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Acid Base Review

Acid Base Review. Which acid will be a better conductor of electricity? Hydrofluoric acid Carbonic acid Cyanic acid Nitric acid. Which of the following acid/salt pairs would make a buffer system? Hydrobromic acid and potassium bromide Sulfuric acid and sodium sulfate

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Acid Base Review

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  1. Acid Base Review

  2. Which acid will be a better conductor of electricity? • Hydrofluoric acid • Carbonic acid • Cyanic acid • Nitric acid

  3. Which of the following acid/salt pairs would make a buffer system? • Hydrobromic acid and potassium bromide • Sulfuric acid and sodium sulfate • Acetic acid and sodium acetate • Nitric acid and potassium nitrate

  4. Notice the equivalence point. For a strong acid; strong base titration it will be pH=7. Weak acid or base systems will be different. Weak acid Buffer System Which is a titration of a weak acid? Of a strong acid? How do you know? Which graph could be a buffer system? Where is the buffer region? Strong acid

  5. Which of the following is NOT a Bronsted-Lowry type acid-base reaction? • NH3(aq) + H3O+(aq) <=> NH4+(aq) + H2O (l) • OH-(aq) + HNO3(aq) <=> H2O (l) + NO3-(aq) • HSO4-(aq) + NH3(aq) <=> NH4+(aq) + SO42-(aq) • Zn (s) + 2 HCl(aq) <=> Zn2+(aq) + H2 (g) + 2 Cl-(aq) • 2 H2O (l) <=> H3O+(aq) + OH-(aq)

  6. Given this equilibrium reaction, NH3 + H2O <==> NH4+ + OH- According to Bronsted-Lowry theory, which species are considered acids? • Both NH3 and OH- • Both NH3 and NH4+ • Both H2O and NH3 • Both H2O and OH- • Both H2O and NH4+

  7. HPO42- is a Bronsted-Lowry acid. Which of the following would be the conjugate base of this acid? • H3PO4 • H2PO4- • PO43- • H3O+ • OH-

  8. The conductivity of an HCl solution is greater than the conductivity of an CH3CO2H solution because: • HCl reacts with water to produce a lesser quantity of ions in solution than the reaction of CH3CO2H with water. • HCl reacts with water to produce a greater quantity of ions in solution than the reaction of CH3CO2Hwith water. • HCl is a weaker acid than CH3CO2H. • the dissociation of water makes a more significant contribution to [H3O+]total in the HCl solution than in the CH3CO2Hsolution. • the conjugate base of HCl is a stronger base than the conjugate base of CH3CO2H.

  9. For the reaction of acetic acid (HOAc) with water, HOAc(aq) + H2O(l) <==> H3O+(aq) + OAc-(aq) which of the following statements is correct? • HOAc and H3O+ are a conjugate acid/base pair. • HOAc and H2O are a conjugate acid/base pair. • H2O and OAc- are a conjugate acid/base pair. • HOAc and OAc- are a conjugate acid/base pair.

  10. Which species is amphoteric?a)H2O b) H2PO4- c)HCO3- d) HSO4- All H2PO4- + H3O+ → H3PO4+ H2O H2PO4-+ OH- → HPO42-+ H2O HCO3- + H3O+ → H2CO3 + H2O HCO3-+ OH- → CO32- + H2O HSO4-+H3O+ H2SO4+ H2O HSO4- + OH- H2O + SO42-

  11. Which hydrogen is most likely to be an acidic hydrogen? Why? Hydrogen attached to an electronegative element

  12. Calculate the pH of an acidic solution with a[H+] of 3.2 x 10 -4. -Log 3.2 x 10 -4 = 3.49 What is the pOH? pH + pOH = 14 so 14 – 3.49 = pOH = 10.51 What is the [OH-]? take the pOH and make it negative -10.51 then take the antilog. (-10.51)= 3.1 x 10 -11 2nd LOG

  13. Titration Problem What is the acid concentration if 1.2 liters requires 54 ml of .01M NaOH for neutralization? MBVB = MAVA (0.01M)(.054L) = MA(1.2L) MA = 0.00045 Be able to do a problem where you are given the grams of titrant and have to calculate the molarity. For example, a solution of NaOH was made by dissolving 4 grams of solid NaOH in 500ml of water. 4gramsx 1moleNaOH x 1000ml = 0.2M NaOH 500ml 40grams 1L

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