Question

explain how the molecular formula for calcium hydroxide was determined. include the balanced equation for ca(s) reacting with water and the balanced equation for the net ionic reaction that occurs during the titration. state your results: indicate the molecular formula for calcium hydroxide for each trial before you rounded to the nearest integer. compare your results to the actual molecular formula, ca(oh)2. explain what experimental error could cause the ratio to be higher or lower than 1 to 2 for calcium to hydroxide ions.

Answer 1

The formula for calcium hydroxide Ca(OH)2 is based on the ionic charges of Ca2+ and OH-. The balanced chemical equation for its formation from calcium and water, as well as the net ionic equation for its titration, illustrate its stoichiometry. Experimental errors can impact the ratio determination during titrations.

Step-by-step explanation:

The molecular formula for calcium hydroxide is determined based on the ionic charges of calcium (Ca2+) and the hydroxide ion (OH−). Since calcium has a charge of +2 and each hydroxide ion has a charge of -1, two hydroxide ions are needed to balance the charge, giving us the formula Ca(OH)2.

When calcium reacts with water, the balanced equation is:

Ca(s) + 2H2O(l) → Ca(OH)2(aq) + H2(g)

During titration, the balanced net ionic equation with HNO3 would be:

Ca(OH)2(s) + 2HNO3(aq) → Ca(NO3)2(aq) + 2H2O(l)

The net ionic equation simplifies to:

Ca2+(aq) + 2OH−(aq) + 2H+(aq) + 2NO3−(aq) → Ca2+(aq) + 2NO3−(aq) + 2H2O(l)

Cancelling spectator ions, we get:

OH−(aq) + H+(aq) → H2O(l)

Experimental errors that could affect the ratio determination may include measurement inaccuracies, incomplete reactions, and impurities in the reactants.