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Practice Problem ATTEMPT
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Chemistry
- What is the pH of a 0.25 M solution of H3PO4? Ka = 7.2 x 10-³ (A) 0.25 (B) 7.2 x 10-3 (C) 0.0018 (D) 0.042 (E) 1.37arrow_forwardCalculate the percent ionization of ascorbic acid (HC6H7O6) in solutions of each of the following concentrations (Ka = 8.0e-05.)(a) 0.114 M (b) 0.438 M (c) 0.869 Marrow_forwardWhich of the following reactions go to completion? (Select all that apply.) O Autoionization of water Strong acid-strong base neutralization reaction O Strong base dissociation in water Weak acid dissociation in water O O Oarrow_forward
- Which of the following statements is/are true? (Select all that apply) OThe higher the concentration of OH in a solution, the lower the pH. OThe higher the concentration of OH in a solution, the lower the pOH. O An acidic solution has a pH of geater than 7. The concentration of H30* in pure water is 1.00 x 107 M. OA Bronsted acid is a proton donor in an acid-base reaction.arrow_forwardWhich of the following 0.10 M acid solutions is expected to have a lower pH than 0.10 M CHBr₂COOH? (Select all that apply.) Structure of CHBr₂COOH [] n n [] Br Br :0 th Br Br CI -C Br -ő- H J16-Ō o=0: CI [4. the -H Br th H C H o=0: :0=0 0=0: o=0: :0: :0: 44 H the H H -Ö-Harrow_forwardWhat is the pOH of a solution of 0.125 M CH3NH2 and 0.130 M CH3NH3Cl? How would you find a Ka value? Calculate [OH-], [H+], and pH for practicearrow_forward
- EXERCISE II -11 1. A chemist,, Hishes to prepare 100.0 mL of a buffer of pH 10.0000 using the base methyl amine, CH,NH2, ánd its salt, CH;NH2, and its salt, CH3NH;CI. (a) What should be the ratio of base to salt to obtain a pH of 10.00? (b) If he makes the solution 0.05000 M CH3NH2, how many moles of methyl ammonium chloride should he add to get the desired pH ? Kp = 5.00 x 104 2. A buffer solution is prepared by dissolving 4.7 g of nitrous acid, HNO2 , and 13.8 g of sodium nitrite, NaNO2, in 1.0 liter of solution. (a) Calculate the pH of the buffer. (b) Calculate the pH of the solution which results when the following are added to separate 100 mL portions of the buffer: (i) 5.0 mmol of HCI; (ii) 5.0 mmol of NaOH. Ka = 4.5 x 104 %3D 3. What change in pH will occur when 0.050 mmol of HOAC (Ka= 1.78 x 10) is added to 100.0 mL of a buffer solution that is 0.1000 M HOAC and 0.1000 M NAOAC? Assume no change in volume.arrow_forward10. Ammonia (NH3) has base dissociation constant (K) of 1.8 x 10-5. What is the concentration of an aqueous ammo- nia solution that has a pH of 11.68? (LO 16.11) (a) 0.28 M (b) 3.6 M 1.3 M (c) 9.0 x 10-3 M 711 ***arrow_forwardPractice Exercise Calculate the concentration of OH ions in a HCl solution whose hydrogen ion concentration is 1.3 M.arrow_forward
- practice pH a.) determine the pH of a nitric acid solution (HNO3) that has been prepared by mixing 2.0 mL of 1.0 M HNO3 with 98.0 mL of water b.) determine the pH of a 25 mL carbonic acid solution (H2CO3) with concentration of 5.7 x 10-5 M. assume all protons will dissociate from the acid and react with water to form hydronium ions. c.) determine the pH and pOH of a NaOH solution that has been prepared by diluting 20.0 mL of 6.0 M NaOH with 80.0 mL of water. d.) determine the pH and pOH of a Ca(OH)2 solution that has been prepared by mixing 0.26 g of Ca(OH)2 pellets in 750 mL of water.arrow_forwardPRACTICE EXAMPLE A: Explain which is the stronger acid, HNO3 or HClO4; CH₂FCOOH or CH₂BrCOOH. [Hint: Draw plausible Lewis structures.] PRACTICE EXAMPLE B: Explain which is the stronger acid, H3PO4 or H₂SO3; CC13CH₂COOH or CCl₂FCH2 COOH. [Hint: Draw plausible Lewis structures.]arrow_forwardExercise 1 Calculate the pH of each of the following solutions: (a) 0.63 M NaCH3CO2(aq), K, = 5.62 × 10-10, %3D (b) 0.19 M NH4CI(aq), K, = 5.6 × 10-10; %3D (c) 0.65 M KCN(aq), K½ = 2 × 10-5.arrow_forward
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