Concept explainers
Write a balanced equation for the neutralization of each of the following:
a.
b.
c.
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Basic Chemistry
- Hydrazine, N2H4, can interact with water in two steps. N2H4(aq) + H2O() N2H5+(aq) + OH(aq) Kb1 = 8.5 107 N2H5+(aq) + H2O() N2H62+(aq) + OH(aq) Kb2 = 8.9 1016 (a) What is the concentration of OH, N2H5+ and N2H62+ in a 0.010M aqueous solution of hydrazine? (b) What is the pH of the 0.010M solution hydrazine?arrow_forwardFor each of the following cases, decide whether the pH is less than 7, equal to 7, or greater than 7. a. 10. mL of 0.25 M propanoic acid, CH3 CH2 CO,H is mixed with 10. mL of 0.25 M NAOH. The pH of the solution is less than 7. The pH of the solution is equal to 7. O The pH of the solution is greater than 7. b. 90. mL of 0.45 M HCIO is mixed with 90. mL of 0.45 M NaOH. The pH of the solution is less than 7. The pH of the solution is equal to 7. O The pH of the solution is greater than 7. c. 55 mL of 0.35 M HNO3 is mixed with 55 mL of 0.35 M NaOH. O The pH of the solution is less than 7. O The pH of the solution is equal to 7. O The pH of the solution is greater than 7.arrow_forwardMg(OH)2 + 2 HCI -> MgCl2 + 2 H20 Use the balanced chemical equation to calculate the mass and volume of 0.99 M hydrochloric acid required to neutralize 750.0 mg of magnesium hydroxide.arrow_forward
- a. What is the pOH of an aqueous solution of 0.483 M hydrochloric acid?pOH =______ b. What is the hydronium ion concentration in an aqueous nitric acid solution that has a pOH of 9.200?[H3O+] = _______Marrow_forwardA solution with a pOH of 11.70 has an [H+] of a. 5.0 × 10−3 M.b. 3.2 × 10−4 M.c. 2.0 × 10−12 M. d. 2.30 M.arrow_forwardA solution containing only Ba(OH) 2 in water has a pH of 13.9. What is the molar concentration of barium hydroxide in the solution? a. 1.4 M b. 0.70 M c. 0.040 M d. 0.40 M e. 0.020 Marrow_forward
- A. What is the pH of an aqueous solution with a hydrogen ion concentration of [H+]=7.2×10−5[H+]=7.2×10−5 M? B. What is the hydroxide ion concentration, [OH−][OH−], in an aqueous solution with a hydrogen ion concentration of [H+]=7.2×10−5[H+]=7.2×10−5 M? C. A monoprotic weak acid, HAHA, dissociates in water according to the reaction HA(aq)↽−−⇀H+(aq)+A−(aq)HA(aq)↽−−⇀H+(aq)+A−(aq) The equilibrium concentrations of the reactants and products are [HA]=0.120 M[HA]=0.120 M, [H+]=3.00×10−4 M[H+]=3.00×10−4 M, and [A−]=3.00 ×10−4 M[A−]=3.00 ×10−4 M. Calculate the ?aKa value for the acid HA.arrow_forwardA solution with a pOH of 10.70 has an [H +] of a.2.0 × 10−12 M. b.5.0 × 10−4 M. c.3.2 × 10−4 M. d.0.36 M. e.5.0 × 10−3 M.arrow_forwardButyric acid is responsible for the odor in rancid butter. A solution of 0.25 M butyric acid has a pH of 2.71. What is the Ka for the acid? a. 7.8 × 10-3 b. 1.5 × 10-5 c. 0.36 Od. 2.4 × 10-2 Oe. 1.9 × 10-3arrow_forward
- What is the H+ion concentration of 8.8 x 10–4M Sr(OH)2 solution? a 8.8 x 10–4M b 2.2 x 10–11M c 1.8 x 10–3M d 7.8 x 10–12M e 1.1 x 10–11Marrow_forwardAt 25 degrees Celsius, what is the hydronium ion concentration in 0.100 M sodium chloroacetate? O a. 3.17 x 10-8 M O b. 1.17 x 10 8 Marrow_forward2. H₂SO4 solution is prepared by dissolving 4.9 grams of H₂SO4 in 100 mL of water. How many H₂SO4 molecules are in this solution? What is the molarity of the solution? What is the pH of the solution? d. What is the pH of the solution if 3.0 grams of NaOH is added to the solution? a. b. C.arrow_forward
- Chemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning