2. Calculate the pH at 25 °C of a solution that is 0.3 M in NaH2AsO4 at 25 °C (Kal =5.8 x 10, Ka2 = 1.1 x 10" and Ka=3.2 x 1012). Submit the answer to 2 decimals
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- A solution is prepared at 25 °C that is initially 0.36M in chlorous acid (HClO₂), a weak acid with K=1.1 × 10¯², and 0.29M in potassium chlorite (KC1O₂). -2 Calculate the pH of the solution. Round your answer to 2 decimal places. pH = 0 X ŚA solution containing 0.0138 M maleic acid and 0.0188 M disodium maleate. The K₁ values for maleic acid are 1.20 x 10-2 (Kal) and 5.37 x 10-7 (Ka2). pH = A solution containing 0.0384 M succinic acid and 0.022 M potassium hydrogen succinate. The Ka values for succinic acid are 6.21 x 10-5 (Kal) and 2.31 x 10-6 (Ka2). pH =Determine the pH of a 0.15 M solution of Ca(BrO2)2 at 25 °C. At the same temperature, Kå for HBrO₂ = 5.6 x 10-7 and K for Ca(OH)2 > 1.
- 2) Determine the concentration of a solution of ammonium chloride (NH4Cl) that has pH of 5.37at 25C. NH3 Kb= 1.8 x 10-5Calculate the pH of a 0.50 M solution of oxalic acid (H2C2O4) given the equilibrium constants below. Ka1 = 5.9 × 10–2 Ka2 = 6.4 × 10–5 Enter your response in pH units to the nearest 0.01.(i) Calculate the mass of NaHCO3 (84.007 g mol) must be added to 4.00 g of K2CO3 (138.206 g mol 1) to give a pH of 10.80 in 500 mL of water? H2CO3 : Ka1 = 4.45 x10-7, Ka2 = 4.69 x 10-11 %3D (ii) Determine the pH of 100 mL of 0.100 M HCl is added to the solution in (i). (iii) Determine the volume of 0.320 M HNO3 that should be added to 4.00 g K2CO3 to give a pH of 10.00 in 250 mL.
- Caculate the pH of a solution prepared by mixing 84.7 mL of a 0.25 M aqueous aniline solution (C6H5NH2, Kb = 4.3 x 10-10) with 100. mL of a 0.11 M aqueous nitric acid solution. Your pH should be reported to two places past the decimal point.A solution is prepared at 25 °C that is initially 0.41 M in chloroacetic acid (HCH2CICO2), a weak acid with K = 1.3 × 103, and 1.3M in potassium chloroacetate (KCH2CICO2). Calculate the pH of the solution. Round your answer to 2 decimal places. pH = 5Calculate the pH of a solution that is 0.0330 M in а. NaHzPOд (Kal %3 7.11 x 10 3, Ка2 — 6.32 х 10 $). pH = b. NaHSO3 (Kal = 1.23 x 10², Ka2 = 6.60 x 10-8). pH =| H2NC, H4NH3+Cl¯ (Ka1 = = 1.42 x 10-7, Ka2 с. 1.18 x 10-10). pH =
- Consider the diprotic acid H2A with K1 = 1.00 x 10-4 and K2 = 1.00 x 10-8 . Find the pH and concentrations of H2A, HA-, and A2- in (a) 0.100 M H2A; (b) 0.100 M NaHA; (c) 0.100 M Na2ACalculate the pH of a weak base solution ([B] > 100 K₂). Calculate the pH of a 0.247 M aqueous solution of hydroxylamine (NH₂OH, K₂ = 9.1×109) and the equilibrium concentrations of the weak base and its conjugate acid. pH [NH₂OH] equilibrium (NH3OH*]equilibrium ΣΣ10. 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?