QUESTION 1QUESTION 2QUESTION 3QUESTION 4QUESTION 5QUESTION 6QUESTION 7QUESTION 8QUESTION 9QUESTION 10QUESTION 11QUESTION 12QUESTION 13QUESTION 14QUESTION 15QUESTION 16QUESTION 17QUESTION 18QUESTION 19QUESTION 20QUESTION 22Q U E STI O N 11. What is the pH of a solution with a [OH-] concentration of 3.70E-04 M? The error interval is +/- 0.1 pH units.1 points Q U E S T I O N 21. Suppose 2.25 mol of NOCl is added to a 2.00 L reaction chamber. After equilibrium has been achieved, then it was determined that 15.0 % of the NOCl had dissociated. Calculate Keq (concentration based) for this reaction: 2NOCl(g) = 2NO(g) + Cl2(g)1 points Q U E S T I O N 31. You are titrating a weak, monoprotic acid with a strong base. There were 0.700 moles of the acid originally and you added 0.200 mol of NaOH. If the pH of the solution at this point was 4.80, then what is the pKa of the weakacid?4.66.14.85.25.51 points Q U E S T I O N 41. How many milliliters of 0.2 N NaOH are required to neutralize 50 mL of 0.25 N HCl? (Question from Barron’s New MCAT 2007, 11th edition)5062.50.252.51 points Q U E S T I O N 51. What is the pH of a 500 mL of water that had 1.00 mL of 0.100 M HCl added to it? The error interval is +/- 0.1 pH units. You can ignore the autoionization of water for this question.1 points Q U E S T I O N 61. What is the solubility of silver iodide in pure water? The Ksp for this compound is 8.30E-17. Enter the answer in units of mg/L.1 points Q U E S T I O N 71. The Ka for HCN is 4.90×10−10. What is the value of Kb for CN−?4.9×104 4.9×10−24 4.0×10−6 2.0×10−5 2.0×1091 points Q U E S T I O N 81. What is the pH of a 0.0100 M (before ionization) solution of formic acid (HCOOH)? The Ka of this acid is 1.80×10−4. The units for the answer is a pH value with an error interval of +/- 0.1 pH units.1 points Q U E S T I O N 91. The addition of which of the following substances will result in an increase in the pH of a 0.01 M acetic acid solution?None of the substances listed will affect the pH ofthe solution.NaClKICaCl2NaClO41 points Q U E S T I O N 1 01. The equivalence point in a weak base-strong acid titration is at a pH of __________.7114<7>71 points Q U E S T I O N 1 11. Which of the following acids is expected to be the strongest acid?HIO3HBrO3HClO31 points Q U E S T I O N 1 21. Which is the strongest acid?Phosophoric, Ka = 7.5x10-3Butanoic, Ka = 1.5x10-5Sulfurous, Ka = 1.7x10-2Hydrofluoric; Ka = 6.8x10-4Hypochlorous; Ka = 3.0x10-81 points Q U E S T I O N 1 31. Which of the following statements is not true?Pure substances do not appear in the equilibrium constant equation so long as they are still present at equilibrium.Increasing the pressure on a system with gases will shift the equilibrium towards the reaction side with more moles of gases.Increasing the temperature of an exothermic reaction will shift the equilibrium towards the reactant side of the chemical reaction.If Q is less than Keq at a particular time, then the reaction is currently forming more products.1 points Q U E S T I O N 1 41. The equilibrium-constant expression depends on the __________ of the reaction.temperaturemechanismstoichiometry and mechanismstoichiometrythe quantities of reactants and products initially present1 points Q U E S T I O N 1 51. Calculate the pOH of a 0.0827 M aqueous sodium cyanide solution at 25.0°C. Kb for CN− is 2.50x10-6. CN−(aq) + H2O(l) = HCN(aq) + OH−(aq)1.083.3410.669.318.81 points Q U E S T I O N 1 61. Given the reaction : H2(g) + F2(g) = 2HF(g); Keq = 1.3E+3, then what is the value of Q when there are 0.03 moles of both H2 and F2 and 0.24 moles ofHF in a sealed flask? At this condition, is the reaction forming product or forming reactant?Q = 0.0037; products are being formedQ = 0.0037; reactants are being formedQ = 0.56; reactants are being formedQ = 267; products are being formedQ = 64; product is being formed1 points Q U E S T I O N 1 71.Which of the following chemicals are acids or can behave like acids? You may select more than one compound.F-Ca(OH)2HClO2HCl1 points Q U E S T I O N 1 81. Suppose 500 mL of 0.200 M chlorous acid , which has a pKa of 1.959, solution is titrated with 75.0 mL of a 1.00 M NaOH. What is the final pH? The error interval is +/- 0.2 pH units.1 points Q U E S T I O N 1 91. What is the pH of a solution with a [H+] concentration of 1.30E-08 M? The error interval is +/- 0.1 pH units.1 points Q U E S T I O N 2 01. The equilibria H2SO4 = H+ + HSO4− and HSO4− = H+ + SO42− have constants of 2.4×102 and 5.0×10−5 respectively. The equilibrium constant for the dissociation of H2SO4 is: (Question from "Cracking the MCAT, 2010-2011 edition" by The Princeton Review)x1.2×10-22.4×1025.0×10-54.8×106Q U E S T I O N 2 11. The addition of hydrochloric acid and ____________ to water produces a buffer solution.phenol (HC6H5O) X NH3 NaNO3 NaOH HNO3 1 points Q U E S T I O N 2 21. Which of the following substances not an acid?XFe3+(aq)HNO2CH3COOH(aq)HIClO−1 points Click Save and Submit to save and submit. Click Save All Answers to save all