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Q 21: Which of the following is the strongest acid? A) HF (K, for HF is...
Which of the following is the strongest acid? A.) HCNO (Ka for HCNO is 2*10^-5) B.) HF (Ka for HF is 7.2*10^-4) C.) H3BO3 (Ka for H3BO3 is 5.4*10^-10) D.) HCN (Ka for HCN is 4.9*10^-10)
estion 10 of 65 > Consider the reaction. HF(aq) + KOH(aq) — KF(aq) + H20(1) What is the net ionic equation for the chemical reaction? HF(aq) + K+(aq) + OH(aq) — K+(aq) + F (aq) + H2O(1) O HF(aq) + K+(aq) + OH-(aq) — K+(aq) + F (aq) + H+(1) + OH-(1) O HF(aq) + OH-(aq) —> F-(aq) + H2O(1) HF(aq) + K+(aq) F (aq) + H+(1) HF(aq) + K+(aq) K+(aq) + H2O(1) - 11 of 65 > Calculate either...
6) Which of the following statements is true? A) If Q = K, it means the reaction is not at equilibrium B) If Q< K, it means the forward reaction will proceed (to the right) to form more reactants. C) If Q< K, it means the reverse reaction will proceed (to the left) to form more reactants. D) If Q> K, it means the forward reaction will proceed (to the right) to form more reactants E) If Q> K, it...
7) Which one of the following is the weakest acid? A) HF (Ka = 6.8 × 10-4) B) HClO (Ka = 3.0 × 10-8) C) HNO2 (Ka = 4.5 × 10-4) D) HCN (Ka = 4.9 × 10-10) B) 5.7 x 10–2 M D) 2.9 x 10–3 M 22) Calculate the hydrogen ion concentration in a solution of iced tea with lemon having a pH of 2.87. A) 2.9x10–2M D) 2.9x10–3M B) 5.7 x 10–2 M E) 5.7 x 10–4...
1. Calculate the concentration of H3O+ for an aqueous solution with a pH of 1.2 A) 6.3 x 10-7M B ) 1.6 x 108 M. C) 1.0 x 10-14 M. D) 6.20 x 10-2 M E) 4.0 x 10-4M 2. Calculate the concentration of OH- for an aqueous solution with a pH of 13.8. A) 0.64 M B) 4.0 x 10-5M C) 1.5 x 10-5M D) 1.0 x 10-14 M E) 2.5 x 10-10 M 3. Which of the following...
please show work 11)2SO2(g) + O2(8) 2503(8) For the reaction at equilibrium, ifO2 is removed, the amount of SO2 present 2 is removed, the amount of SO2 present will 11) A) decrease B) increase C) stay the same 12) According to the Arrhenius concept, if HNOs were dissolved in water, it w A) a source of Hions. B) a source of hydroxide ions. C) an acid. D) a base. E) a proton acceptor. vater, it would act as12) 13) The...
Q(38) What is the pH of a 0.0200 M aqueous solution of HF (K. of HF is 6.8 A) pH=14 B) pH=2.4 C) pH 47 D) pH=9,3 10 ) E) pH=12,6 Q(39) What is the pH of a 0.1 M aqueous solution of NH3 (Ko of HF is 1.8 * 10-5)? A) pH=14 B) pH=2.4 C) pH 6.7 D) pH=11.3 6) pH=12.6 Q(40) Aqueous metal ions behave as Lewis acids because they A) can readily accept electrons in their vacant...
Explain the process of how to get the answer. The answer is highlighted. Ch. 18 Values The following values will be useful for problems in this chapter. Acid Substance or Species HF HNO2 CH3COOH HOCI HOBr HOCN HCN H2SO4 KA = 7.2 x 10-4 Ka = 4.5 x 10-4 Ka = 1.8 x 10-5 Ka = 3.5 x 10-8 = 2.5 x 10-9 K4 = 3.5 x 10-4 Ka = 4.0 x 10-10 Kai = very large Kq2 = 1.2...
Calculate the percent ionization of hydrofluoric acid, HF, in a 0.600 M solution. (K for HF - 6.6 x 10-4) HF(aq) + H2O(l) = H30*(aq) + F(aq) O 3,3% O 42% O 6.0% O 2.1% 9.1%
A) H20 c) нсоз- E) H2CO3 DOH. 22) Which of the following statements correctly describes the hydronium-hydroxide balance in the given solution? A) In acids, [OH-] is greater than [H3O* B) In bases, [OH-]- [H3o*]. C) In neutral solutions, [H3O"] = [H20]. D) In bases, [OH-] is greater than [H3o*]. E) In bases, [OH-] is less than [H30*]. 23) Which of the following is a buffer system? A) NaCl(aq) and NaNO3(aq) C) H2CO3(aq) and KHCO3 (aq) E) H20(0) and HCl(aq)...