Notes from Dr. Borkosky

Get access risk-free for 30 days, Simplifying, I find that 4x^3 = 1.6 * 10^-5, and therefore x = 0.016. Just like with Keq, small values of Ksp suggest that the reaction is dominant in the reverse direction or reactant heavy. She has an interest in astrobiology and manned spaceflight. Sodium chloride, NaCl, is very soluble in water. Fourth, substitute the equilibrium concentrations into the equilibrium expression and solve for K sp.

What allows the calculation of molar solubility. The process of determining solubilities using. [NaI(aq)] = c(NaI(aq)) = 1.4 × 10-9 mol L-1, V(NaI(aq)) = 25.0 mL = 25.0/1000 = 0.0250 L, [AgNO3(aq)] = c(AgNO3(aq)) = 7.9 × 10-7 mol L-1, V(AgNO3(aq)) = 35.0 mL = 35.0/1000 = 0.0350 L, IF ion product > Ksp a precipitate will form: Ksp was given as 2.5 × 10-9 in the question, so we are confident our answer is correct. All Chemistry Practice Problems Ksp Practice Problems. This is a pretty small number, and this solution is saturated! The concentration of the ions leads to the molar solubility of the compound. The concentration of the ions leads to the molar solubility of the compound. How does ionic strength affect equilibrium constant? Example #9: A saturated solution of magnesium fluoride , MgF2, was prepared by dissolving solid MgF2 in water. Set up an ICE problem (Initial, Change, Equilibrium) in order to use the K sp value to calculate the concentration of each of the ions. credit-by-exam regardless of age or education level. In this case, write the law of mass action. The common-ion effect describes a decrease in solubility of an ionic compound when the solution already contains an ion that is the same as one from the compound. This means that my concentration of Pb^2+ is 0.016 mol/L and the concentration of Cl^- is 0.032 mol/L. [Ag+] ≈ 4 × 10-7 M after mixing (volume roughly doubles so concentration halves), ion product = [Ag+][I-] = [0.7 × 10-9][4 × 10-7] = 2.8 × 10-16 Solubility is the ability to be dissolved in a given volume of a solvent at a given temperature. Solubility data can be used to calculate the K sp for a given compound.

1) Write the chemical equation for the dissolving of barium phosphate in water: 2) Write the Ksp expression for barium phosphate: 4) Put values into and then solve the Ksp expression: 5) Note that the formula weight of Ba3(PO4)2 is not involved at any point. So let's imgaine an experiment in which I have 100 mL water at 25°C and I add solid barium sulfate (BaSO4) 0.0002 g at a time, stirring between each addition and analysing the solution to determine the concentration of barium ions (Ba2+(aq)) and sulfate ions (SO42-). We know that AgCl is in a dynamic equilibrium with its constituent ions, Ag^+ and Cl^-, which can be expressed as AgCl(s) <==> Ag^+(aq) + Cl^-(aq). Example #1: Calculate the milligrams of silver carbonate in first 100 mL (then 250 mL) of a saturated solution of Ag 2 CO 3 (K sp for silver carbonate = 8.4 x 10¯ 12) Solution: 1) Solve for the molar solubility of Ag 2 CO 3: Ag 2 CO 3 ⇌ 2Ag + + CO 3 2 ¯ . Example : Calculating the solubility of an ionic compound (MA). In the case of AgBr, the value is 5.71 x 10¯7 moles per liter.       = 2.5 × 10-9. This means that, when 2.52 x 10¯8 mole per liter of Hg2Br2 dissolves, it produces 2.52 x 10¯8 mole per liter of Hg22+, as well as 5.04 x 10¯8 mole per liter of Br¯ in solution.

Calculating the Solubility of an Ionic Compound in Pure Water from its K sp. For each compound, the molar solubility is given. One can also determine the maximum concentration of ions for a compound with a given Ksp value. As a member, you'll also get unlimited access to over 83,000 Will a precipitate form? We can write an equilibrium expression for this by using the law of mass action. We can substitute x for the concentrations of each ion and plug in our known value of Ksp, then solve for x!

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