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Predict the products for the reactions given below. Be sure to balance each equation. a. \(\mathrm{HF}(a q)+\mathrm{NaOH}(a q) \longrightarrow\) b. \(\mathrm{HCl}(a q)+\mathrm{Mg}(\mathrm{OH})_{2}(a q) \longrightarrow\) c. \(\mathrm{HF}(a q)+\mathrm{N} \mathrm{H}_{4} \mathrm{OH}(a q) \longrightarrow\) d. \(\mathrm{CH}_{3} \mathrm{COOH}(a q)+\mathrm{NaOH}(a q) \longrightarrow\) e. \(\mathrm{HNO}_{3}(a q)+\mathrm{Mg}(\mathrm{OH})_{2}(a q) \longrightarrow\) f. \(\mathrm{HNO}_{3}(a q)+\mathrm{NH}_{4} \mathrm{OH}(a q) \longrightarrow\) g. \(\mathrm{CH}_{3} \mathrm{COOH}(a q)+\mathrm{Mg}(\mathrm{OH})_{2}(a q) \longrightarrow\) \(\mathrm{h} . \mathrm{CH}_{3} \mathrm{COOH}(a q)+\mathrm{NH}_{4} \mathrm{OH}(a q) \longrightarrow\) i. \(\mathrm{H}_{2} \mathrm{SO}_{4}(a q)+\mathrm{HNO}_{3}(a q) \longrightarrow\) j. \(\mathrm{H}_{2} \mathrm{SO}_{4}(a q)+\mathrm{Mg}(\mathrm{OH})_{2}(a q) \longrightarrow\)

Step by step solution

01

Reaction HF with NaOH

The reaction involves the neutralization of hydrofluoric acid (HF) with sodium hydroxide (NaOH). This produces sodium fluoride (NaF) and water (H鈧侽).Balanced Equation: \[\mathrm{HF} + \mathrm{NaOH} \longrightarrow \mathrm{NaF} + \mathrm{H}_{2}\mathrm{O}\]

02

Reaction HCl with Mg(OH)鈧�

Hydrochloric acid (HCl) reacts with magnesium hydroxide (Mg(OH)鈧�), leading to the formation of magnesium chloride (MgCl鈧�) and water (H鈧侽).Balanced Equation: \[2\mathrm{HCl} + \mathrm{Mg(OH)}_{2} \longrightarrow \mathrm{MgCl}_{2} + 2\mathrm{H}_{2}\mathrm{O}\]

03

Reaction HF with NH鈧凮H

Hydrofluoric acid (HF) reacts with ammonium hydroxide (NH鈧凮H) to form ammonium fluoride (NH鈧凢) and water (H鈧侽).Balanced Equation: \[\mathrm{HF} + \mathrm{NH}_{4}\mathrm{OH} \longrightarrow \mathrm{NH}_{4}\mathrm{F} + \mathrm{H}_{2}\mathrm{O}\]

04

Reaction CH鈧僀OOH with NaOH

Acetic acid (CH鈧僀OOH) is neutralized by sodium hydroxide (NaOH) to form sodium acetate (CH鈧僀OONa) and water (H鈧侽).Balanced Equation: \[\mathrm{CH}_{3}\mathrm{COOH} + \mathrm{NaOH} \longrightarrow \mathrm{CH}_{3}\mathrm{COONa} + \mathrm{H}_{2}\mathrm{O}\]

05

Reaction HNO鈧� with Mg(OH)鈧�

Nitric acid (HNO鈧�) reacts with magnesium hydroxide (Mg(OH)鈧�) to form magnesium nitrate (Mg(NO鈧�)鈧�) and water (H鈧侽).Balanced Equation: \[2\mathrm{HNO}_{3} + \mathrm{Mg(OH)}_{2} \longrightarrow \mathrm{Mg(NO}_{3})_{2} + 2\mathrm{H}_{2}\mathrm{O}\]

06

Reaction HNO鈧� with NH鈧凮H

Nitric acid (HNO鈧�) reacts with ammonium hydroxide (NH鈧凮H) to form ammonium nitrate (NH鈧凬O鈧�) and water (H鈧侽).Balanced Equation: \[\mathrm{HNO}_{3} + \mathrm{NH}_{4}\mathrm{OH} \longrightarrow \mathrm{NH}_{4}\mathrm{NO}_{3} + \mathrm{H}_{2}\mathrm{O}\]

