What is the expected pH of a solution when you dissolve 20 mmoles of Na₂HPO4 in 100 mL of MilliQ water? (Answer with two decimal places) pK₂ values for phosphate: 2.15, 6.80 and 12.37
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- Salts containing the phosphate ion are added to municipalwater supplies to prevent the corrosion of lead pipes. (a) Basedon the pKa values for phosphoric acid (pKa1 = 7.5 x 10 - 3,pKa2 = 6.2 x 10 - 8, pKa3 = 4.2 x 10 - 13) what is the Kbvalue for the PO43 - ion? (b) What is the pH of a 1 x 10 -3 M solution of Na3PO4 (you can ignore the formation ofH2PO4- and H3PO4)?4. (a) Calculate [H3O*] and [OH] for the solutions indicated: lemon juice, pH = 2.42 (1) (ii) household ammonia pH = 11.21 (iii) (iv) (v) phosphate buffer pH = 6.96 human urine pOH = 7.8 tomato juice pOH = 9.9What is the pH of a solution that is a prepared by dissolving 4.90 g of (NH4)2SO4 ( K₁ (NH4+) = 5.70 × 10-¹0) in water, adding 150.0 mL of 0.1263 M NaOH, and diluting to 900.0 mL? pH = b0.124 M in piperidine and 0.054 M in its chloride salt ( Ka (C5H₁1NH+) = 7.50 × 10−¹² )? -12 pH = C prepared by dissolving 2.12 g of aniline (93.13 g/mol, Ką (anilinium ion) = 2.51 × 10−5) in 100. mL of 0.0330 M HCl and diluting to 500.0 mL? pH =
- What is the pH of a solution of 0.400 M CH3NH₂ containing 0.130 M CH3NH3l? (Kb of CH3NH₂ is 4.4 x 10-4)How many grams of acid are needed to prepare a 0.1 M 100 mL phosphate buffer solution with a pH of 7.4? (Use sodium salt in the calculations, Na:23 g/mol, O:16 g/mol, P:31g/mol ; H:1g/mol ; pK1: 2.14 ; pK2:7.2 ; pK3: 12.3 ).10) What is the pK of a weak acid with a Kof 4.7 X 10“?
- What is the pH of a 0.349 M C6H5CO2H M solution if the Ka of C6H5CO2H is 6.5 x 10-5?(f) Calculate the pH of the following solutions: (i) A 0.045 M solution of sulphuric acid. (ii) A solution containing 0.4 g sodium hydroxide in 100 cm³ water. (iii) Given the Ka value for CH3COOH is 1.8 x 10-5, calculate the pH of the acid. The initial concentration of the acid is 0.2 MA weak acid solution with concentration 0.020 M has a pH of 3.7, what is the pKa of this acid?
- Given that pK₂ = 3.14 at 25 °C for HNO₂, what is the pH of 0.165 mol L-1 NaNO₂(aq) at 25 °C? What is the equilibrium concentration of HNO₂? pH = Number (Give your answer accurate to 2 decimal places.) Number mol L-¹ (Give your answer accurate to 2 signficant [HNO₂]eq figures.) =What is the pKb of an unknown weak acid if the pH of the solution was measured to be 4.52. when [HA]=0.540 and [A-]=0.580.(2) When ammonium sulfate dissolves, both the anion and cation have acid-base reaction: (NH4)2SO4(s)< 2NH4* + SO4²- NH4* + NH3(aq) + H* SO42- + H2O → HSO4 + OH- Ksp = 276 Ka = 5.70 ×10-10 Кь 3 9.80 х 10-13 (a) (b) (c) (Show your Calculation) Write a charge balance for this system. Write a mass balance for this system. Find the concentration of NH3(aq) if the pH is fixed at 9.25.