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- A solution of sodium cyanide, NaCN, has a pH of 12.10. How many grams of NaCN are in 425 mL of a solution with the same pH?24. A solution of volume 0.500 L contains 1.68 g NH3 and 4.05 g (NH4)2SO4. (a) What is the pH of this solution? (b) If 0.88 g NaOH is added to the solution, what will be the pH? (c) How many milliliters of 12 M HCl must be added to 0.500 L of the original solution to change its pH to 9.00?The pH of a 0.225 M weak acid solution, HA, is 4.05, what is the K, of the acid? НА (аq) + H,О (). H;O* (aq) +A ¨(aq)
- In which one of the following reactions does an H20 molecule behave as a Lewis base? O A. Na(s) + H20() = Na*(aq) + OH¯(aq) + ½ H2(g) O B. H20() + F (aq) = HF(aq) + OH-(aq) O C. H2O() + HCO3 (aq) = Co,²-(aq) + H3O*(aq) O D. 2H,0 = 2H2 + O2 O E. NH3(aq) + H2O() NH4*(aq) + OH(aq)Which of the following reactions is an acid-base reaction? A) AGNO:(aq) + KF(aq) → AgF(s) + KNO:(aq) B) NH:(aq) + HF(aq) → NH:"(aq) + -F(aq) C) NO: (aq) + AI(s) → NH3(g) + AIO: (aq) D) CH:(g) + 202(g) - 2H:O(g) + CO:(g)8) What is the pH of a 0.035 M HNO, solution? HNO3 (aq) + H,0 (1) H;O* (aq) + NO; (aq)
- What is the molarity of an NH4NO3(aq) solution that has a pH = 4.80? The K, for ammonia is 1.76E 5.The ionization constant of lactic acid, CH,CH(OH)CO,H, an acid found in the blood after strenuous exercise, is 1.36 x 10-4. What is the concentration of hydronium ion in the solution of 0.102 M lactic acid? CH;CH(OH)CO,H (aq) + H,O (1) → H;O• (aq) + CH;CH(OH)CO, (aq) O 0.00372 M O 0.0165 M O 0.00549 M O 0.227 MIn the following acid-base equilibria of weak acids in water, label the acid (A), the base (B), the conjugate acid (CA), and the conjugate base (CB). HCIO, (aq) + H,O(1) = H,O*(aq) + CI0, (aq) H,CO, (aq) + H,O1) – H;O*(aq) + HCO; (aq) Answer Bank H,O(1) + CH;NH†(aq) = CH,NH,(aq) + H;O*(aq) СА А B СВ CH, COOH(aq) + H,O(1) - CH;COO (aq) + H;O*(aq)
- 6. Acids and bases are defined by their donation or acceptance of a proton according to the (a) Arrhenius model. (b) Bronsted-Lowry model. (c) Lewis model.Calculate the hydronium ion concentration in an aqueous solution of 0.198 M carbonic acid, H,CO3 (aq). [H;O"]=[ M.The average blood pH is 7.40. The blood volume in humans, on average, is 5 liters. On average bicarbonate concentration in blood is 25 mM. A vinegar jar has a label that says its acetic acid concentration is 3.0%, meaning 3.0 g of acetic acid in 100 mL vinegar. (1) How many mL of vinegar does a person have to intake in order to lower the blood pH to 7.25? (2) if ALL the bicarbonate in 5.0 L of blood is neutralized by vinegar, how many mL of vinegar will be needed? (3) When all the bicarbonate ions are neutralized to carbonic acid, what will be the resulting blood pH? Note: pKa values for carbonic acid (diprotic acid) are 6.4 and 10.3, respectively.
