An example of an insoluble substance, AgBr (silver bromide), has a minuscule molar solubility with the value being close to 5.71 x 10 to the … Still have questions? If it was in g dm-3, or any other concentration units, you would first have to convert it into mol dm-3. The molar solubility of AgI is 9.0 x 10 -9 mol/L. Calculate the molar solubility of Fe(OH)2 when buffered at pH = 11.9. let x = mol/L of Fe(OH)2 that dissolve : this will give x mol/L Fe2+ and 2x mol/L OH-. Now, solve for s: s 2 = 8.5 x 10 -17. s = $\sqrt {8.5 \times 10^ {-17} }$ s = 9.0 x 10 -9 mol/L. Molar solubility (M) is a measure of the ability of a compound, called a solute, to dissolve in a specific substance, called a solvent.Specifically, it is the maximum number of moles of a solute that are able to dissolve in one liter of solvent, so molar solubility is measures as moles/L. calculate the molar solubility of Ag2CrO4 AT 25 C in: a- pure water b- 0.200M AgNO3 C- 0.200M Na2CrO4 for Ag2CrO4 AT 25C, Ksp=1.2x10^(-12) Calculate the molar solubility of Fe(OH)2 when buffered at pH = 10.1. Calculating solubility products from solubilities. [OH-]. What is the molar solubility of MgF 2 in a 0.20 M solution of NaF? It is a constant property of each substance - for example, the molar mass of water is approximately equal to 18 g/mol. I found x to equal 2.7 x 10^-3 . Can someone please help with these questions? a.) 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I thought I knew how to work them but keep coming up with the wrong answer for both. Can someone explain what to do after this to get the answer? Calculate the K sp for Ba 3 (PO 4) 2. b.) moles of solute in 100 mL; S = 0.0016 g / 78.1 g/mol = $$2.05 \times 10^{-5}$$ mol $S = \dfrac{2.05 \times 10^{ –5} mol}{0.100\; L} = 2.05 \times 10^{-4} M$ Calculate the molar solubility of Fe(OH)2 when buffered at pH = 10.1. If 50.0 mL of 0.540 mol/L sodium hydroxide reacts with 85.6 mL of sulfuric acid, calculate the concentration of the sulfuric acid. This will tell you how much Fe(OH)2 has dissolved. I went to a Thanksgiving dinner with over 100 guests. molar solubility of gas at 101.3 kPa = c(gas) = P × 1/K = 101.3 × 1/k The graph below shows how the solubility of a gas increases as its partial pressure increases according to Henry's Law: concentration / mol L-1: Molar Solubility of gases in water at 25°C. Can someone please help with these questions? b.) Soilids have not got a concentration, so we are able to forget approximately approximately it here. Join Yahoo Answers and get 100 points today. Calculate the molar solubility of Fe(OH)2 when buffered at pH = 10.1. Solution: 1) Write the chemical equation for the dissolving of barium phosphate in water: Ba 3 (PO 4) 2 (s) ⇌ 3Ba 2+ (aq) + 2PO 4 3 ¯(aq) 2) Write the K sp expression for barium phosphate: K sp = [Ba 2+] 3 [PO 4 3 ¯] 2. Calculate the value of K s under these conditions. pOH = - log[OH-] = 3.9 to find conc. The chief was seen coughing and not wearing a mask. Example #1: Silver chloride, AgCl, has a K sp = 1.77 x 10¯ 10. Taking the square root of both sides allows you to solve for the molar solubility: Thus, the molar solubility of both Ag + and Cl - is thus 1.3 x 10 -5 M. Finding Ksp From Molar Solubility Example #10: The molar solubility of Ba 3 (PO 4) 2 is 8.89 x 10¯ 9 M in pure water. It is expressed in grams per mole. ? P.S. even though it is immportant ffor calculating Ka and Kb. a.) Given the K sp, calculate the molar solubility (in mol/L) of a saturated solution of the substance. Molar mass is the mass of 1 mole of the solute. Calculate … From pH the H+ ions = a million.2x10^3 = C6HJ5COO- ions Ksp =, (a million.2x10^-3)^2 = a million.44x10^-6 Moles consistent with Litre. Calculate its solubility in moles per liter. Draw structures of OF2, BrF3, SCl2, XeF4, PF3 in a way that indicates their molecular shape? Use the ksp value and [OH-] above to find [Fe+2]. The solubility of CaF 2 (molar mass 78.1) at 18°C is reported to be 1.6 mg per 100 mL of water. b.) The formula for K sp is: K sp = [Ag + ] [I –] K sp = s 2 = 8.5 x 10 -17. where s is the concentration of each ion at equilibrium. a.) Calculate the molar solubility of Fe(OH)2 when buffered at pH = 11.9. I thought I knew how to work them but keep coming up with the wrong answer for both. Which of the following is not a geometric (cis-trans) isomer. well assuming that the value of 0.01835 M ( 1.835 X 10^-2 M ) is the correct and represents the amount of Ca(OH)2 in a std solution ..then the formal solubility is 1.835 x 10^-2 M..the amount of Ca+2 is 1.835 X 10^-2 M, the amount of OH^-1 = 3.67 x 10^-2 M, the solubility … Do the same for b) but [OH-] will be different because pH is different. I thought I knew how to work them but keep coming up with the wrong answer for both. K sp (MgF 2) = 8.0 x 10-8.. Can someone please help with these questions? I am going to assume that you are given the solubility of an ionic compound in mol dm-3. 3) Determine [Ba 2+] and [PO 4 3 ¯]: Solution. The solubility of barium sulphate at 298 K is 1.05 x 10-5 mol dm-3. I found the molar solubility of MgF2 using Ksp = [Mg 2+] [2F-]^2. Which of the following compounds is most soluble in water?