Q: Choose the solubility statement from below which is correct. a) The ionic compound with the…
A: Answer
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A: Given Solubility product ( Ksp ) = 6.5 × 10-6 Molar solubility ( M ) = ?
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Q: 3. You place some solid copper(1) chloride CuCl in a beaker of distilled water. You measure the…
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Q: For the following, how would decreasing the temperature affect the solubility of the solute? NaCl…
A: ΔH = + 3.9 kJ/mol i.e. reaction is endothermic.
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Q: Which of the following is the least soluble in water? Sodium chloride Ammonium acetate Calcium…
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Q: lid potassium carbonate is slowly added to 75.0 mL of a cobalt(II) fluoride solution until the…
A: Given : Volume of cobalt(II) fluoride = 75.0 mL Concentration of carbonate = 0.0578 M
Q: Given the reaction: CaF2 2 Ca2+ + 2F Which of the following conditions will decrease the solubility…
A: Given, the reaction CaF2 ⇔Ca2+ + F-
Q: The Ksp of beryllium hydroxide, Be(OH)2, is 6.92 × 10-22. Calculate the solubility of this compound…
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Q: 1. Define the terms “saturated solution" and “molar solubility of a salt."
A: Definition of Molar Solubility & Saturated Solution
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A: It’s as shown below :
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A: The compound given is CaCO3. The solubility reaction of CaCO3 can be written as, => CaCO3 (s)…
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A: "Since you have asked multiple questions, we will solve the first question for you. If you want any…
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Q: The solubility of silver sulfate, Ag, SO4, in water has been determined to be 8.00 g/L. What is the…
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Q: True or False…
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Q: Which of the following statement is TRUE? potassium hydroxide is soluble Sodium acetate is soluble…
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A: A numerical problem based on solubility product, which is to be accomplished.
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A: All nitrate salt are water soluble
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Q: 5. Calculate the solubility of compounds. Assume T=25° C. a) Mg(OH)2(s) b) FeSts)
A: a) Mg(OH)2 b) FeS
Q: What is the solubility of Ag2CO3 (s) in moles per liter (mol/L) in pure water? O 2.0 x 10-4 O 1.3 x…
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Q: Calculate the molar solubility of strontium fluoride, SrF2 (FW = 125.26 g/mol; Ksp = 4.33 × 10-9),…
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A: Given: AgCl (s), CaCO3 (s) and Cu(OH)2 (s).
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Q: Calculate the molar solubility of Barium Sulfate. (Ksp 1.1 x 10 10) O 1.3 x 10^(-6) M O 1.2 x…
A:
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- The Ksp for CsClO4 is 0.00757. What is the molar solubility for CsClO4 in M?At a certain temperature the solubility of tin(II) bromide is 0.0116 M. What is the Ksp? Question 2 options: 1.6 x 10–6 1.4 x 10–1 3.1 x 10–6 1.3 x 10–4 6.2 x 10–6 Answer and ExplainThe solubility of the ionic compound M2X3, having a molar mass of 267 g/mol, is 3.60 × 10-7 g/L. Calculate the Ksp of the compound. Ksp =
- What is the molar solubility of cadmium(II) carbonate? Question 3 options: 6.6 x 10–4 1.6 x 10–6 1.1 x 10–6 1.1 x 10–4 2.3 x 10–6 Answer and ExplainConsider 500mL of solution that is .1 M in Co^2+ and .25 M in Ba^2+. What concentration of OH- is required to get the Co^2+ to precipitate? (please type answer not write by hend)The solubility of Gd2(SO4)3 is 4.0 g/100 mL. What is the Ksp?
- 2)What is the Molar Solubility of copper(II) phosphate in a 0.40 M sodium phosphate solution? The KSP of copper(II) phosphate is 1.40E–37. Use Rices table.Determine the concentration of carbonate ion in water due to solubility limit oflimestone (CaCO3). (Experiment: drop a small piece of limestone in a 1L distilled waterand wait until it reaches its solubility limit controlled by the solubility product). (Problemdiscussed in section 2.7).6) If 200 mL of some Pb(NO3)2 solution is mixed with 500 mL of 3.50 x 10−2 M NaCl solution, what is the maximum concentration of the Pb(NO3)2 solution added if no solid PbCl2 forms? (Assume Ksp = 2.00 x 10−5 M at this temperature.) Enter the concentration in M. Hint: Figure out the new concentration of Cl− ions, after adding the two solutions, then calculate the unknown concentration from the Kspequation.
- The solubility of the ionic compound M2X3, having a molar mass of 274 g/mol, is 3.60x10-7 g/L. Calculate the Ksp of the compound. Ksp = __________Activity 4 Another example of going from KSP to Solubility. Then, another application of LeChatelier’s Principle: The Common Ion Effect: BaSO4 is a very toxic ion, yet BaSO4 is used for gastrointestinal x-rays because it is opaque to x-rays. The drink given is actually a suspension, with solid BaSO4 suspended in the solution, so the solution is saturated. KSP for this compound is 1.10 x 10-10. (a) What is the concentration of Ba2+ in a saturated solution of BaSO4? (b) Given the toxicity of Ba2+ ions, why do you think magnesium sulfate is added to the drink? Hint: What would the presence of more sulfate ions do to the amount of dissolved Ba2+ in the solution? Think Le Chatelier’s Principle! Note: sulfate ions are called “common ions” here. (c) Suppose you start with the saturated solution of BaSO4 from part (a) of this problem. Now, figure out what the solubility of BaSO4 becomes if enough MgSO4 is added to the solution to make it 0.10 M in…For magnesium hydroxide, Mg(OH)2 , Ksp = 2.67x10-13 at a certain temperature. Calculate the molar solubility of Mg(OH)2 in pure water. Report your answer to 3 significant figures. S = Answer mol/L