10. What is the pH of an aqueous solution of (sodium hypochlorite) that is 0.0 (Hint...
Household bleach is a solution of sodium hypochlorite. What is the pH of an aqueous solution that is 4.73-% NaClO by mass? (The density of the solution is 1.0 g/mL, and Kb = 2.9 × 10−7)
The pH of an aqueous solution of 0.282 M sodium hypochlorite, NaClO (aq), is ________. ACIDIC OR BASIC OR NEUTRAL?
What is the pH of a 0.255 M aqueous solution of sodium hypochlorite, NaClO? (Ka for HClO = 3.5×10-8)
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...
a. The pH of an aqueous solution of 0.272 M potassium hypochlorite, KClO (aq), is: __________ is this solution acidic/basic/neutral? b. The pH of an aqueous solution of 0.274 M sodium cyanide, NaCN (aq), is: __________ is this solution acidic/basic/neutral?
Predicting pH
Imagine you have a 0.125 M aqueous solution of aspirin, an acid drug with pKa = 3.5, in equilibrium. a) Estimate the pH of the solution Hint: Determine if it is an acid or base solution, weak or strong If weak acid/base, first try (H+) = /K,C, or [OH-] = K,C, b) Predict what would happen to the pH when you add more H2 Hint: First figure out what happens to the concentrations HA(aq) + H2O(0) A (aq)...
1" . I TV a OH Imagine you have a 0.125 M aqueous solution of aspirin, an acid drug with pKa = 3.5, in equilibrium. a) Estimate the pH of the solution Hint: Determine if it is an acid or base solution, weak or strong If weak acid/base, first try [H+] = VK.C, or [OH-] = /K,C, b) Predict what would happen to the pH when you add more H20 Hint: First figure out what happens to the concentrations HA(aq)...
10. For an aqueous solution labeled "0.10 M potassium bromide," A) the pH is greater than 7. B) the pH = 13. D) the pH is less than 7. E) the pH = 7. C) the pH = 1. 11. For a 0.10 M solution of a weak acid, HA, with pKa = 6, which of the following is true? A) [HA] =[A-] B) [HA] does not equal [H3O+] C) [HA] =[H3O] D) [HA] = K E) [HA] = 0...
a OH Old Exam Question Example #2 Imagine you have a 0.125 M aqueous solution of aspirin, an acid drug with pk, = 3.5, in equilibrium. a) Estimate the pH of the solution Hint: Determine if it is an acid or base solution, weak or strong If weak acid/base, first try (H*] = KC, or [OH-] = K,C, b) Predict what would happen to the pH when you add more H20 Hint: First figure out what happens to the concentrations...
A. What is the pH of an aqueous solution with a hydrogen ion concentration of H 20 x 10-'M? pH = B. What is the hydroxide ion concentration, OH"), in an aqueous solution with a hydrogen ion concentration of (H) = 2.0 x 10-'M? [OH-] = C. A monoprotic weak acid, HA, dissociates in water according to the reaction HA(aq) H(aq) + A+ (aq) 3.00 x 10-M, and The equilibrium concentrations of the reactants and products are (HA) = 0.140...