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Answer: 29) Consider the following generalized buffer solution equilibrium: When a small amount of a strong base such as sodium hydroxide is added to the solution, which of the four species shown would experience an increase in concentration? A) BH B)H C) HO D)B E None of the species would increase in concentration. Answer: ( 30) What is true about a solution whose pH is less than 7 at 25°C? A) It has a hydronium ion concentration less than 1 x 10-M B) It has a hydronium ion concentration that is higher than pure water itself C) It has a hydroxide ion concentration equal to its hydronium ion concentration. D) It is a solution that requires a buffer E) is a basic solution. Answer:( 31) A particular buffer solution consists of a weak acid and its conjugate base. How could this buffer solution be modified so as to increase its buffer capacity against added base? A) Increase the concentration of the weak acid C) Use a strong base and its conjugate acid instead. D) Use a strong acid and its conjugate base instead. E) Make the concentrations of the weak acid and its conjugate base equal. B) Increase the concentration of its conjugate base. Answer: ( 32) Fomic acid (HCO:H) is a weak acid found in the venorn of bees and ant stings. an accurate statement conceming Which of the following is an aqueous solution of fomic acid? A) The reaction between formic acid and water is slow, due to the low value for K B) A formic acid solution predominantly contains undissociated HCO:H molecules. C) A formic acid solution predominantly contains H:O and HC02 ions. D) A formic acid solution contains a greater concentration of dissolved ions than it does neutral formic acid molecules. E) A formic acid solution contains equal amounts of H O and HCO H Answer: ( 33) HCl is a strong electrolyte. A bottle of HCl contains the label 0.015 MHC(a). Which statement concerning this HCI solution is FALSE? A) The solution is acidic. B) The pH of the solution is 1.5. C) The hydronium ion concentration in this solution is 0.015 M. D) The solution has a higher concentration of hydronium ions than hydroxide ions. E) The solution contains dissolved HO and Cl ions only; no HCl molecules are present Answer: ( 34) An aqucous solution with a low pH is necessary for a certain industrial process. Which of the following solutions would have the lowest pH? A) 2.0MNaOH B) 0.5 M HCI C1.0 M acetic acid D) 1.0 M HCI E) All solutions would have the same pH. Answer: 35) A 50-mL buffer solution has an initial pH of 8.78. Ifa student adds 5 drops of HCl to this solution, what would be a reasonable pH for the resulting solution? A)-1.78 B1.78 C)8.64 D)8.78 E) 8.89 Answer: ( 36) Which one of the following is not a strong acid? (or a weak electrolyte?) a) HNO b)HC d) HF e)HCI0 Answer ( 37) The species that remains after an acid donates a proton is called its conjugate base. What is the conjugate base of the hydronium ion, HO? A) OH B)H:O C)H:O D)HO E) H O has no conjugate base. Answer. 38) For the reaction shown below, which of the following is a conjugate acid-base pair? A) CsHsN, H O B)CsHSN, CsH$NH C)CSHSNH, OH D)H O, OH E) Both B and D Answer. ( 39) Which of the following statements concerning acids and bases is TRUE? A) All Bronsted-Lowry bases contain hydroxide B) All Bronsted-Lowry bases contain hydronium. C) A pH of 0 is considered neutral D) The pH of a 12.0 M solution of HCl is-1.1 E) All buffer solutions operate at a pH at or near 7 Answer. 40) Which one of the following combinations can function as a buffer solution? C) HNO, and NaNO A) HCI and KCI E) KHSOs and H SO B) NaHCO, and H:CO D) HC104 and NaCIO Answer ( II) Problems 41) Which of the following solutions can act as a buffer? (a) KCVHC: (b) KHSO/H:SO (c) Na HPO/ Nall: PO4 (d) KNO HNO2 42) Classify each of the following species as a weak or strong acid (a) HNO, (b) HF, (c)H SO, (d HSO, (e)HCOHCO, (g) HC, (h) HCN, () HNO 3) What is the HO concentration to the correct number of significant figures for solutions with the following pH values? (a) 0.00 b) 7.00 (c)-0.20 (d) 15.18 (e)263 ( 10.756 (g)-0.42 (h 1.21 (i) 6.96 44) Calculate the pH of each of the following solutions (a) 0.0010MHCI (b) 0.16 M KOH; (c) 0.88 M NaOH:

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