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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![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](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc5d31d0c-d4ca-4807-b7ff-b6d8b3bb9466%2Fed1f554b-5da4-4fd4-b5de-06454f8d1a5d%2Fgmurtle_processed.png&w=3840&q=75)
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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 mLA 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?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
- (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)Which 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)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?
- 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?12. The following quantities of salts were added to a volume of water to make 1 liter of solution: 1 x 10-2 moles NaCl 2 x 10-2 moles CaCl, 2 x 10-2 moles BaCl, (a) What is the ionic strength of the solution? (b) A small amount of phosphate salt is added to the same solution with negligible change in ionic strength. Given K = 10-7.2 for the reaction H,PO, = H+ + HPO,?- Calculate (H*][HPO,2-1/[H,PO,"), called °K, using the Güntelberg ap- proximation of the DeBye-Hückel law. (c) Calculate the "salting-out" coefficient, k,, for a nonelectrolyte in the same solution if its activity is 10-3 M and its concentration is 9.5 x 10 4 M.Write the products for the balanced equation for the dissociation into ions of each of the following soluble salts in aqueous solutions: Input the cation and then anion with correct coeffiecients and charges. For example: The answer for ??(??3)2⟶??2++2??−3Ba(NO3)2⟶Ba2++2NO3− would be inputted in two separate fields, inputting the cation first: Ba^2+ 2NO_3^- Use carats for superscripts and underscores for subscripts. Include coefficients, if the coefficient is greater than 1. a) ???⟶CaS⟶ + b) ??3??4⟶Na3PO4⟶ +
- What reagent might be used to separate the ions in each of the following mixtures, which are 0.1 M with respect to each ion? In some cases it may be necessary to control the pH. (a) Hg2 2+ and Cu2+(b) SO4 2− and Cl–(c) Hg2+ and Co2+(d) Zn2+ and Sr2+(e) Ba2+ and Mg2+(f) CO3 2− and OH–3:46 1 ul 5G OKINETICS AND EQUILIBRIUM Calculating the solubility of an ionic compound when a commo. db Data Bacro4 1.17x10-10 Calculate the solubility at 25 °C of AgCl in pure water and in a 0.0030M AGNO, solution. BasO4 1.08x10-10 Round both of your answers to 2 significant digits. CaCo, 3.36x10-9 CaFa 3.45x10-11 Co(OH)2 5.92x10-15 solubility in pure water: CuBr 6.27x10-9 CucOs 1.4x10-10 solubility in 0.0030 M AgNO, solution: 0: Fe(OH)2 4.87x10-17 7.40x10-14 PbCro4 2.8x10-13 PbF2 3.3x10-8 Mg(OH)2 5.61x10-12 Ni(OH)2 5.48x10-16 AgBro 5.38x10-5 Ag;CO 8.46x10-12 AgC 1.77x10-10 AgzCro4 1.12x10-12 Srco, 5.60x10-10 ZnCo 1.46x10-10 Zn(OH)2 2.0x10-1 AgBr 5.35x10-13 AuCI 1.77x10-10 Explanation Check 2021 MGrew tton ARhs 23 TO MacBook AirA 10.00 ml sample containing 6.0000 g/L of a mixture of KCI (74.5 g/mol) and NaCl (58.5 g/mol) was titrated with 0.10 M standard solution of AgNO; where 5.6 mL was needed to reach the end-point. Calculate the mass of sample (in grams). O 0.0063 b) 0.0337 c) 0.0033 d) 0.0221 e) 0.0600