Chemistrywill like if correct. QUESTION 11Determine the molar solubility of MX (Ksp 8.3x108) in 0.748 M NaCN. The metal ion M forms M(CN)2 (K-2.1x10) in the presence of CN ion, Enteryour answer in scientific notation with two significant figures. For example, 0.001357 would be entered as 140-3QUESTION 12The metal ion M²+ in ammonia, NH3 forms the complex ion M(NH3)62+ (K= 6.4x1012). Calculate the M2+ concentration when the equilibriumconcentrations of NH3 and M(NH3)62+ are 0.065 and 0.43 M respectively. Enter your answer in scientific notation with two significant figures. Forexample, 0.001357 would be entered as 1.4e-3.

Solubility is defined as the maximum amount of a substance that will dissolve in a given amount of…

QUESTION 11 Determine the molar solubility of MX (Ksp-8.3x108) in 0.748 M NaCN. The metal ion M forms M(CN)2 (K-2.1x10) in the presence of CN ion Enter your answer in scientific notation with two significant figures. For example, 0.001357 would be entered as 1.-40-3 QUESTION 12 The metal ion M2* in ammonia, NH3 forms the complex ion M(NH3)62+ (K 6.4x1012). Calculate the M2 concentration when the equilibrium concentrations of NH3 and M(NH3)62+ are 0.065 and 0.43 M respectively. Enter your answer in scientific notation with two significant figures. For example, 0.001357 would be entered as 1.4e-3.

QUESTION 11 Determine the molar solubility of MX (Ksp-8.3x108) in 0.748 M NaCN. The metal ion M forms M(CN)2 (K-2.1x10) in the presence of CN ion Enter your answer in scientific notation with two significant figures. For example, 0.001357 would be entered as 1.-40-3 QUESTION 12 The metal ion M2* in ammonia, NH3 forms the complex ion M(NH3)62+ (K 6.4x1012). Calculate the M2 concentration when the equilibrium concentrations of NH3 and M(NH3)62+ are 0.065 and 0.43 M respectively. Enter your answer in scientific notation with two significant figures. For example, 0.001357 would be entered as 1.4e-3.

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter15: Complex Ion And Precipitation Equilibria

Section: Chapter Questions

Problem 64QAP

See similar textbooks

Similar questions

What is the molar solubility (in mol L-1) of a salt in pure water with general molecular formula MX (where M is a cation and X is an anion) that has Ksp = 1.38 x 10-9 ? Remember: if you want to express an answer in scientific notation, use the letter "E". For example "4.32 x 104" should be entered as "4.32E4".
What is the molar solubility (in mol L-1) of a salt in pure water with general molecular formula MX2 (where M is a cation and X is an anion) that has Ksp = 4.83 x 10-9 ? Remember: if you want to express an answer in scientific notation, use the letter "E". For example "4.32 x 104" should be entered as "4.32E4".
A solution is prepared by mixing 20.0 mL of 0.100M Fe(NO3)3 with 20.0 mL of 0.00300M KSCN and 10.0 mL of DI water. Calculate the initial concentration of Fe^3+ in this solution? Give answer with correct amount of sig figs.
1. Calculate the solubility of Sn(OH)2 (Ksp = 3.0 x 10-27) in both moles/liter and grams/liter. 2. Which solid is more soluble, FeS (3.7 x 10-19) or NiS (Ksp = 3.0 x 10-21). Justify your answer with a calculation.
Lead(II) carbonate, PbCO3, is one of the components of thepassivating layer that forms inside lead pipes. (a) If the Kspfor PbCO3 is 7.4 x 10 - 14 what is the molarity of Pb2+ ina saturated solution of lead(II) carbonate? (b) What is theconcentration in ppb of Pb2+ ions in a saturated solution?(c) Will the solubility of PbCO3 increase or decrease as thepH is lowered? (d) The EPA threshold for acceptable levelsof lead ions in water is 15 ppb. Does a saturated solution oflead(II) carbonate produce a solution that exceeds the EPAlimit?
The Ksp of AgI is 8.5 ´ 10–17 at 25 °C. Calculate the molar solubility of AgI in 0.0045 M KI(aq) at 25 °C. A. 1.9 x 10–14 mol/L B. 3.8 x 10–12 mol/L C. 9.2 x 10–9 mol/L D. 1.4 x 10–7 mol/L E. 2.0 x 10–6 mol/L
the Ksp= 1.46x10^-10 for CaF2. suppose you add 0.080M of NaF. Use an ICE table to calculate molar solubility(S), in the presence of a common ion (F^-1)
What is the molar solubility (in M to two decimal places) of copper(II) hydroxide in water (at 25 °C)? Ksp = 2.2 × 10–20
Calculate the molar solubility od strontium sulfate SrSO4, in 0.0012 M sodium sulfate, NaSO4. Solve the equation exactly. The Ksp for SrSO4 is 2.8 x 10^-7.
The Ksp of PbBr2 is 6.60x10^-6. What is the molar solubility of PbBr2 in a 0.500 M Pb(NO3)2 solution?
The molar solubility of SrF2 is 2.5 x 10-9 M. Calculate the Ksp of SrF2.
The solubility products of Fe(OH)2 and Fe(OH)3 are 10-17 and 10-38 respectively. If the concentrationsof Fe2+ and Fe3+ are each 10-5, at what pH will each hydroxide just begin to precipitate? A compound containing chlorine is titrated with a solution of 0.075 M Ag2SO4. If 0.250 g of thesample requires 22.07 ml of Ag2SO4 to reach the endpoint, what is the mass percent of chlorine in thesample?