Write your name, banner id # and the date in the space provided on the scantron. All answers must be

Write your name, banner id # and the date in the space provided on the scantron. All answers must be
Write your name, banner id # and the date in the space provided on the scantron. All answers must be on the scantron and this exam. B. Read each item carefully select the word, phrase or expression that best completes the test item. Indicate the answer by blackening the appropriate space on your answer sheet. You MUST erase completely to for an erased item. This AND the scantron must be in. All questions are worth 5 points. R = 0.08206 (atm middot L)/(mol middot K) = 8.314 J/(mol middot K) pH = -log[H_3O^+] pH + POH = 14 = pK_a + pK_b [OH^_] [H_3O^+] = 10^-14 = k_a times K_b (at least in water, at 25 degree C) pH = pK_a + log([base)/[acid]) pOH = pK_b + log ([acid]/[base]) K_p = K_ (RT)^For a salt that dissociated into a cation with a coefficient of n and an anion with a coefficient of m: Molar Solubility = Squareroot K_sp/n^m^x = -b plusminus Squareroot b^2 – 4ac/2a where 0 = ax^2 + bx + c 1) Which following solutions would have the second lowest pH? Assume all their concentrations are 0.10 at 25 degree C. The acid is followed by its K_a value. HF, 3.5 times 10^-4 HCN, 4.9 times 10^-10 HNO_2 46 times 10^-4 HCHO_2, 1.8 times 10^-4 HClO_2, 1.1 times 10^-2 Which of the following are false about systems at equilibrium? The rate of the forward and reverse reactions are the same. The concentrations of each component are equal. The concentrations of each component don't change over time. Catalysts do not affect the equilibrium. This symbol is used in a reaction where an equilibrium is present: The reaction below has a K_c value of 3.64 times 10^-3 What is the value of K_p for this reaction at 25 degree C? CO_2(g) + C(s, graphite) 2CO(g) A) 3.64 times 10^-3 B) 6.09 times 10^-6 C) 8.90 times 10^-2 D) 1.49 times 10^-4 E) 2.17 Express the equilibrium constant K for the reaction in question 3. A) [CO(g)]/[CO_2(g)] [C(s)] B) [CO(g)]/[CO_2(g)] [CO(g)]^2/[CO_2(g)] [C(s)] D) [CO_2(g)]^2
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