Net Ionic equation?

Question

Which of the following statements are true for the reaction


Ca(OH)2(aq) + HCl(aq) -->



a) CaCl(aq) is a product

b) When balanced the coefficient of HCl(aq) is 3

c) Ions cannot appear in the net ionic equation because they always cancel out on both sides of the equation

d) Ca(OH)2(aq) appears in the net ionic equation

e) H2O(l) appears in the net ionic equation

Answer 1

The balanced reaction equation is
Ca(OH)2(aq) + 2HCl(aq) --> CaCl2(aq) + 2H2O

The total ionic equation is
Ca2+(aq) + 2OH-(aq) + 2H+(aq) + 2 Cl-(aq) --> Ca2+(aq) + 2Cl-(aq) + 2H2O

The net ionic equation is
OH-(aq) + H+(aq) --> H2O


a) CaCl(aq) is a product
Answer: CaCl2(aq) is a product.

b) When balanced the coefficient of HCl(aq) is 3
Answer: False. It is 2.

c) Ions cannot appear in the net ionic equation because they always cancel out on both sides of the equation
Answer: False. OH-(aq) and H+(aq) are ions and they are in the net ionic equation.

d) Ca(OH)2(aq) appears in the net ionic equation
Answer: False. Ca(OH)2 is a strong base, and dissociates completely yo Ca2+(aq) and OH-(aq).

e) H2O(l) appears in the net ionic equation
Answer: True.

Answer 2

i think of you're lacking something on your equation. Sodium metallic, Na(s), plus HCl will bring about a redox reaction, not a metathesis reaction: 2Na(s) + 2HCl ----> 2 NaCl + H2(g) it is that if the solvent is HCl. If the solvent is water, then you certainly gets sodium hydroxide forming too. once you're reacting a sodium salt like NaOH with HCl, a extra a possibility occasion to apply for ionic equations, the molecular equation would be: NaOH(aq) + HCl(aq) ----> H2O(l) + NaCl(aq) This factor shows each and all of the molecules as though they weren't ionizing in answer. it fairly is easily prevalent that they do ionize however, so a extra precise thank you to depict the reaction is the ionic equation, which shows the species as they exist interior the reaction medium (water, for this reason). the completed ionic equation shows each and all of the ions of their solvated, dissociated state, and any insoluble and/or covalently bonded reactants or products that are formed besides: Na+ + OH- + H+ + Cl- ----> H2O(l) + Na+ + Cl- the internet ionic equation leaves out something that occurs as its solvated self in the two the reactants and the products. for this reason, the Cl- and Na+ ions are interior an identical state on the two factors of the reaction, so which you will basically... cancel them out. the only "product" formed is the recent, non-ionic molecule of water, and the only ions in touch in its formation are the H+ and the Cl- ions: OH- + H+ -----> H2O(l) you could write Na(s) + HCl in an ionic trend, even though if it is going to possibly not likely describe the reaction o.k.. Ionic equations are inteded to describe metathesis reactions extra effective than they're meant to describe redox reactions. nonetheless, the completed and internet ionic equations for Na + HCl may well be: 2Na(s) + 2H+(aq) + 2Cl-(aq) -----> H2(g) + 2Na+(aq) + 2Cl-(aq) 2Na(s) + 2H+(aq) -----> H2(g) + Na+

Answer 3

a,e