Write the balanced equation for the equilibrium reaction for the dissolution of

Question

Write the balanced equation for the equilibrium reaction for the dissolution of Ca(OH)2 .

Constants Peniodic Table ? Part A How do the concentrations of HCl, OH-and Ca2+ relate to each other stoichiometrically at the end- point (end-point identifies the equivalence point) of the acid- base titration? How is this information used to determine Ksp and AG? Write the balanced equation for the equilibrium reaction for the dissolution of Ca (OH)2 Include all phases. Ca(OH)2 (s)Ca2+()+20H (aq) Subnit Correct Part B Write the net ionic equation between the acid-base titration in this experiment Include all phases. Submit Request Answer Part c Based on your answers parts A and B, what is the stoichiometric mole ratio between HCl : OH-? If your answer is HCI:OH is 2:3, use this format to input your answer: 2,3 Submit

Explanation / Answer

Answer:

Part A: The balanced equation is

Ca(OH)2 (s) ---------> Ca^+2 (aq) + 2OH^-(aq)

Part B: The reaction between acid- base reaction

2HCl(aq) + Ca(OH)2(aq) -----> CaCl2(s) + 2H2O(aq)

Ionic equation is

2H^+(aq) +2Cl^- + Ca^+2(aq) +2OH^- (aq) ------> CaCl2(s) +2H^+(aq) + 2OH^-(aq)

The net ionic equation is 2Cl^- (aq) + Ca^+2(aq) ------> CaCl2(s)

Since H^+ and OH^- are spectator ions, so cancelled on both sides.

Part C: The stoichiometric ratio between HCl and OH^- is 1:1.

Since Ca(OH)2 has 2 moles of OH^- and moles of HCl=2. Therefore stoichiometric ratio betqbet HCl:OH^- = 2:2=1:1.

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