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Study Guide – Solutions, Acids, and Bases Solutions: 1. Describe the difference between homogeneous and heterogeneous mixtures. OMIT 2. What is the solvent and solute of a solution? Solute is dissolved while the solvent does the dissolving. 3. What does “like dissolves like” refer to? Explain the rule. Polar solvent dissolves polar solutes while nonpolar solvents dissolves nonpolar solutes. 4. What kinds of things can alcohols dissolve? Polar and nonpolar, because alcohols have a polar and nonpolar end. 5. How can you tell if something is polar or nonpolar? Polar- unequal sharing of electrons; nonpolar- equal sharing of electrons 6. What are electrolytes? In general, what KINDS of things are electrolytes? Conduct electric currents. Ionic compounds, acids, and bases. 7. What does solubility mean? Ability to dissolve in a solvent. 8. Describe the particles in a concentrated versus dilute solution. Same amount of particles, but more solvent in dilute than concentrated solutions. 9. What do the words “unsaturated”, “saturated”, and “supersaturated” mean? Unsaturated- below maximum capacity; saturated- at maximum capacity; supersaturated- above maximum capacity 10. How does temperature affect solubility? Increase solubility for solids; decreases solubility for gases 11. If you wanted to speed up how fast something dissolves, how could you do it? Increase the temperature, stir it, and crush it. 12. What is molarity? Unit for concentration. Moles/Liters 13. What equation do you use for dilutions? M1V1=M2V2 Acids & Bases: 14. Describe acids. Sour taste, release H+ ions in solution, pH< 7, turn litmus paper red 15. Describe bases. Bitter taste, release OH- ions in solution, pH >7, turn litmus paper blue 16. What are the Arrhenius definitions for acids and bases? Acids give up H+ ions, Bases give up OH- ions 17. What is the general reaction for a neutralization reaction? Acid + base -> salt + water 18. What salt would form from the reaction of Ca(OH)2 and HBr? CaBr2 19. Write the reaction of H2SO4 + Al(OH)3 H2O + Al2(SO3)3 20. What are the Bronsted-Lowry definitions of an acids and a base? Acids are proton donors and bases are proton acceptors. 21. Write the conjugate base for each ACID: OMIT b. HCO3- a. H2O c. NH4+ d. HPO42- 22. Write the conjugate acid for each BASE: OMIT b. HSO4- a. H2O c. HPO42- d. OH- 23. Label the acid, base, conjugate acid and conjugate base for this reaction: OMIT H2O + HCO3- H3O+ + CO3224. Sketch the pH scale and label strong acids, weak acids, strong bases, weak bases and neutral. 0 2 Strong acid 4 6 Weak acid 7 8 Neutral 10 12 Weak base 14 Strong Base 25. A pH of 13 is how many times more basic than a pH of 10? OMIT 26. Describe how a strong acid is different from a weak acid. Strong acids completely ionize in solution (completely let go of H+ ions) while weak acids only partially ionize/break apart. 27. How do you make a strong acid weak? OMIT 28. List the strong acids. HCl, HBr, HF 29. How do you know if a base is strong? Lets go off all of its OH- ions in solution 30. What is a titration? Uses a neutralization reaction to determine the concentration of an acid or base. 31. What is the standard solution? The solution with a known molarity 32. Write the formula: a. hydrofluoric acid HF b. rubidium hydroxide RbOH c. sulfuric acid H2SO4 d. copper (II) hydroxide Cu(OH)2 33. Write the name: a. HNO2 nitrous acid b. H2SO3 sulfurous acid c. Mg(OH)2 magnesium hydroxide d. LiOH lithium hydroxide Graphs and Problems 1. Which salt is the most soluble at 72oC? KNO3 2. How much NaNO3 could you put into 300g of water at 50oC? 336 grams 3. What kind of solution would you have if you added 80 g of KNO3 to 100g of water at 60oC? unsaturated 4. What molarity is a solution made from 20g of NaCl in 400 mL of water? 0.86 M 5. What volume should be used to make a solution that is 3.0 M if you only have 2 moles of a substance? 0.67 L 6. To what volume should you dilute a solution that has a concentration of 6 molar if you want to end up with 500 mL of 2.0 M? 166.7 mL or 0.17L 7. What is the pH of a solution with a [H+] of 2.3 x 10-5M? 4.64 8. If a solution has a [OH-] of 4.5 x 10-3M, is it an acid, base, or neutral? pH= 11.66 basic 9. What is the [OH-] if the pH is 3.7? 1 x 10-10.3 10. A student did a titration using 30mL of Ca(OH)2 to neutralize 75mL of 3.4M HCl. What is the concentration of the base? 8.5 M State the direction in which each of the following equilibrium systems would be shifted upon the application of the following stress listed beside the equation. 1. 2 SO2 (g) + O2 (g) ⇄ 2 SO3 (g) + energy decrease temperature right ⇄ increase temperature right 2 NO2 (g) increase total pressure left 4. CO (g) + H2O (g) ⇄ decrease total pressure 5. 2 NOBr (g) ⇄ 2 NO (g) + Br2 (g) 2. C (s) + CO2 (g) + energy 3. N2O4 (g) ⇄ 6. 3 Fe (s) + 4 H2O (g) ⇄ 2 CO (g) CO2 (g) + H2 (g) Fe3O4 (s) + 4 H2 (g) no shift decrease total pressure right add Fe(s) right ⇄ 7. CaCO3 (s) 8. N2 (g) + 3 H2 (g) 9. SO3(g) + CaO (s) + CO2 (g) remove CO2 (g) right ⇄ H2 is added right 2 NH3 (g) ⇄ H2O(g) At equilibrium [SO3] = 0.400M H2SO4(l) [H2O] = 0.480M [H2SO4] = 0.600M Calculate the value of the equilibrium constant. 3.125 10. H2 (g) + I2 (g) ⇄ 2HI (g) If at equilibrium [H2] = 0.200M and [I2] = 0.200M and Keq=55.6 at 250oC, calculate the equilibrium concentration of HI. 1.49 11. At equilibrium, a 2.0 L flask contains: 0.200 mol of PCl5 0.30 mol of H2O 0.60 mol of HCl Calculate the Keq for the reaction: PCl5 0.9 (g) + H2O (g) ⇄ 2HCl (g) + POCl3 (g) 0.300 mol of POCl3