20. What is the [Ag+] when 36.6 ml each of 0.0205 M AgNO3 and 0.610 M Na2S2O3 are mixed? The Kf of Ag(S2O3)2³ = 2.88x10¹³. (1) 4.40x10-15 M (2) 1.21x10-15 M (3) 3.47x10-14 M (4) 1.03x10-12 M (5) 2.05x10-15 M
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- The literature Ksp value for Mg(OH)2 is 1.8×10¬11. (a) Calculate the theoretical [OH ] in a saturated solution of Mg(OH)2. 4.0 3.3e-4 (b) What volume of 0.00177 M HCI would be required to neutralize the OH- in 100.0 mL saturated Mg(OH)2 solution? 4.0 mL(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)4. A solution prepared to be initially 1 M in NH3 and 0.5 M in HCl is (Kb for NH3 = 1.8 x 10¯5): (A) a solution with a pH less than 7 that is not a buffer solution (B) a buffer solution with a pH between 4 and 7 (C) a buffer solution with a pH between 7 and 10 (D) a solution with a pH greater than 7 that is not a buffer solution (E) a solution with a pH of 7
- Parts B and C onlyWhich is the best solution to buffer at pH = 10.50? (A) A buffer solution containing 0.25 M H2CO3 and 0.45 M Na2CO3; (Ka (H2CO3) = 4.3 x 10–7) (B) A buffer solution containing 0.25 M NaHCO3 and 0.45 M Na2CO3; (Ka (HCO3–) = 5.6 x 10–11) (C) A buffer solution containing 0.12 M NaHCO3 and 0.22 M Na2CO3; (Ka (HCO3–) = 5.6 x 10–11) (D) A buffer solution containing 0.12 M NH4Cl and 2.2 M NH3; (Ka (NH4+) = 5.6 x 10–10)In the experiment conducted to determine the amount of acetic acid in vinegar, 8.2 mL of NaOH standard solution adjusted to 0.098 M was spent besides the phenolphthaleley indicator. Accordingly, which of the following is the amount of acetic acid in the vinegar sample in grams? (Ma (CH3COOH): 60.05 g / mol)
- 7. You are given a 500 ml solution of 0.1 M HNO3 and an indicator Hin (Ka = 3.2x10) which changes from yellow (Hin) to green (In'). If you add two drops of indicator to the solution: (a) What colour is the solution initially? (b) What pH would the colour change become visible if you were adding 0.10M NaOH?(5e) Which two of the following compounds would you make a buffer of pH = 12.5. H3PO4 (MM=98.00 g/mol), NaH2PO4 (MM=119.98 g/mol), NazHPO4 (MM=141.96 g/mol), and Na3PO4 (MM = 163.94 g/mol)? [For H3PO4: pK; = 2.148; pKz=7.199; pK3=12.15]!
- Consider the reaction of a 20.0 mL of 0.220 M CSHSNHCI (Ka = 5.9 x 10 °) with 12.0 mL of 0.241 M CSOH. %3D How many moles of CSHSNH' would be present at the start of the titration?G.268.The following pictures represent solutions of AgCI, which may also contain ions other than Ag + and CI which are not shown. Gray spheres represent Ag + ions and dotted spheres represent CI ions. o Oo (1) (2) (3) If solution (1) is a saturated solution of AgCI, which of solutions (1)-(4) represents the solution after a small amount of HN0 3 is added and equilibrium is restored? (1) (2) (3) (4) Click Save and Submit to save and submit. Click Save All Answers to save all answers. Save All Answer MacBook Air DD F10 20 000 000 F9 F8 F7 F6 F5 F4 F3 F2 %23 6 7 8 60 %24