When an aqueous solution of sodium hydroxide, NaOH, is added to an aqueous solution of chromium(III) nitrate, Cr(NO3)3, a precipitate of chromium(III) hydroxide, Cr(OH)3, forms. Write a balanced net ionic equation for this reaction.
Cr(NO3)3(aq) + 3NaOH(aq) ==> Cr(OH)3(s) + 3NaNO3(aq)
Now you convert that balanced molecular equation into a balanced ionic equation.
Cr^3+(aq) + 3(NO3^-)(aq) + 3Na^+(aq) + 3OH^-(aq) ==> Cr(OH)3(s) + 3Na^+(aq) + 3NO3^-(aq) and here are the rules you follow.
1. Gases remain as molecules.
2. Solids remain as molecules.
3. Weak electrolytes remain as molecules.
4. All others are separated into ions.
[Note: There are no gases. The solid is Cr(OH)3 so that is NOT separated into ions. There are no weak electrolytes so all of the others are shown as the ions.
The last step is to cancel ions that are common(that is the same) on both sides. That is the Na^+ and the NO3^-. What is left?
Cr^3+(aq) + 3OH^-(aq) ==> Cr(OH)3(s)
It's really a simple three step process.
1. Write and balanced the molecular equation.
2. Using the rules above, separate into the COMPLETE balanced ionic equation.
3. Cancel ions common to both sides.
Oh, chemistry, you always keep me on my toes! Alrighty, here's a balanced net ionic equation for this reaction:
3 NaOH(aq) + Cr(NO3)3(aq) → Cr(OH)3(s) + 3 NaNO3(aq)
See? This reaction is just like a little chemistry dance party, with sodium hydroxide and chromium(III) nitrate joining forces to create chromium(III) hydroxide and sodium nitrate. It's all about those balancing acts! Keep up the good work, my chemistry friend!
To write the balanced net ionic equation for the reaction between sodium hydroxide and chromium(III) nitrate, we need to first write the balanced complete ionic equation and then identify the spectator ions.
The balanced complete ionic equation for the reaction is:
3NaOH(aq) + Cr(NO3)3(aq) -> Cr(OH)3(s) + 3NaNO3(aq)
In this equation, sodium hydroxide (NaOH) reacts with chromium(III) nitrate (Cr(NO3)3) to form chromium(III) hydroxide (Cr(OH)3) and sodium nitrate (NaNO3).
Next, we need to identify the spectator ions, which are the ions that do not participate in the reaction. In this case, the sodium ions (Na+) and nitrate ions (NO3-) appear on both sides of the equation and do not undergo any chemical changes. Therefore, they are spectator ions.
The net ionic equation represents the reaction involving only the species that undergo chemical changes. In this case, the spectator ions (Na+ and NO3-) are removed from the equation.
The balanced net ionic equation for the reaction is:
Cr3+(aq) + 3OH-(aq) -> Cr(OH)3(s)
To write a balanced net ionic equation for this reaction, we'll need to first write the balanced chemical equation, and then convert it into its net ionic form. Here are the steps:
Step 1: Write the balanced chemical equation.
The molecular equation for the reaction is:
NaOH(aq) + Cr(NO3)3(aq) → Cr(OH)3(s) + NaNO3(aq)
Note that NaOH and Cr(NO3)3 are the reactants, and Cr(OH)3 and NaNO3 are the products.
Step 2: Convert the equation into its ionic form.
To convert the equation into its ionic form, we need to dissociate the compounds that are strong electrolytes (they ionize completely in aqueous solution) into their respective ions. Here’s the ionic equation:
Na+(aq) + OH-(aq) + Cr3+(aq) + 3NO3-(aq) → Cr(OH)3(s) + Na+(aq) + 3NO3-(aq)
Step 3: Write the net ionic equation.
The net ionic equation shows only the species that participate in the reaction. In this case, the Na+ and NO3- ions are spectator ions, meaning they are present on both sides of the equation but do not take part in the reaction. Therefore, we eliminate them from the equation:
OH-(aq) + Cr3+(aq) → Cr(OH)3(s)
So, the balanced net ionic equation for this reaction is:
OH-(aq) + Cr3+(aq) → Cr(OH)3(s)