalence point. pH Use correct number of significant digits;arrow_forward
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