Predict the products and write a balanced molecular equation...

Predict the products and write a balanced molecular equation for each reaction. If no reaction occurs, write "NO REACTION." a. $\mathrm{HCl}(a q)+\mathrm{Hg}_{2}\left(\mathrm{NO}_{3}\right)_{2}(a q) \longrightarrow$ b. $\mathrm{KHSO}_{3}(a q)+\mathrm{HNO}_{3}(a q) \longrightarrow$ c. aqueous ammonium chloride and aqueous lead(II) nitrate d. aqueous ammonium chloride and aqueous calcium hydroxide

Predict the products and write a balanced molecular equation for each reaction. If no reaction occurs, write "NO REACTION."
a. $\mathrm{HCl}(a q)+\mathrm{Hg}_{2}\left(\mathrm{NO}_{3}\right)_{2}(a q) \longrightarrow$
b. $\mathrm{KHSO}_{3}(a q)+\mathrm{HNO}_{3}(a q) \longrightarrow$
c. aqueous ammonium chloride and aqueous lead(II) nitrate
d. aqueous ammonium chloride and aqueous calcium hydroxide

Key Concepts

Balancing Chemical Equations

Balancing chemical equations is the process of ensuring that the number of atoms of each element and the overall charge are the same on both sides of a chemical reaction. This practice is essential to obey the law of conservation of mass and is a fundamental skill in writing accurate chemical equations.

Acid-Base Reactions

Acid-base reactions involve the transfer of protons between an acid and a base, often resulting in the formation of water and a salt. Recognizing acid-base behavior is important for predicting products when an acid is mixed with a compound that can act as a base or contains a basic ion.

Precipitation Reactions

Precipitation reactions are a subclass of double displacement reactions where one of the products is an insoluble solid (the precipitate) that forms in the aqueous solution. The formation of a precipitate drives the reaction forward as the solid separates from the solution.

Double Displacement Reactions

Double displacement reactions, also known as metathesis reactions, involve the exchange of ions between two reacting compounds in aqueous solution. In these reactions, the cations and anions of the reactants swap partners to form two new compounds, and the reaction proceeds if one of the products is insoluble, a weak electrolyte, or a gas.

Solubility Rules

Solubility rules are guidelines used to predict whether an ionic compound will dissolve in water. These rules help determine whether the products formed in a double displacement reaction remain in solution or form a precipitate, which is critical when predicting the outcome of a reaction.

Transcript

00:01 For question 77, you're asked to predict the products and write a balanced molecular equation for each reaction.

00:07 First, we have hcl reacting with mercury 1, or mercury, yeah, mercury 1 nitrate.

00:17 Mercury 1 is the polyatomic ion hg22 plus.

00:23 The cations will switch places.

00:25 We'll get mercury 1 combining with chloride and we'll get hydrogen combining with nitrate.

00:32 Hydrogen has a plus 1 charge, nitrate has a 1 minus charge, so we just need one of each of them.

00:38 Hg 2, 2 plus has a 2 plus charge, chloride has a 1 minus charge, so we'll need 2 chlorides for every hg2 2 plus.

00:46 And this is a solid.

00:49 To balance it, we have 2 chlorides here, we had 1 chloride there, so we put a 2 in front of the hcl, which gives us 2 hydrogen, so we're going to need a 2 there.

00:59 Now that we have 2 nitrogen, but we have 2 nitrogen, so it's balanced.

01:02 For the next one, we have potassium bisulfite reacting with nitric acid producing.

01:13 The cation will switch places.

01:15 So this hydrogen will go over here and we'll get h2 -s -o -3.

01:19 This potassium will go with the nitrate and we'll get potassium nitrate and it's balanced as is.

01:25 For the next one, we have aqueous ammonium chloride.

01:28 Ammonium is an h -4 plus.

01:30 Chloride is cl -minus, so we just need one of each of them.

01:32 And then we have aqueous lead to nitrate.

01:36 Lead 2 has a 2 plus charge.

01:38 Nitrate has a 1 minus charge, so we need 2 nitrates per lead...