Q1: Part 1) The solubility product (Ksp) of AuCl3(s) is 3.2 × 10-25. Calculate the molar...
Q1:
Part 1) The solubility product (Ksp) of AuCl3(s) is 3.2 × 10-25. Calculate the molar solubility of AuCl3(s) in pure water and with the molar solubility found, calculate the solubility of AuCl3(s) in units of mg AuCl3/mL in pure water. The molar mass of AuCl3 is equal to 303.33 g AuCl3/mol AuCl3.
Part 2 )Calculate the molar solubility of AuCl3(s) in an aqueous 1.5 M NaCl solution.
Q2: Calculate the pH of a solution if 75.0 mL of 0.195 M HBr is mixed with 75.0 mL of 0.195 M Ca(OH)2 at 25.0 °C assume the volumes of the solutions are additives
please use correct sig figs for all parts.
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Q1:
Part 1) The solubility product (Ksp) of AuCl3(s) is 3.2 × 10-25.
Calculate the molar...
Please answer these questions: -Calculate the molar solubility of Cr2(CrO4)3 (Ksp = 6.47 x 10-22) in...
Please answer these questions:
-Calculate the molar solubility of Cr2(CrO4)3 (Ksp = 6.47 x 10-22) in a 0.25M Na2CrO4 solution. USE AN ICE TABLE Calculate the molar solubility of AuCl3 (Ksp = 3.2 x 10-25) in a 0.65 M MgCl2 solution. USE AN ICE TABLE
5. a) Determine the molar solubility of PbSO4 in pure water, Ksp (PbSO4) = 1.82 *...
5. a) Determine the molar solubility of PbSO4 in pure water, Ksp (PbSO4) = 1.82 * 10-8 b) A solution containing AgNO3 is mixed with a solution of NaCl to form a solution that is 0.10 M in AgNO3 and 0.075 M in NaCl. Calculate the value for the process. Will a precipitate of AgCl form? Give evidence to support your claim. Ksp (AgCl) = 1.77 10-10
Part A Use the molar solubility, 1.08 x 10-5 M in pure water to calculate Ksp...
Part A Use the molar solubility, 1.08 x 10-5 M in pure water to calculate Ksp for BaCrO4 Express your answer using three significant figures. Y AL OO ? Ksp = Submit Request Answer Part B. Use the molar solubility, 1.55 X 10' M in pure water to calculate Ksp for Ag, SO3 Express your answer using three significant figures. AED O ? Ksp = Submit Request Answer Part C Use the molar solubility, 2.22 x 10-8 M in pure...
Calculate the pH of a solution if 75.0 mL of 0.195 M HBr is mixed with...
Calculate the pH of a solution if 75.0 mL of 0.195 M HBr is mixed with 75.0 mL of 0.195 M Ca(OH)2 at 25.0 °C. Note: assume the volumes of the solutions are additive. Show work.
Calculating Molar Solubility: (Please show all work! will upvote.) Part 1: Calculate the molar solubility of...
Calculating Molar Solubility:
(Please show all work! will upvote.)
Part 1: Calculate the molar solubility of CaSO4 in pure water. Ksp for CaSO4 = 2.4 x 10-5 Part 2: Calculate the molar solubility of CaSO4 in a solution containing 0.100 M Na2SO4.
Calculate the molar solubility of Cu2SO3 (Ksp 8.1 x 1016) a) in water b) in 0.10...
Calculate the molar solubility of Cu2SO3 (Ksp 8.1 x 1016) a) in water b) in 0.10 M CUNO3(aq) solution Will PBF2(s) form when 100 mL of 0.010 M Pb(C2H3O2)2(aq) is mixed with 100 mL of 0.0020 M NH4F(aq)? Explain (show all your work). (Ksp( PbF2)= 4.1 x 10
(20 marks) 5. Consider Agl(s), Ksp -8.3x10-17 a) Calculate the molar solubility of Agl in pure wa...
(20 marks) 5. Consider Agl(s), Ksp -8.3x10-17 a) Calculate the molar solubility of Agl in pure water. b) Considering the complex formation constant K 1.0x1021 for [Ag(CN)2], calculate the equilibrium constant for the reaction: Agl(s) + 2 CN (aq)[Ag(CN2] (aq) + I'(aq) c) Calculate the molar solubility of Agl in a 0.100 M NaCN solution.
(20 marks) 5. Consider Agl(s), Ksp -8.3x10-17 a) Calculate the molar solubility of Agl in pure water. b) Considering the complex formation constant K 1.0x1021...
he solubility product (Ksp) of PbBr2 is 8.9 X 10. Please calculate the molar solubility in:...
he solubility product (Ksp) of PbBr2 is 8.9 X 10. Please calculate the molar solubility in: A) Pure water B) 0.20 M Pb(NOs)2 Pb Brs) Pbap +2 Br 8.9- M0T 2 LOZJLES . 45 25 O.Zts Zs 4.45./05 4 4s 0.2x0.2+s 13:105- J S0-60334 9. The solubility of an ionic compound MX (molar mass = 346 g/mol) is 4.63 X 103 g/L. What is the Ksp for this compound? HoW
4) Calculate the molar solubility of AgCl (Ksp = 1.8 x 10-) at 25°C in: (a)...
