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- 35 of 44 > A monoprotic weak acid, HA, dissociates in water according to the reaction HA(aq) + H,O(1) = H,O*(aq) + A (aq) The equilibrium concentrations of the reactants and products are (HAJ = 0.270 M. [H,O*] = 3.00 x 10 M, and |A] = 3.00 x 10 M. Calculate the K, value for the acid HA. K, =What is the pH of the solution when Henry has added 35.00 mL of 0.50 M NaOH to the 50.00 mL of 0.25 M nitrous acid? KaHA = 4.0 x 10-4 pH = [?] PH Enter4. Complete neutralization of 10 mL of hydrochloric acid solution by NaOH 0.1 N in the presence of phenol phthalein until the appearance of purple color (pHf= 9) 15 mL of NaOH is consumed. (a) What is the concentration of hydrochloric acid? (b) Calculate the indicator error.
- Determine the pH of (a) A 0.10 M CH3COOH solution (ICE) (b) A solution that is 0.10 M CH3COOH and 0.10 M CH3COONa. Ka for CH3COOH = 1.8 X 10-5.5:50 1 Search Question 5 of 20 Submit Determine the mass of solid NaCH;COO that must be dissolved in an existing 500.0 mL solution of 0.200 M CH3COOH to form a buffer with a pH equal to 5.00. The value of Ka for CH-COОH is 1.8 х 10-5. 1 2 Let x represent the original concentration of CH;COO in the water. Based on the given values, set up the ICE table in order to determine the unknown. CH3COOH+ H20(1) =H;O*(aq) +CH3COO-(a Initial (M) Change (M) Equilibrium (M) 5 RESET 0.200 5.00 -5.00 1.0 x 10-9 -1.0 × 10-9 1.0 x 10-5 -1.0 x 10-5 1.8 x 10-5 -1.8 x 10-5 х+ 5.00 x - 5.00 x + 1.0 × 10-9 х - 1.0 х 10-9 1.0 x 10-5 x - 1.0 × 10-5 x + 1.8 × 10-5 х - 1.8 х 10-5"For H3PO4, Kaj = 7.3 x 103, Kaz = 6.2 x 106, and Kaz = 4.8 x 10-13. An aqueous solution of NaH2PO4 therefore would be" neutral basic O acidic Which anion will not form any precipitate to either AGNO3 or BaClz solution? O CH3CO0 NO3 O so? SCN All of the following anions will precipitate out in the presence of AgNO3 EXCEPT: PO O co3 CH3C0
- Calculate the change in pH that occurs when 1.10 mmol of a strong acid is added to 100. mL of the solutions listed below. Ka (CH3COOH) = = 1.75 x 10-5 a. 0.0680 M CH3COOH. Change in pH = b. 0.0680 M CH3COONa. Change in pH =Part 3 - Put it all together. Calculate the concentrations of all species in a 0.690 M Na, So, (sodium sulfite) solution. The ionization constants for sulfurous acid are Ka = 1.4 x 102 and K = 6.3 x 108. !! [Na*] = 1.38 [SO] =| 0.690 [HSO,] = - TOOLS x10 [H,SO,] = [OH ] = M. %3D [H*] =6. A buffer solution is formed by adding 0.500 mol of sodium acetate (CH3CO2NA) and 0.500 mol of acetic acid (CH3CO2H) to 1.00 L H,0. What is the pH of the solution at equilibrium? (K, = %3D 1.8 x 10°)
- The strong acid HI is added to 0.1 M/0.1M CH3COOH/CH3COONa. What is the full reaction equation, full ionic equation, and net ionic equation for the reaction that will occur? Thank you so much im really lost.A solution is made initially with 0.200 M HIO3 (Kc = 0.170). Once the equilibrium below is established, what is the equilibrium concentration of H+ ions? HIO3 (aq)=H+ (aq) + 103 (aq) + + esc F2 72 C MAR 20 80 F3 #3 000 F4 $ 14 4 MacBook Air F5 F6 % alo5 666 tv & 7 WERTY F7If 31.4 mL of a 0.75 M NaOH solution is added to a 47.1 mL sample of a 0.75 M weak acid, HA, what is the pH of the resulting solution? (K. = 1.8 x 10-) pH=