A sample of lake water at 25°C has a phenolphthalein alkalinity of 2× 104 M. Which of the following statements is true? OA. Bicarbonate ion (HCO3) concentration is 2 × 10-4 M. OB. Hydrogen ion concentration is 2 x 10-4 M. OC Carbonate ion (CO32) c (CO32) concentration is 2 × 10-4 M. OD. Total alkalinity is 2 × 10-4 M

A sample of lake water at 25°C has a phenolphthalein alkalinity of 2× 104 M. Which of the following statements is true? OA. Bicarbonate ion (HCO3) concentration is 2 × 10-4 M. OB. Hydrogen ion concentration is 2 x 10-4 M. OC Carbonate ion (CO32) c (CO32) concentration is 2 × 10-4 M. OD. Total alkalinity is 2 × 10-4 M

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter16: Principles Of Chemical Reactivity: The Chemistry Of Acids And Bases

Section: Chapter Questions

Problem 73PS: Hydrazine, N2H4, can interact with water in two steps. N2H4(aq) + H2O() N2H5+(aq) + OH(aq) Kb1 =...

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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?
Does the pH of the solution increase, decrease, or stay the same when you (a) Add solid sodium oxalate, Na2C2O4, to 50.0 mL of 0.015-M oxalic acid? (b) Add solid ammonium chloride to 100. mL of 0.016-M HCl? (c) Add 20.0 g NaCl to 1.0 L of 0.012-M sodium acetate, NaCH3COO?
Even though Ca(OH)2 is an inexpensive base, its limited solubility restricts its use. What is the pH of a saturated solution of Ca(OH)2?
1. Nitrogen in an industrial wastewater is primarily in the form of ammonia (NH3) and ammonium (NH4+) ions. The acid/base equilibrium reaction for ammonia and ammonium is given as: NH4+ → H+ + NH3 Ką = 10-9.26 The total nitrogen concentration in wastewater is given as 2 x 10-3 moles/L (or 28 mg N/L), a. Calculate the concentration of ammonia (NH3) and ammonium (NH4*) ions at pH 10. NH3: moles/L NH4*: moles/L Check b. In ammonia stripping, nitrogen is removed from wastewater by volatilization of NH3. Would ammonia stripping be more effective above or below pH 9? Briefly explain your reasoning.
1a. Write out the reaction for acetic acid (CH3COOH) and water. 1b. Calculate the pH of a 0.15 M solution of acetic acid, which has a K₂ of 1.8 x 10 1c. What would happen to the pH of the solution if you added some sodium acetate (NaCH3COO) to it? Why? (Hint: NaCH3COO contains the conjugate base of CH3COOH) Describe how the acetate ion would interact with the reaction of acetic acid in water that you wrote in part A. 1d. If it was 0.10 M sodium acetate that was added in part C, what would be the new pH value?
pH Titration A student is titrating 150.0 mL of a 0.300 M solution of lactic acid (pKa of lactic acid is 3.85) with a 0.250 M solution of NaOH. Calculate the initial pH of the lactic acid solution, before any NaOH has been added. Round your answer to 2 decimal places. pH = Calculate the pH of the acid solution after the chemist has added 100.0 mL of the 0.2500 M NaOH solution to it. Round your answer to 2 decimal places. pH = Calculate the pH of the acid solution after the chemist has added 200.0 mL of the 0.2500 M NaOH solution to it. Round your answer to 2 decimal places. pH =
9. We prepared a solution containing 1.0 mol.L' HF and 1.0 mol.L·' C,H3OH. The K, of hydrofluoric acid and phenol are 7.2 x 104 and 1.6 x 10-10 respectively. What is the pH of this solution? (Hint: find which acid is strongest and make the appropriate assumptions) b. What is the concentration of C,H;O¯ at equilibrium? а.
A 0.050 M solution of the salt NaA has a pH of 9.00. Determine the [OH] and the pH of a 0.010 M solution of the acid HA. Show your work in the question parts below. Determine the equilibrium concentration of H3O* using the acid ionization equation. Recall that [OH] = 1.0 x 10-5. Consider the ionization equation described below.. HA(aq) + H20(1) =H;O*(aq) + A (aq) 1 Based on the given information, set up the ICE table in order to determine the unknown equilibrium concentration of all reactants and products. НА(ag) H20(1) H;O*(aq) А (ag) + Initial () Change () Equilibrium () 5 RESET 0.010 0.050 +x -2х +2x -x 0.010 + x 0.010 - x 0.050 + x 0.050 - x 0.010 + 2x 0.010 - 2x 0.050 + 2x 0.050 - 2x
A lake has been acidified to a pH of 4.418. If the lake has a volume of 1.48×105 cubic meters, what mass, in kg, of CaO must be added to raise the pH to a value of 7.00? CaO+H2O->Ca(OH)2
Consider hypoiodous acid (HOI). HOI (aq) ⇌ H+ (aq) + OI- (aq) pKa = 10.5 1. A solution of Ba(OH)2 is titrated into a solution of HOI. Calculate the volume of 0.140 M Ba(OH)2 (aq) needed to reach the equivalence point when titrated into a 56.0 mL sample of 0.194 M HOI (aq).2. Indicate whether the pH at the equivalence point is less than 7, equal to 7, or greater than 7. Explain.
Adding as little as 0.1 mL of concentrated HCl to a liter of H2O shifts the pH from 7.0 to 3.0. Adding the same amount of HCl to a liter of a solution that 0.1 M in acetic acid and 0.1 M in sodium acetate, however, results in a negligible change in pH. Why do these two solutions respond so differently to the addition of HCl?
A solution is prepared by adding 500 mL of 0.3 M NACIO to 500 mL of 0.4 M HCIO. What is the pH of this solution? Multiple Choice The pH will be equal to the pka of hypochlorous acid. The pH will be less than the pKa of hypochlorous acid. The pH will be greater than the pka of hypochlorous acid. The pH will equal the pkp of sodium hypochlorite. None of these chnices are correct