Mercury thiocyanate - Hg(SCN)2 - is slightly soluble in water. Its Ksp is 2.8 x 10-20. a. Write the equilibrium reaction for mercury thiocyanate's dissolution. b. Write the equilibrium expression for the above reaction. c. In the titration of 50.00 mL of 0.0457 M Hg2+ with 0.200 M SCN-, show or calculate the following: i. The titration reaction ii. The volume of SCN- needed to reach the equivalence point (Ve). iii. pHg at 0.4 Ve iv. pHg at Ve v. pHg at 1.4 Ve

Mercury thiocyanate - Hg(SCN)2 - is slightly soluble in water. Its Ksp is 2.8 x 10-20. a. Write the equilibrium reaction for mercury thiocyanate's dissolution. b. Write the equilibrium expression for the above reaction. c. In the titration of 50.00 mL of 0.0457 M Hg2+ with 0.200 M SCN-, show or calculate the following: i. The titration reaction ii. The volume of SCN- needed to reach the equivalence point (Ve). iii. pHg at 0.4 Ve iv. pHg at Ve v. pHg at 1.4 Ve

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter15: Additional Aqueous Equilibria

Section: Chapter Questions

Problem 15.BCP

See similar textbooks

Similar questions

PART 2: A solution is prepared by mixing 150.0 mL of 0.0010 M magnesium nitrate and 250.0 mL of 0.100 M sodium fluoride (Ksp = 7.4x10-11). Is Ksp greater than , equal to, or lower than Qsp? Will a precipitate form, Y/N? What is the fluoride ion concentration (in solution) after mixing is complete? Give your answer in exponential form and to three sig. figs. (e. g. 1.23E-3). What is the magnesium ion concentration (in solution) after mixing is complete? Give your answer in exponential form and to three sig. figs. (e. g. 1.23E-3).
Solid potassium chromate (K2CrO4) is slowly added to a solution containing 0.50 mol L-1 AgNO3 and 0.50 mol L-1 Ba(NO3)2. What is the Ag+ concentration when BaCrO4 just starts to precipitate? The Ksp for Ag2CrO4 and BaCrO4 are 1.1 × 10-12 and 1.2 × 10-10, respectively.
0.10 M potassium chromate is slowly added to a solution containing 0. 50 M AgNO3 and 0. 50 M Ba(NO3)2. What is the [Ag+ ] when BaCrO4 just starts to precipitate? The Ksp for Ag2CrO4 and BaCrO4 are 1.1 × 10-12 and 1.2 × 10-10, respectively. A. 6.5 × 10-5 M B. 1.3 × 10-4 M C. 3.2 × 10-4 M D. 6.8 × 10-2 ME. None of the above is correct.
What is the Cl- concentration just as Ag2CrO4 begins to precipitate when 1.0 M AgNO3 is slowly added to a solution containing 0.015 M Cl- and 0.015 M I-? Ksp for Ag2CrO4 is 1.2 x 10-12.
1. For the reaction: PbCl2(s) ↔ Pb2+(aq)+2Cl1-(aq), what is Q* when 8.0 mL of 0.054 M lead nitrate is added to 21 mL of 0.025 M sodium chloride? Ksp of lead chloride is 1.6 x 10-5 M3. *Recall: Q is compared to Ksp to determine whether a precipitate forms. 2.Sodium phosphate is added to a solution that contains 0.0088 M aluminum nitrate and 0.046 M calcium chloride. The concentration of the first ion to precipitate (either Al3+ or Ca2+) decreases as its precipitate forms. What is the concentration of this ion when the second ion begins to precipitate?
Calculate The solubility of Ba(IO3)2 in a solution prepared by mixing 200 mL of 0.00100 M Ba(NO3)2 with 100 mL of 0.0100 M NaIO3. The Ksp for barium iodate is 1.57 x 10-9(a) Write the solubility equilibria expression for Ba(IO3)2(b) Write the Ksp expression for the reaction in (a)(c) Determine the new concentration of Barium and Iodate ions(d) Determine the limiting and excess reactant(e) Calculate the molar solubility of Barium Iodate(f) What does a small value of Ksp tell us?
Given that the Ksp for CaF2 at 25 °C is 3.9 × 10–11, will a precipitate form when 0.10 L of 2.3 x 10–4 M CaCl2 is added to 0.50 L of 5.0 × 10–3 M NaF? Assume volumes are additive. A. No, because Q = 6.6 × 10–10 and therefore Q > Ksp. B. Yes, because Q = 1.6 × 10–7 and therefore Q > Ksp. C. Yes, because Q = 5.8 × 10–9 and therefore Q > Ksp. D. Yes, because Q = 6.6 × 10–10 and therefore Q > Ksp.
At 15 °C, the solubility product of PbCrO4 is 1.69 × 10-14 mol2dm-6. (a) Write an expression for the solubility product of PbCrO4.(b) Calculate the solubility of PbCrO4.(c) On adding concentrated aqueous lead(II) nitrate dropwise to 0.010 moldm-3 potassium chromate (VI), what is the concentration of lead(II) ions when the first trace of precipitate appears?
1. a. When excess solid SrCrO4 is shaken with water at 25°C, it is found that 6 x 10^-3 mol dissolves per liter. Use this information to calculate the solubility product constant for SrCrO4. b. The Ksp of BaF2 is 1.8 x 10-7, what is its water solubility in moles per liter.
Consider the reaction of 25.0 mL of 0.20 M AgNO3(aq) with 25.0 mL of 0.20 M NaBr(aq) to form AgBr(s) at 25 °C. What is ΔG for this reaction? The Ksp of AgBr is 5.0 × 10-13 at 25 °C
Consider a solution that is made from mixing 122.3ml of 0.333M ZnCl2 and 83.57ml of 0.654M Na2CO3 a. What is the concentration of cations and anions at equilibrium(in molarity)? Use x-is-small approximation. b. What is the ‘net’ amount of precipitate produced(in moles)? ksp (ZNCO3) = 1 x 10^-10
In order to form Ba(IO3)2, 500 mL of 0.5000 M Ba(NO3)2 was mixed with 500 mL of 0.0500 M NaIO3. Ksp= 1.57x10^-9What is the concentration of the excess reagent?What is the molar solubility of Ba(IO3)2 in this solution? 2.04x10^-5 M 4.07x10^-5 M 6.15x10^-5 M 8.30x10^-5 M