4) Calculate the molar solubility of AgCl (Ksp = 1.8 x 10-) at 25°C in: (a) Pure water (b) 3.0 M NH3 [Hint: AgCl(s) + 2NH3(aq) Ag(NH3)2(aq) + Cl(aq) K = 3.1 x 10
Calculate the molar solubility of barium carbonate, Ksp = 2.58 x 10-?, in the following conditions:...
Calculate the molar solubility of barium carbonate, Ksp = 2.58 x 10-?, in the following conditions: Part 1: Pure water Part 2:0.20 M sodium carbonate Part 3: Would the solubility increase or decrease in acidic solution? Explain. You must show ALL of your work to get full credit. Use the formatting tools to enter superscripts, subscripts, arrows, and equations.
Please answer these questions:
-Calculate the molar solubility of Cr2(CrO4)3 (Ksp = 6.47 x 10-22) in a 0.25M Na2CrO4 solution. USE AN ICE TABLE Calculate the molar solubility of AuCl3 (Ksp = 3.2 x 10-25) in a 0.65 M MgCl2 solution. USE AN ICE TABLE
5. a) Determine the molar solubility of PbSO4 in pure water, Ksp (PbSO4) = 1.82 * 10-8 b) A solution containing AgNO3 is mixed with a solution of NaCl to form a solution that is 0.10 M in AgNO3 and 0.075 M in NaCl. Calculate the value for the process. Will a precipitate of AgCl form? Give evidence to support your claim. Ksp (AgCl) = 1.77 10-10
Part A Use the molar solubility, 1.08 x 10-5 M in pure water to calculate Ksp for BaCrO4 Express your answer using three significant figures. Y AL OO ? Ksp = Submit Request Answer Part B. Use the molar solubility, 1.55 X 10' M in pure water to calculate Ksp for Ag, SO3 Express your answer using three significant figures. AED O ? Ksp = Submit Request Answer Part C Use the molar solubility, 2.22 x 10-8 M in pure...
Calculating Molar Solubility:
(Please show all work! will upvote.)
Part 1: Calculate the molar solubility of CaSO4 in pure water. Ksp for CaSO4 = 2.4 x 10-5 Part 2: Calculate the molar solubility of CaSO4 in a solution containing 0.100 M Na2SO4.
Calculate the molar solubility of Cu2SO3 (Ksp 8.1 x 1016) a) in water b) in 0.10 M CUNO3(aq) solution Will PBF2(s) form when 100 mL of 0.010 M Pb(C2H3O2)2(aq) is mixed with 100 mL of 0.0020 M NH4F(aq)? Explain (show all your work). (Ksp( PbF2)= 4.1 x 10
(20 marks) 5. Consider Agl(s), Ksp -8.3x10-17 a) Calculate the molar solubility of Agl in pure water. b) Considering the complex formation constant K 1.0x1021 for [Ag(CN)2], calculate the equilibrium constant for the reaction: Agl(s) + 2 CN (aq)[Ag(CN2] (aq) + I'(aq) c) Calculate the molar solubility of Agl in a 0.100 M NaCN solution.
(20 marks) 5. Consider Agl(s), Ksp -8.3x10-17 a) Calculate the molar solubility of Agl in pure water. b) Considering the complex formation constant K 1.0x1021...
he solubility product (Ksp) of PbBr2 is 8.9 X 10. Please calculate the molar solubility in: A) Pure water B) 0.20 M Pb(NOs)2 Pb Brs) Pbap +2 Br 8.9- M0T 2 LOZJLES . 45 25 O.Zts Zs 4.45./05 4 4s 0.2x0.2+s 13:105- J S0-60334 9. The solubility of an ionic compound MX (molar mass = 346 g/mol) is 4.63 X 103 g/L. What is the Ksp for this compound? HoW
4) Calculate the molar solubility of AgCl (Ksp = 1.8 x 10-) at 25°C in: (a) Pure water (b) 3.0 M NH3 [Hint: AgCl(s) + 2NH3(aq) Ag(NH3)2(aq) + Cl(aq) K = 3.1 x 10
Calculate the molar solubility of barium carbonate, Ksp = 2.58 x 10-?, in the following conditions: Part 1: Pure water Part 2:0.20 M sodium carbonate Part 3: Would the solubility increase or decrease in acidic solution? Explain. You must show ALL of your work to get full credit. Use the formatting tools to enter superscripts, subscripts, arrows, and equations.
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