Complete and balance the equations for the following...

Complete and balance the equations for the following double-displacement reactions: a. $\operatorname{AgNO}_{3}(a q)+\operatorname{NaCl}(a q) \longrightarrow$ ________ b. $\operatorname{Mg}\left(\mathrm{NO}_{3}\right)_{2}(a q)+\mathrm{KOH}(a q) \longrightarrow$ ________ c. $\operatorname{LiOH}(a q)+\mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{3}(a q) \longrightarrow$ ________

Complete and balance the equations for the following double-displacement reactions:
a. $\operatorname{AgNO}_{3}(a q)+\operatorname{NaCl}(a q) \longrightarrow$ ________
b. $\operatorname{Mg}\left(\mathrm{NO}_{3}\right)_{2}(a q)+\mathrm{KOH}(a q) \longrightarrow$ ________
c. $\operatorname{LiOH}(a q)+\mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{3}(a q) \longrightarrow$ ________

Key Concepts

Double-Displacement Reaction

A type of reaction where the ions of two compounds exchange places to form two new compounds. This reaction typically occurs in aqueous solutions, and its outcome is often determined by the solubility of the resulting compounds.

Balancing Chemical Equations

The process of ensuring that the same number of each type of atom appears on both sides of a chemical equation. This is necessary to comply with the law of conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction.

Precipitation Reaction

A reaction that occurs when ions in solution combine to form an insoluble salt, known as the precipitate. These reactions are often a subset of double-displacement reactions and are identified by the formation of a solid from two aqueous solutions.

Solubility Rules

A set of guidelines used to predict whether an ionic compound will dissolve in water. These rules help determine which products of a chemical reaction remain in solution and which form a precipitate, thereby guiding the identification of double-displacement reactions.

Transcript

00:01 Okay, so this question asks us to complete and balance three different equations.

00:05 Here's the first equation so let's start so to balance this equation we need to make sure that the same number of each type of atom is present on both sides of the equation so um first we need to complete it.

00:23 So what i like to do is this trick right here we're going to join this first side of the compound with the second side of the compound and then we're gonna join from the second compound the first side with the second side of the first component.

00:42 It's gonna look like this agcl plus na no three and now to balance this equation like i said, we need to make sure that we have the same number of each type of atom on each side of the equation so every time you make a change on one side, you gotta go and make a change on the other side so we added a two there.

01:12 We're gonna put a two here.

01:13 We have uh, two for the silver atoms so we're good in there.

01:18 We're gonna add a two here.

01:20 We're gonna have two sodium atoms so we're gonna have a uh, add a two on the other side of the equation and now we have six oxygen, i mean six, uh, two no3 atoms and we have two no3 atoms on the reactant side of the equation.

01:41 So this equation is done.

01:43 It's balanced.

01:43 Okay, so we here we have the second equation and we're gonna follow the same steps we're gonna join this first side with the second side and it's a little bit trickier now because there's a parenthesis here but basically what's gonna happen is that the oh is gonna replace no3 inside the parenthesis.

02:07 So it's gonna look a little bit like this ng oh plus k no3 and now to balance this equation, we have one mg on this side.

02:28 We have one mg on this side.

02:30 We have one mg on this side...

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