Calculate the concentration of A when chemical AB is dissolved in pure water. Ksp = 0.00001331 AB2(s) ⇌ A2+(aq) + 2B¯(aq) Enter answer to 3 sig figs using exponential format.
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Calculate the concentration of A when chemical AB is dissolved in pure water. Ksp = 0.00001331
AB2(s) ⇌ A2+(aq) + 2B¯(aq)
Enter answer to 3 sig figs using exponential format.
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- Measurement of the concentration of Fe 3+ ions in a saturated solution of Iron(III) chloride was found to be 0.35 M. Calculate the Ksp of Iron(III) chloride.The dissociation expression of a dilute aqueous solution of acetic acid is shown as: CH3COOH(aq) + H2O(l) <-> CH3COO-(aq) + H3O+(aq) True FalseAmong the solubility rules previously discussed is the statement: Carbonates, phosphates, borates, andarsenates—except those of the ammonium ion and the alkali metals—are insoluble. (a) Write the expression for the equilibrium constant for the reaction represented by the equationCaCO_3(s) ⇌ Ca^2+(aq) + CO3^1−(aq). Is Kc > 1, < 1, or ≈ 1? Explain your answer. (b) Write the expression for the equilibrium constant for the reaction represented by the equation3Ba^2+(aq) + 2PO_4^3−(aq) ⇌ Ba_3(PO_4)_2(s). Is Kc > 1, < 1, or ≈ 1? Explain your answer.
- (a) If Qc > Kc, how must the reaction proceed to reachequilibrium? (b) At the start of a certain reaction, onlyreactants are present; no products have been formed.What is the value of Qc at this point in the reaction?All of the conditions below are standard and represented in DeltaG0' except _______. a. P = 1 atm b. T = 298oC c. pH = 7 d. Initial concentrations for products and reactants are 1 M.Among the solubility rules previously discussed is the statement: Carbonates, phosphates, borates, and arsenates—except those of the ammonium ion and the alkali metals—are insoluble.(a) Write the expression for the equilibrium constant for the reaction represented by the equation CaCO3(s) ⇌ Ca2+(aq) + CO3 −(aq). Is Kc > 1, < 1, or ≈ 1? Explain your answer.(b) Write the expression for the equilibrium constant for the reaction represented by the equation 3Ba2+(aq) + 2PO4 3−(aq) ⇌ Ba3 PO4 2(s). Is Kc > 1, < 1, or ≈ 1? Explain your answer.
- A saturated AgClAgCl solution was analyzed and found to contain 1.25 x 10-5 M Ag+AgX+ ions. Use this value to calculate the Ksp of AgClThe concentration of calcium carbonate in a sample of water saturated with the solid was found to be 7.00 x 10-5 moldm-3 at 200C. What is the solubility product of calcium carbonate at this temperature?The KspKsp of a salt corresponds to a reaction with the following general format: salt(s)⇌mcation(aq)+nanion(aq)where mm and nn are the coefficients that balance the equation. Equilibrium constants follow the general format of products over reactants (excluding pure liquids and solids) with each species raised to the power of its coefficient in the balanced equation. KspKsp is no exception, so Ksp=[cation]m[anion]nKsp=[cation]m[anion]n Part A If 500.0 mLmL of 0.10 mol L−1 Ca2+mol L−1 Ca2+ is mixed with 500.0 mLmL of 0.10 mol L−1 SO42−mol L−1 SO42−, what mass of calcium sulfate will precipitate? KspKsp for CaSO4CaSO4 is 2.40× 10−52.40×10−5. Express your answer to three significant figures and include the appropriate units
- Calculate the molar solubility (moles/L) of CaF2 in water. And also calculate the solubility of CaF2 in water in grams/L. Ksp = 5.3 x 10^-11. b). Calculate the solubility of CaF2 in moles/L and in grams/L in a solution that already contained 0.010 M F-.Consider the following mixtures of chemicals. Complete the table by writing balanced equations and calculating the value of Q. Hence indicate whethe precipitation will occur. Mixture Balanced equation Ksp Q Precipitation occurs (yes or no) 100mL 0.5 molL-1 Ca(NO3)2 mixed with 100 mL 0.2 molL-1 Na2SO4 6.1x10-5 20 mL 0.01 molL-1 AgNO3 mixed with 80 mL 0.05 molL-1 K2CrO4 1.7x10-12Write the reaction quotients for the following reactions making the approximation of replacing activities by molar concentrations or partial pressures:(a) 2 CH3COCOOH(aq) + 5 O2(g) → 6 CO2(g) + 4 H2O(I)(b) Fe(s) + PbSO4(aq) → FeSO4(aq) + Pb(s)(c) Hg2CI2(s) + H2(g) → 2 HCI(aq) + 2 Hg(l)(d) 2 CuCI(aq) → Cu(s) + CuCI2(aq)