4. Identify the conjugate acid of S042 A) H:SO4 B) HSQF C) H3SO3 D) H3O+ E)...
What is the OH ion concentration in a 4.8 x 10-2 M KOH solution? 2.1 x 10-13 M 4.8 x 10-2 M 1.0 x 10-7 M 4.8 x 10-12 M What is E' for the following balanced reaction? Fe(s) + Cu2+(aq) Fe2+ (aq) + Cu(s) Standard Reduction Potential Half-reaction Fe2+ (aq) + 2e Fe(s) Cu2+ (aq) + 2e Cu(s) -0.44 40.34 O +.010 +0.78 0 -0.78 -0.1
Calculate either [H3O+] or [OH-] for each of the solutions. Solution A: [OH") - 3.25 x 10-7M Solution A: [H,011- M Solution B: [H, O'] = 7.75 x 10-M Solution B: [OH-]= M Solution C: [H, 0+1=6.43 x 10 M Solution C: [OH-= M Which of these solutions are basic at 25 °C? A: [OH-] = 3.25 x 10-7M B: [H0+1= 7.75 x 10-'M C: [H,0+) = 6,43 x 10 M What is the pH of an aqueous solution with...
2,6,7 For which type of titration will the pH be acidic at the equivalence point? 6. Identify the correct conjugate acid-base pairs in the reaction HSO+HF HaSO+ P A) Strong acid vs. strong base, B) Strong acid vs. weak base. C) Strong base vs. weak acid D) None of the above. A) HF/ HSO B) F/HSO C) HSO HaSO D) Not enough information 2. What is the OH ion concentration in a 5.2 x 10 M HNO3 solution? 7. A...
9) What is the H+ ion concentration in a 4.8 x 10–2 M KOH solution? A) 4.8 x 10–2 M B) 1.0x 10–7 M C) 2.1 x10–13 M D) 4.8 x 10–11 M 10) HA is a weak acid. Which equilibrium corresponds to the equilibrium constant Kb for A-? A) HA (aq) + H2O (l) H2A+ (aq) + OH-(aq) B) A- (aq) + H3O+ (aq) C) HA (aq) + OH- (aq) H2O (l) + H+ (aq) HA (aq) + H2O...
11. Which Brønsted-Lowry base has the strongest conjugate acid? A) CH.COM B) CN- C) F- D) NOZ E) CIO 12. Which Brønsted-Lowry acid has the strongest conjugate base? A) HBr B) HCIOC) HFD) HI E) HNO3 13. Calculate the H30+ concentration in an aqueous solution that contains 2.50 x 104 M in OH-. A) 4.00 x 10-'M B) 4.00 10-10M C) 4.00 10-11 M. D) 5.00 10-11 M E) None of these 14) What is the pH of a 0.020...
Question 2 (1 point) A solution is made by dissolving 0.0112 g KOH in enough water to make 1.0 liter of solution. What is the H+ ion concentration of this solution? O2.0 x 10-3M 5.0 x 10-12 M O 1.2 x 10-13 M 5.0 x 10-11 M 8.0 x 10-2M Olection 3.11 nointi
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...
1. Identify the Brönsted acid and base in the following reaction, and identify the conjugate base and acid formed. HSO3-(aq) + CH3NH3(aq) ------ H2SO3(aq) + CH3NH2(aq) 2. Write the formulae for the conjugate acids of: 1. a) C2042: the oxalate ion. 2.b) C6H5NH2, aniline. 3.c)NH2OH, hydroxylamine. (Use above question as a guide for where to put the H.) 3. Calculate the molarity of OH' in solutions with the following concentrations of H30*: a) 0.020 mol LP b) 1.0 x 10-5...
Calculate the concentration of H3O for an aqueous solution with a pH of 6.20. A) 6.3 x 10-7 M E) 4.0 x 10 M 1. B) 1.6 x 10 M C) 1.0x 10-14 M D) 6.20 x 1014 M 2. The pH of a 0.010 M aqueous solution of Ca(OH)2 is A) 11.70 B) 12.00 C) 12.30 E) 1.70 D) 12.60 alution with a nH of 9.60. for an aqueous solution with a pH of 9.60. C) 1.5 x 10-5...
(d) Conjugate acid: OH"; conjugate base: H3* (e) None of these 5. Identify the conjugate acid/base pairs in the following equation (10) HASO4 + H2O <H2AsO4 + OH (A). HASO. (acid)HAsO4 (base): H2O (acid)/ OH (base) (B). HASO4 (acid)/HASO. (base): H2O (acid)/ OH (base) (C). H2AsO4 (acid)/ OH (base) ; H2O (acid)/HASO4 (base) (D). H AsO4 and H20 (acids): OH and HASO4(bases) (E). None of these 6. Which is an INCORRECT statement?(10) a) The conjugate base of H2O is OH....