Chapter 14 Test Review

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Chapter 14 Test Review. Acids and Bases 14.1-14.3, 14.5-14.8. 1. According to the Arrhenius concept, if HNO 3 were dissolved in water, it would act as ___. A) a base B) an acid C) a proton acceptor D) a source of H- ions E) a source of hydroxide ions.
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Chapter 14 Test ReviewAcids and Bases14.1-14.3, 14.5-14.81. According to the Arrhenius concept, if HNO3 were dissolved in water, it would act as ___.A) a baseB) an acidC) a proton acceptorD) a source of H- ionsE) a source of hydroxide ions2. The name given to an aqueous solution of HBrO2 is ___.A) bromous acidB) hydrobromic acidC) hypobromous acidD) hydrogen bromideE) bromic acid3. The name of HClO is ___.A) Chloric acidB) Hypochlorous acidC) Hydrochlorous acidD) Hydrogen chlorideE) Perchloric acid4. The I.U.P.A.C. name of the following ___ acid.CH3COOHA) carbonicB) chloric acidC) ethanoicD) aceticE) carboxylic5. According to the Brønsted-Lowery definition, a proton-donor is a(n) ___.A) H+ acceptorB) OH- acceptorC) saltD) baseE) acid6. Which of the following compounds would be an Arrhenius base?A) NaClOB) Na2SO4C) NaOHD) CuCl2E) H3P7. Identify the B-L acid in forward direction of the following reaction.A) H2O(l) B) CO32-(aq) C) OH-(aq) D) H2CO3 (aq)E) HCO32- (aq)H2O(l) + CO32-(aq) HCO32- (aq) + OH-(aq) 8. Identify the B-L base in reverse direction of the following reaction.A) CH3CH2NH3+(aq) B) CH3CH2NH2(aq) C) H2S(aq)D) CH3CH2NH4-(aq) E) HS-(aq) CH3CH2NH3+(aq) + HS-(aq) CH3CH2NH2(aq) + H2S(aq) 9. For KW, the product of [H3O+] and [OH-] is __.A) 1 x 10-1B) 1 x 1014C) 1 x 107D) 1 x 101E) 1 x 10-1410. What is the [H3O+] in a solution with [OH-] = 1 x 10-12 M?A) 1 x 102 MB) 1 x 10-12 MC) 1 x 10-7 MD) 1 x 10-8 ME) 1 x 10-2 M11. What is the [OH-] in a solution with [H3O+] = 1 x 10-6 M?A) 1 x 10-6 MB) 1 x 10-2 MC) 1 x 10-12 MD) 1 x 10-10 ME) 1 x 10-8 M12. A solution with a pH of 4 is ___.A) extremely acidicB) neutralC) moderately acidicD) extremely basicE) slightly basic13. The [H3O+] of a solution with a pH = 2.0 has a concentration of ___.A) 10 MB) 1 x 10-2 MC) - 10MD) 1 x 10-12 ME) 1 x 102 M14. Which of the following has the pH values correctly arranged from the most basic to the least basic?A) 6, 7, 8, 9, 10B) 14, 13, 12, 11, 10C) 3, 7, 9, 11, 13D) 13, 6, 10, 5, 1E) None of these are correct.15. Which of the following is one of the 7 strong acids?A) NH4+B) HFC) H3O+D) HClO3E) NaOH16. Which of the following has been correctly identified?A) HClO4, strong acidB) Al(OH)3, strong baseC) H3O+, strong acidD) NH3, strong acidE) NaOH, weak base17. Ammonia is a weak base because __.A) it is completely ionized in aqueous solutionB) it is only slightly soluble in waterC) it cannot hold on to its hydroxide ionsD) it produces few hydroxide ions in waterE) it is a dilute solutionNH3(aq) + H2O(l) NH4+ (aq) + OH-(aq) 18. Water is an example of a(n) ___ compound.A) organicB) nonpolarC) amphotericD) ionicE) carboxylic acid19. One example of an Arrhenius base is ___.A) H2SO4B) KOHC) NaClD) H2O2E) C2H4O220. Acetic acid is an example of a(n) ___.A) inorganic compoundB) weak acidC) strong acidD) oxy acidE) binary acid21. In water solution, the