Calculate the pH at 25 °C of a 0.32M solution of potasslum acetate (KCH,CO,). Note that acetic acid (HCH,CO,) Is a weak acid with a p K, of 4.76. Round your answer to 1 decimal place. pH =
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Q: The acid dissociation constant K, of alloxanic acid (HC,H,N,0,) is 2.24 × 10 '. Calculate the pH of…
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- Calculate the pH at 25 °C of a 0.46 M solution of potassium butanoate (KC,H,CO,). Note that butanoic acid (HC,H,CO,) is a weak acid with a pK, of 4.82. Round your answer to 1 decimal place.In the laboratory, a general chemistry student measured the pH of a 0.589 M aqueous solution of phenol (a weak acid), C6H5OH to be 4.997. Use the information she obtained to determine the K₂ for this acld. Ka(experiment) = Submit Answer $ 4 R LL F F4 % 5 A T Retry Entire Group 9 more group attempts remaining G Cengage Learning Cengage Technical Support F5 A 6 MacBook Air S Y H & 7 ◄◄ F7 U J * 00 8 ► 11 F8 L ( 9 K F9 O 1 0 L F10 P 4) Previous Next F11 + = Save and F12 8Ascorbic acid (H₂C,H,O) is a diprotic acid. The acid dissocation constants for H₂C,H,O, are Kal = 8.00 x 10-5 and K₁2 = 1.60 x 10-12 Determine the pH of a 0.117 M solution of ascorbic acid. pH = Determine the equilibrium concentrations of all species in the solution. [H₂C,H,O,] = [HC,H,O,]= [C,H,O2] = M M M
- Calculate the pH at 25 °C of a 0.13M solution of trimethylammonium chloride ((CH;) NHCI 3 CH;),NHC!) Note that trimethylamine ((CH3),N) i is a weak base with a pK, of 4.19. b. Round your answer to 1 decimal place.3. A 0.0560 g quantity of acetic acid is dissolved in enough water to make 50.0 mL of solution. Calculate the concentrations of H;O*, CH;COO and CH;COOH at equilibrium. What is the pH of the solution? (Ka = 1.8x10) CH;COOH(aq) = CH;COO (aq) + H;O* (aq) a) Calculate the initial concentration of CH;COOH. (C:12; H:1; 0:16) b) Calculate the concentration of CH;CoO (aq) and H;O* (aq) at equilibrium. c) Calculate pH of the solution.Calculate the pH at 25 °C of a 0.15M solution of lidocaine HC1 (C4H2,NONH,CI). Note that lidocaine (C14H2,NONH) is a weak base with a p K, of 7.94. Round your answer to 1 decimal place. pH = | olo Ar
- 3. In biology, evergy is stored as adenosime triphosphate (ATP or ATP+). When this compound hydrolyses, a leturns to its low energy form, adenosine diphosphate (ADT, or ADT¹"): 3- 4- ATP ² (aq) + H₂O → ADP + HPO₂²² + H₂O + and Gran AG At 37°C and pH=7₁0, AH₂ = -20 kJ. Mol" 31 RJ.mol" for this process. (a) How much non-expansion work is ducilable per mole of ATP hydrolysed. ? (2) ($) Calculate and explain the sign of (3) AS rxn for this process at 37°C and pte=7What is the pH of a grapefruit that contains 0.007 M citric acid solution (CsH2O-)? CH;O;(aq) + H;O(2) = CH;0, (aq) + H3Oʻ(aq) K, = 7.5 x 104 Round your answer to 2 decimal places.2 2- 3c₂²- 1 W Write the acidic ionization equation for HCI. Be sure to include the proper phases for all species within the reaction. + radditional resources OH- 3 E 2 $ 4 H3O* 3 R % 5 Reset 4 T (1) Question 16 of 28 ^ H₂O 6 5 6 Y & 7 H U (g) * 00 8 7 →> 1 ( 9 8 CI O ) O 9 (aq) • x H₂O P
- Important equations Attach additional paper, if necessary, to show complete work Indicate which problems you have worked out on a separate sheet of paper [HJOH)=K1.00 x 10" (at 25 "C) pH=- log (H) pOH- log (OH) pH+ pOH- 14.00 Moroo K- IHAJ ort 1. Determine the phi of 0.055 M oxalic acid (HCO, K. -5.6x 10' and K-54x 10). Note: both steps are important here, therefore we have to set up two "ICE boxes 2. Nicotine, CHN, is a base that will accept two protons (K,7x 10, K 14x 10"). What is the pH and the concentration of each species present in a 0.010 M solution of nicotine?10. Calculate the pH of a solution of CH3NH2(aq) Methylamine, Kb = 4.3x104 that has an initial concentration of 0.20 M? Is it acidic, basic, or neutral solution?Elc. A JU student was asked to prepare a pH = 4.0 acid solution in which the molarity of H is 1.0 x 10-4 M. The only acid that is available is sulfuric acid, H2SO4. Assume that H2SO4 (1) will completely dissociate according to Eq. 1. H2SO4 (aq) S0 (aq)+2H* (aq) First, the student transferred 1.500 mL pure H2SO4 into a volumetric flask and made 200.0 mL solution (solution 1). The density of pure H2SO4 is 1.84 g/mL. Then he transferred exactly 10.00 mL solution 1 with a pipet into another volumetric flask and made 250.0 mL solution (solution 2). Please calculate the molarities of both solutions for him. If he can solve this problem correctly, it will prove to his supervisor he has necessary skills.