Write formulas for the acid and indicated solid that could...

Write formulas for the acid and indicated solid that could be used to prepare each of the following salts:
a. $\mathrm{CuCl}_2$ (solid is an oxide)
b. $\mathrm{MgSO}_4$ (solid is a carbonate)
c. LiBr (solid is a hydroxide)

Key Concepts

Reactivity of Basic Solids

Basic solids such as metal oxides, carbonates, and hydroxides react with acids in a predictable manner. Metal oxides typically yield water as a byproduct, carbonates release carbon dioxide upon reaction, and hydroxides form water. Understanding these reactivity patterns is key to selecting the appropriate solid for the synthesis of a particular salt.

Stoichiometry in Salt Preparation

Proper stoichiometric calculations ensure that the acid and basic solid react in the correct proportions, allowing for complete conversion to the desired salt without excess reactants. This is crucial for obtaining a pure product and optimizing reaction efficiency in salt synthesis.

Acid-Base Neutralization

This concept involves the reaction between an acid and a base to produce a salt and another product, often water or carbon dioxide. It is essential in salt synthesis because the acid provides the anion part of the salt while the basic solid offers the cation, allowing for controlled formation of the desired salt.

Transcript

00:01 Before we write these formulas for the following ionic compounds, we need to know that all ionic compounds have to be electrically neutral.

00:13 This means that some of positive charges and negative charges in each formula has to be zero.

00:21 So this gives the rule of writing the formula.

00:25 The subscript of the cate ion is numerically equal to the charge on the n -ion.

00:32 And a subscript of an ion is numerically equal to the charge on the cate ion.

00:38 If the charges for the cate ion and ion ion are the same numerically, then we don't need to write any subscripts.

00:45 This rule is also in accordance with the point that the formulas of ionic compounds are usually the same as their empirical formulas.

00:54 The subscripts is reduced to the smallest ratios possible.

01:00 Therefore, by using this rule, we can start writing the femurricular.

01:03 Of the compound in question.

01:06 First we have copper bromide.

01:10 Let's look at the table.

01:13 Copper, the question, gave us as a plus one charge.

01:19 How about bromide ion? right, bromide ion has a minus one charge and since the charge are numerically equal, we can just write the formula as c -u -b -r.

01:44 Next we have manganese oxide.

01:51 The question gives us magnesium at a plus -3 charge and from the table we can see that oxide ion usually have a two minus charge.

02:04 So by using the of writing formulas...

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