**Writing the Solubility Product Formula (Ksp) for Slightly Soluble Salt Equilibria** Below are the reactions for slightly soluble salts and their dissociation in aqueous solutions. The aim is to express their solubility product constants (Ksp). a. **Calcium Sulfide (CaS) Dissociation:** \[ \text{CaS (s)} \leftrightarrow \text{Ca}^{2+} \text{(aq)} + \text{S}^{2-} \text{(aq)} \] b. **Barium Sulfate (BaSO₄) Dissociation:** \[ \text{BaSO}_4 \text{ (s) } \leftrightarrow \text{Ba}^{2+} \text{(aq)} + \text{SO}_4^{2-} \text{(aq)} \] c. **Calcium Phosphate (Ca₃(PO₄)₂) Dissociation:** \[ \text{Ca}_{3}(\text{PO}_{4})_{2} \text{ (s) } \leftrightarrow 3\text{Ca}^{2+} \text{(aq)} + 2\text{PO}_4^{3-} \text{(aq)} \] **Explanation of Diagrams:** 1. **Chemical Equilibrium Arrows:** - Double arrows (\( \leftrightarrow \)) indicate that the salt is in dynamic equilibrium with its ions in aqueous solution. 2. **States of Matter:** - (s) denotes solid. - (aq) denotes that the species are in an aqueous solution. Understanding the Ksp for these reactions helps to predict the solubility of each salt under varying conditions in a solution.

Writing the Solubility Product Formula (Ksp) for Slightly Soluble Salt Equilibria Below are the reactions for slightly soluble salts and their dissociation in aqueous solutions. The aim is to express their solubility product constants (Ksp). a. Calcium Sulfide (CaS) Dissociation: \[ \text{CaS (s)} \leftrightarrow \text{Ca}^{2+} \text{(aq)} + \text{S}^{2-} \text{(aq)} \] b. Barium Sulfate (BaSO₄) Dissociation: \[ \text{BaSO}_4 \text{ (s) } \leftrightarrow \text{Ba}^{2+} \text{(aq)} + \text{SO}_4^{2-} \text{(aq)} \] c. Calcium Phosphate (Ca₃(PO₄)₂) Dissociation: \[ \text{Ca}_{3}(\text{PO}_{4})_{2} \text{ (s) } \leftrightarrow 3\text{Ca}^{2+} \text{(aq)} + 2\text{PO}_4^{3-} \text{(aq)} \] Explanation of Diagrams: 1. Chemical Equilibrium Arrows: - Double arrows (\( \leftrightarrow \)) indicate that the salt is in dynamic equilibrium with its ions in aqueous solution. 2. States of Matter: - (s) denotes solid. - (aq) denotes that the species are in an aqueous solution. Understanding the Ksp for these reactions helps to predict the solubility of each salt under varying conditions in a solution.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Example: Let us determine the concentrations of Ag+, CN, and Ag(CN)₂ when 10.0 mL of 2.00 M KCN is mixed with 10.0 mL of 0.0200 M of AgNO3. Kf for Ag(CN)₂¯ = 1.0 × 10²¹. := Q16.86 What is the initial concentration of Ag+ ion (in M) after mixing but before reaction or equilibrium is established? Type your numeric answer and submit Answered - Incorrect 3 attempts left Q16.87 What is the initial concentration of CN (in M) after mixing but before reaction or equilibrium is established? Cannot be empty Resubmit
A solution has a concentration of 1.0 x 105M of both Fe2* and Co3, If strong base (OH') is slowly added to this solution, what will precipitate first? Fe(OH)2 (Ksp = 8.0 x 10 -16 ) or Co(0H)3 (Ksp = 1.6 x 10 44) O a. neither will ever precipitate O b. Co(OH)3 O c. they will precipitate at the same time O d. Fe(OH)2
Please don't provide handwriting solutions...
Calculate the solubility of CuCO3 in water at 25 °C. You'll find K sp data in the ALEKS Data tab. Round your answer to 2 significant digits. 0+ x10
Write the equilibrium constant expression, Keq, or solubility product constant, Ksp, for each of the following reactions. COCI2 (g) → CO (g) + Cl2 (g) a. b. 2 CO2 (g) 02 (g) + 2 CO () c. AGCI (s) > Ag* (aq) + Cl (aq) d. PbCl2 (s) → Pb2* (aq) + 2 CI (aq) e. NaOH (aq) + HI (aq) <→ Nal (aq) + H20 (I)
13. The Kp of SrCO3 is 1.6 x 10. What is the solubility of SrCO3 (in mol/L) in pure water? sp 14. The KOH(aq) concentration is 1.2 x 10³ M. What concentration of Fe³ must be added to just start forming a precipitate Fe(OH),(s)? 3 15. The solubility of LaF¸ in water is 1.8 x 10°³ g/L. What is the value of K? sp 16. The K of PbBг, is 4.6 x 106. What is the solubility of PbBr₂ (in g/L) in pure water? sp
CS 10 nousT200 7. Tooth enamel (Ca5(PO4)3OH) is a slightly soluble compound that exists as the equilibrium shown below. If the Ksp of tooth enamel in water is 6.8 x 10-37 calculate the molar solubility of tooth enamel. a. b. 2+ 3- Cas(PO4)3OH (s) → 5Ca²+ (aq) + 3PO4 (aq) + OH- (aq) 2.7 x 105 M 5.84 x 10-8 M C. 8.2 x 10-¹9 M d. 6.4 x 109 M 2.00
The Ksp value for magnesium arsenate [Mg3(AsO4)2] is 2.00 X 10-20 so if a chemist added 1.19 x 10-2 M of Pb3(AsO4)2(aq) which is a common ion then what would be the concentration of the Magnesium ion Mg2+(aq) in Molarity at equilibrium? 3.89 x 10-6 4.07 x 10-6 3.47 x 10-6 2.45 x 10-6 2.81 x 10-6 3.28 x 10-6 2.64 x 10-6 3.69 x 10-6 3.01 x 10-6 4.29 x 10-6
Fractional precipitation was performed to separate the metal ions in an aqueous solution containing equimolar concentrations of Mg2+, Pb²+, Fe³+, and Cr³+ by gradual addition of KOH(aq). Which of the following solids will be the first to precipitate? O Mg(OH)2 (Ksp = 1.8 x 10-11) O Pb(OH)2 (Ksp = 1.2 x 10-15) Fe(OH)3 (Ksp = 4.0 x 10-38) O Cr(OH)3 (Ksp = 6.3 x 10-³1)
Calculate the solubility product constant for Th (OH4). The molar concentration of Th (OH4) in the saturated solution is 3.3 x 10-4 mol / L.
Barium sulphate is a relatively insoluble salt used for medical radiographs of the gastrointestinal tract: BaSO4 (s) - Ba2 (aq) + SO42 (aq) The concentration of Ba2* ions in a saturated aqueous solution is 1.05x10 M. Determine Ksp for barium sulphate dissolving in water. O2.12 x 10 5 O1.05 x 1025 O 1.12 x 10-5 O 1.10 x 10-25 1.10 x 10 10
Ksp for PbCl2(s) is 1.6 x 10-³. If you mix 200.0 mL of 0.010 M Pb(NO3)2(aq) with 400.0 mL of 0.010 M NaCI(aq), then sodium nitrate will precipitate. the concentration of CI will be 0.0033 M. no precipitate will form. PbCl2(s) will precipitate.