7. You have 1.0 L of 100 mM K₂HPO, solution. What volume of 1.0 M HCI must be added to adjust the pH of the solution to 6.77? H₂PO4 + H₂O ⇒ H₂O* + H₂PO¡¯ ⇒ H₂O* + HPO³ = H₂O* + PO³ The pk, values for these equilibria are 2.14, 6.86, and 12.4 A. 6 mL B. 17 mL C. 32 mL D. 55 mL 98 mL
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- Marble is almost pure CaCO3. Acid rain has a devastating effect on marble statuary left outdoors. Assume that the reaction which occurs is CoCO3(s)+ H+(aq)Ca2+(aq)+HCO3(aq) Neglecting all other competing equilibria and using Tables 15.1 and 13.2, calculate (a) K for the reaction. (b) the molar solubility of CaCO3 in pure water. (c) the molar solubility of CaCO3 in acid rainwater with a pH of 4.00.1: Cônsider the following buffer solution: 600.0 ml 0.550 M CH,COOH 0.325 M NACH,CO K - 1.76 x 10 Determine the pH of the buffering system after 170.0 ml of 2.00 M NaOH has been added. Part "A": Process the initial information and determine the buffer's initial pH and the initial moles of CH;COOH, NACH,CO0 and NAOH. Part "B": Analyze the in information above and determine if this is a Type I, Il or III Bothering the Buffer problem. Explain your decision (.a sentence or two should be sufficient) Part "C": Perform the necessary calculations and determine the pH of the buffer after the NAOH addition. Your answer should contain the correct number of S.F. Part "D": Compare your answer to the buffer's original pH and determine whether it is reasonable or not. Explain your rationale. O Focus 中Calculate the molar solubility (aq., 20 oC) of aluminum hydroxide, Al(OH)3, in 0.000852 M NaOH. The Ksp of Al(OH)3is 2.0 x 10–32.
- Please help me...... a. Do you expect the pH at the equivalence to be lowest when a 0.0500 M (CH3)3N(aq) solution or a C5H5N(aq) solution is titrated with a 0.0500 M HCl(aq) solution at 25.0 oC? Motivate your answer! (CH3)3N (Kb = 6.5 × 10-5) and C5H5N (Kb = 1.7×10-9) are weak monoprotic bases. Calculate the pH at the equivalence point and 25 oC when 1.00 L of a 0.0500 M C5H5N(aq) solution is titrated with a 0.0500 M HCl(aq) solution. Calculate the molar solubility for CaCO3 in a 0.060 M Ca(NO3)2(aq) solution. Ksp= 3.1 × 10-9 for CaCO3.(b) Lead(II) hydroxide, Pb(OH)2 consists of lead(II) ion and hydroxide ion. Given that Kyp value of Pb(OH)2 is 4.0 × 10-20. (i) What is the pH needed for an aqueous solution of 7.5 x 10-13 M Pb2+ begin to precipitate as Pb(OH)2?3. (а) When 40 mL of benzoic acid (C,H;COOH) and 35 mL of potassium hydroxide were titrated, the pH at the equivalence point was 9.12. Calculate the number of moles of potassium benzoate produced at the equivalence point. Kp of benzoate ion = 1.6 x 101º
- 1. Consider the titration of 25.0 mL of a weak acid, 0.100 M HCOOH (Ka = 1.8 x 10- 4) with 0.100 M NaOH. NaOH (aq) + HCOOH(aq) →H2O(1) + NaCHO2(aq) (i) What is the pH of the solution after adding 5.00 mL of NAOH? (ii) After adding 12.5 mL 2 Veq= midpoint pH = pKa = 3.74In a titration, the equivalence point is the moment at which the number of moles of H+ from the acid that has been added is equal to the number of moles of OH- from the base that has been added. Remember that in a molecule like H2SO4, there are 2 moles of H+ per mole of H2SO4. 16.75 mL of 0.100M H2SO4(aq) is placed in a beaker. After 17.65 mL of NaOH is added to the beaker, the equivalence point is reached. What is the concentration (M) of the NaOH solution?In a titration, the equivalence point is the moment at which the number of moles of H+ from the acid that has been added is equal to the number of moles of OH- from the base that has been added. Remember that in a molecule like H2SO4, there are 2 moles of H+ per mole of H2SO4. 24.54 mL of 0.100M H2SO4(aq) is placed in a beaker. After 22.04 mL of NaOH is added to the beaker, the equivalence point is reached. What is the concentration (M) of the NaOH solution? Report your answer with 3 sig figs
- A chemistry graduate student is given 125. mL of a 0.90M benzoic acid (HC,H,CO2) solution. Benzoic acid is a weak acid with K,=6.3 × 10 °. - 5 What mass of NaC,H,CO, should the student dissolve in the HC,H,CO, solution to turn it into a buffer with pH = 3.97? You may assume that the volume of the solution doesn't change when the NaCH,CO, is dissolved in it. Be sure your answer has a unit symbol, and round it 2. to 2 significant digits. x105:50 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 10-5In an air pollution analysis, 3 L of polluted air is passed through 50 mL of 0,0116 M Ba(OH)2 solution and the carbon dioxide (CO2) in it is precipitated as BaCO3. The excess of the base is titrated with 23.6 mL 0.0108 M HCl in addition to the phenol phthalate indicator. Calculate the CO2 concentration in this air sample in ppm.(Take the density of CO2 as 1.98 g/L, C=12, O=16 g/mol).