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Calculate the pH of the following aqueous solutions at
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Chapter 16 Solutions
Chemistry
- Determine the pH of the solution resulting from mixing a solution of 154 mL of HNO2 (Ka = 5.62e – 04) at a 1.800 M concentration, with 115 mL of a 1.400 M solution of C'sOH ? O (a) 3.250 O (b) 1.696 O (c) 3.392 O (d) 3.192 O (e) 0.308arrow_forwardDetermine the pH of the solution resulting from mixing a solution of 153 mL of CH₂BrCOOH (Ka = 1.26e - 03) at a 1.540 M concentration, with 136 mL of a 1.380 M solution of KOH? O (a) 0.317 (b) 3.492 (c) 2.492 (d) 1.746 O (e) 2.900arrow_forward7. Aniline (C6H5NH2) has a Kb of 3.8 x 10-10. What is the pH of a 0.150 M aniline solution? (a) 5.12 (b) 8.88 (d) 13.18 (c) 9.42arrow_forward
- What is the pH of a 0.40 M solution of benzoic acid,C6H5COOH? (The Ka value for benzoic acid is given inTable )(a) 2.30 (b) 2.10 (c) 1.90 (d) 4.20 (e) 4.60arrow_forwardFor which of the following solutions must we consider the ionization of water when calculating the pH or pOH?(a) 3 × 10−8 M HNO3(b) 0.10 g HCl in 1.0 L of solution(c) 0.00080 g NaOH in 0.50 L of solution(d) 1 × 10−7 M Ca(OH)2(e) 0.0245 M KNO3arrow_forwardIf the household water source has a tenfold decrease in H+ concentration from its initial value of pH 6.5, what is the new pH of the water source? (A) 3.5 (B) 7.5 (C) 5.5 (D) 7.5 (E) 7.0arrow_forward
- What is the pH of a 0.65 M solution of pyridine, C5H5N? (a) 4.48 (b) 8.96 (c) 9.52 (d) 9.62 (e) 9.71arrow_forward9. What is the pH of a solution whose hydronium ion concentration is 2.5 X 10-8 M? (a) 7.6 (b) 8.0 (c) 2.5 (d) 6.4 (e) 6.0 10. An aqueous solution has a pOH of 9.35, this solution is: (a) Neutral (b) Basic (c) Acidic (d) Impossible - this pOH cannot be reached in an aqueous solution (e) More information is needed. 11. Which is the strongest acid in the provided table below? Acid Acetamide 2-Pyridinamine Alloxanic Acid (a) Acetamide (b) 2-Pyridinamine (c) Alloxanic Acid (d) 4-chlorophenol (e) Quinoxaline pka 0.63 6.82 6.64 4-chlorophenol 9.18 Quinoxaline 0.56 avods rollorarrow_forwardIf the pH of a solution is equal to 3, the hydroxide ion concentration is _____. (A)1 x 1O11 M(B)1 x 103 M(C)1 x 10-3 M(D)1 x 10-11 Marrow_forward
- Which of the following statements describes a strong acid? (Select all that apply) The Ka is very small. Dissociates completely into ions in water. Is a strong electrolyte. Have a strong conjugate base.arrow_forwardCalculate the pH of solutions having the following [H+]: (a) 0.68 M (b) 1.42 M (c) 4.5 × 10-5 Marrow_forwardWhich of the following statements is true? (Select all that apply.) In an acid solution, K₂ = [H3O*]. Consider 1.0 M acidic solutions of the imaginary acids, HA, HB and HC and the 1.0 M salt solutions NaA, NaB, and NaC. If HA has the lowest pH, then 1.0 M NaA would have the highest pH. Ka of an acid multiplied by the Kb of its conjugate base equals Kw. The stronger the base, the weaker its conjugate acid. None of these are true.arrow_forward
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