conjugate base of HF is ___.A) H2OB) H+C) F-D) OH-E) H2HF(aq) + H2O(l) H3O+ (aq) + F-(aq) 22. The conjugate acid of NO2- is ___.A) OH-B) H2OC) HNO3D) HNO2E) H+23. Bicarbonate ion, HCO3-, is an example of a(n) ___ substance.A) gaseousB) neutralC) strongly acidicD) amphotericE) strongly basic24. The conjugate acid of NH3 is ___.A) NH2-B) NH4+C) H3O+D) H2OE) OH-25. The pH of a 0.05 M solution of KOH is ___.A) 12.7B) 1.3C) 13.5D) 5.0E) 9.00.05 M KOH = 0.05 M OH-2) pOH = -log(0.05) → 1.33) 14.00 – 1.3 = 12.726. The pH of a solution is 4.50. The pOH of this solution is ___.A) 14.00B) 4.50C) 2.00D) 9.50E) 7.00pH + pOH = 14.0014.00 – 4.50 = 9.5027. What is the pOH of a solution with a pH of 3.77?A) 2.5B) 0.25C) 10.3D) 0.115E) 14.0pH + pOH = 14.0014.00 – 3.77 = 10.328. A solution with a pH of 10.00 is basic.TRUE or FALSE29. What are the products of the following reaction between an active metal and a strong acid?A) SrHNO3B) SrH + NO3C) NOH + SrO2D) O2 + SrNO2 + HE) H2 + Sr(NO3)2Sr(s) + HNO3(aq) ????The products are always hydrogen gas and the metal salt of the acid.30. In an acidic solution ___.A) [H+] = 0B) [OH-] = 0C) [OH-] > [H+] D) [OH-] = [H+] E) [H+] > [OH-] 31. A solution with a pH of 2.0 is ___ times more acidic than a solution with a pH of 5.0.A) 2B) 5C) 10D) 1,000E) 10032. According to the table at the right, which of the following is the weakest acid?A) HFB) H2OC) H2PO4-D) HClE) NH4+33. According to the table at the right, when H2S and HF are reacted, what will be the proton donor?A) HFB) H2OC) H2SD) F-E) HS-The stronger of the two acids will be the H+ donor.34. Which of the following acids has the strongest conjugate base?A) HFB) H2OC) H2SD) HClE) H3O+The acid with the conjugate which is furthest down on the right.35. Are reactants or products favored in the following acid-base equilibrium?HF(aq) + H2O(l) H3O+ (aq) + F-(aq) A) reactantsB) products36. Predict the products of the following reaction between a strong acid and a metal carbonate. Balance the equation when you are done.Li2CO3 + HNO32 2 LiNO3 + CO2(g) + H2O(l)????The products are always carbon dioxide gas, water, and the metal salt of the acid.37. 50.0 mL of HNO3 were titrated to the end point with 25.0 mL of 0.35 M KOH solution.Write a balanced chemical equation for this acid-base neutralization reaction.HNO3 (aq) + KOH(aq) → H2O(l) + KNO3Remember: the products of the neutralization reaction between a strong acid and a strong base are always water and the metal salt of the acid.38. 50.0 mL of HNO3 were titrated to the end point with 25.0 mL of 0.35 M KOH solution.Calculate the number of moles of KOH needed to completely neutralize the HNO3.0.35 mole KOH / L x 0.0250 L = 0.0088 mol KOHDetermine the number of moles of HNO3 which were neutralized by the KOH.1 : 1 stoichiometry between HNO3 and KOH, so 0.0088 mol KOH used = 0.0088 mol HNO3 neutralizedCalculate the Molarity of the acid solution.0.0088 mol HNO3 / 0.0500 L = 0.18 M 39. 50.0 mL of HNO3 were titrated to the end point with 25.0 mL of 0.35 M KOH solution.Which solution was the standardized solution?KOHIf phenolphthalein indicator had been added to the acid, what color would the solution be at the endpoint of the titration?Pink
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