Special Instructions: Put the weak base (B) or weak acid (HB') species before the water species (H₂O & OH). (1) = (aq) + Kc Kb = Kc [ [ [₁ 11 ][ ][ [[ ] ]] ]][ (aq) + 1 (aq)
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- Complete the balanced chemical equation for the following reaction between a weak acid and a strong base. CH:NH:CI(aq) + NaOH(aq) 4- 2+ | ]3+ 1 3 4 6 7 8 D4 15 Do ) (s) (1) (g) (aq) Na H C CI Reset • x H2O Delete 1L 2. +The pH for 0.0850 M solution of CoHsCH2COOH is 2.68. Determine the value of Ka for CoHsCH2COOH. 1 NEXT > Based on the given values, fill in the ICE table to determine concentrations of all reactants and products. C&H:CH2COOH(a_ H2O(1) H;O*(aq) CoHsCH2CO0 (aq) q) Initial (M) Change (M) Equilibrium (M) RESET 0.0850 2.68 -2.68 2.1 x 10-3 -2.1 x 10 3 0.0829 -0.0829 0.428 -0.428 +x 2.68 + x 2.68 - x 2.1 x 10-3 + x 2.1 x 10-3-x 0.428 + x 0.428 xDetermine if the following salt is neutral, acidic or basic. If acidic or basic, write the appropriate equilibrium equation for the acid or base that exists when the salt is dissolved in aqueous solution. If neutral, simply write only NR. (CH:):NH2CIO4 2+ 13+ 14+ 1 2 3 4 5 7 8 9 Do (1) (g) (aq) H NR C OH- H2O CI N CO LO 3. 4.
- (c) after adding 0.030_mol of HCI to 1.0 L of the buffer solution in part (a) 0.030mol [H;O*]addea Step 1. Use Stoichiometry to calculate new concentrations Concentration (M) CH;COO-(aq) + H;O*(aq) = 0.030M %3D 1.00L solution CH,COOH(aq) + H,O (1) Initial 0.40 0.030 0.40 Change Final Step 2 Set up a reaction table with the new concentrations. Concentration (M) CH,COOH(aq) + H2O(1) + CH;COO((aq) + H;O*(aq) Initial Change EquilibriumAscorbic acid (H, C,H,0,) is a diprotic acid. The acid dissocation constants for H,C,H,O, are Kal = 8.00 x 10-5 and K„2 = 1.60 x 10-12. Determine the pH of a 0.134 M solution of ascorbic acid. 2.49 pH = Determine the equilibrium concentrations of all species in the solution. [H,C,H,O,] = 0.131 M [HC,H,0G] = 3.22 x10-3 M 7.18 x10 -8 [C,H,O; = M IncorrectAscorbic acid (H,C, H,0,) is a diprotic acid. The acid dissocation constants for H,C. H,O, are K - 800 x 10 and Ka- 1.60 x 10-1 Determine the pH of a 0.138 M solution of ascorbic acid. pH = Determine the equilibrium concentrations of all species in the solution. (H,C,H,0, = M |HC, H,0;] - C,H,O-
- Topic: The Nernst Equation Using the Nernst equation, show whether 1.0 M HCI wil| dissolve lead from lead pipe. 2H* (aq) + 2e H2(g) pE° = 0.0 Pb2+ (aq) + 2e- Pb(s) pE° = -2.13Using only the Henderson-Hasselbalch equation, what is the pH of a solution that is 0.22M phenol, C6H5OH, and 0.29M sodium phenoxide, CoHsONa. 3. C6H5OH (aq) H*(aq) + C6H50(aq) Ka = 1.3 × 10-8Complete the data sheet below. DETERMINATION OF pH OF DIFFERENT SOLUTIONS For those who will be using scientific notation, please follow the format below: Example: 0.00455 -> 4.55E-3 45000 -> 4.5E+4 SOLUTION pH [H*), M РОН [он1, м 0.0345 M HCI 0.000890 M Sr(OH)2 Mixture of 10.0 mL each of the 2 solutions above
- Cl2(aq) reacts with H,O(€) as follows: Cl2 (aq) + 2 H20(€) 2H;0* (aq) + Cl¯(aq) + HOCI(aq) For an experiment to succeed, Cl2(aq) must be present, but the amount of CI"(aq) in the solution must be minimized. For this purpose, should the pH of the solution be high, low, or neutral? Explain.QUESTION 7 Determine the acid dissociation constant, Ka, for a 0.10 Ma weak acid solution that has a pH of 2.87. HA, is a weak.monoproticacid and the equilibrium equation of interest is HA(ag) + H20()= H30*(aq) + A (ag) Enter your answer in exponential format using a capital "E" (example 1.23E-4) and no units (value + 2%).Propanoic acid, CH₂CH₂COOH, is a weak monoprotic acid that is used to inhibit mould formation in bread. A student prepared a 0.10 mol/L solution of propanoic acid and found that the pH was 2.96. What is the acid dissociation constant for propanoic acid? [Hint: Setup an I.C.E. table] CH3CH₂COOH (aq) Ka for propanoic acid is: ←CH3CH₂COO (aq) + H (aq)