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- 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.Calculate the final [Ag1+] concentration in solution when 0.035 moles of AgNO3 are added to 500. mL of 0.21 M NaCN. Assume the volume remains constant. Ksp = 1.2 ✕ 10-16 for AgCN. (in M)What is the pH of the buffer 0.13 M Na₂HPO4/0.16 M KH₂PO4? Round your answer to 2 decimal places. Note: Reference the K of acids at 25 °C table for additional information. pH I = x10 X Ś
- 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 10-51: 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What is the molar solubility of Nis in 0.60 M NH3? The K for Nis is 3.0 x 10-19. The K; for Ni(NH3),*+ is 5.6 × 10°. Molar solubility = |
- (f). Following are the titre values of two students when 25 mL of KIO3(aq) is titrated against Na2S2O3(aq).Titration no. Student 1 Student 21 2 3 24 24.9 25.7 25 24.1 24.0Which student is best in doing titration and why do you say so?(g). Taking the values of best student, calculate the concentration of the solution for which molarity is not known.(Note: first calculate moles of pipet solution in 25 mL, then moles of I2 and then moles of solution of unknown concentration and then its molarity by using average titre)A sample of 50.00 mL of 0.1000 M aqueous solution of benzoic acid (C6H5COOH) K = 6.46 x 10- , is titrated with a 0.1000 M NaOH solution. Calculate the pH at the following points: 5i) after 0 NaOH has been added. Choose from answers A-D. a ii) after 5.00 mL of NaOH has been added. Choose from answers E-H. iii) after 25.00 mL of NaOH has been added. Choose from answers I-L. iv) after 49.90 mL of NaOH has been added. Choose from answers M-P. v) after 50.00 mL of NaOH has been added. Choose from answers Q-T. vi) after 55.00 mL of NaOH has been added. Choose from answers U-X.(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?
- An analytical chemist has been given the task of precipitating lead cation (Pb2+) out of solution that is 0.424 M in Pb2+ . At her disposal is a large bottle of solid sodium iodide (NaI). What must the concentration of iodide be for precipitation to begin? (The Ksp of lead iodide is 9.8 x 10-9).A diprotic acid, HzA, has K1 = 1.41 x 10 and K2 = 3.09 x 10. If 50.00 mL. of 0.113 M H2A is placed in an flask and is titrated with 0.289 M N2OH. (a) What volume of NAOH would be needed to reach the second equivalence point? (b) What is the pH at the second half-equivalence point? (c) what would be the pH when 24.5 ml. of base has been added to the flask?< A buffer solution that is 0.401 M in HF and 0.401 M in KF has a pH of 3.14. The addition of 0.01 mol of H3O+ to 1.0 L of this buffer would cause the pH to A C The capacity of this buffer for added H₂Ot could be increased by the addition of 0.159 mol