07

Reaction CH鈧僀OOH with Mg(OH)鈧�

Acetic acid (CH鈧僀OOH) reacts with magnesium hydroxide (Mg(OH)鈧�) to form magnesium acetate {Mg(CH鈧僀OO)鈧倉 and water (H鈧侽).Balanced Equation: \[2\mathrm{CH}_{3}\mathrm{COOH} + \mathrm{Mg(OH)}_{2} \longrightarrow \mathrm{Mg(CH}_{3}\mathrm{COO})_{2} + 2\mathrm{H}_{2}\mathrm{O}\]

08

Reaction CH鈧僀OOH with NH鈧凮H

Acetic acid (CH鈧僀OOH) reacts with ammonium hydroxide (NH鈧凮H) to yield ammonium acetate (NH鈧凜H鈧僀OO) and water (H鈧侽).Balanced Equation: \[\mathrm{CH}_{3}\mathrm{COOH} + \mathrm{NH}_{4}\mathrm{OH} \longrightarrow \mathrm{NH}_{4}\mathrm{CH}_{3}\mathrm{COO} + \mathrm{H}_{2}\mathrm{O}\]

09

Reaction H鈧係O鈧� with HNO鈧�

When sulfuric acid (H鈧係O鈧�) reacts with nitric acid (HNO鈧�), the reaction product typically involves the formation of nitronium cations (NO鈧傗伜), but since this is not a basic reaction, it may not form neutral products.Balanced Equation: \[\text{Typically does not form a neutral compound under these conditions.}\]

10

Reaction H鈧係O鈧� with Mg(OH)鈧�

Sulfuric acid (H鈧係O鈧�) reacts with magnesium hydroxide (Mg(OH)鈧�) to form magnesium sulfate (MgSO鈧�) and water (H鈧侽).Balanced Equation: \[\mathrm{H}_{2}\mathrm{SO}_{4} + \mathrm{Mg(OH)}_{2} \longrightarrow \mathrm{MgSO}_{4} + 2\mathrm{H}_{2}\mathrm{O}\]

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Neutralization Reactions

A neutralization reaction is a type of chemical reaction that occurs when an acid and a base react to form water and a salt. It is a special case of double displacement reactions. Neutralization reactions are essential in various real-life applications like pharmaceuticals, agriculture, and environmental management.
A common example of a neutralization reaction is when hydrochloric acid (HCl) reacts with sodium hydroxide (NaOH) to form water (H鈧侽) and sodium chloride (NaCl), a common table salt.
These reactions typically follow the general form:

• Acid + Base 鈫� Salt + Water

Understanding neutralization reactions helps in predicting the outcomes of acid-base combinations and their respective practical applications.

Balancing Chemical Equations

Balancing chemical equations is crucial to accurately represent the conservation of mass in a chemical reaction. Each element must have the same number of atoms on both sides of the equation. This ensures the reaction respects the Law of Conservation of Mass.
In practice, balancing equations involves identifying and adjusting the coefficients before each compound to ensure equal numbers of each type of atom appear on both sides of the equation.
For example, the balanced equation for the reaction of hydrochloric acid and magnesium hydroxide would be:

• Unbalanced: HCl + Mg(OH)鈧� 鈫� MgCl鈧� + H鈧侽
• Balanced: 2HCl + Mg(OH)鈧� 鈫� MgCl鈧� + 2H鈧侽

Balancing ensures that we account for every molecule involved in the process, providing accurate stoichiometric calculations.

Acid-Base Reactions

Acid-base reactions are a critical part of chemistry involving the transfer of protons between reactants. An acid donates a proton (H鈦� ion) to a base, which accepts it. These reactions are characterized by the change in pH, a measure of acidity or alkalinity of the solution.
Typically, acid-base reactions lead to the formation of water and a salt, making them a subset of neutralization reactions.
Key points to consider in acid-base reactions include:

• The strength of acids and bases determines the completeness of the reaction.
• Strong acids/bases dissociate completely in water, whereas weak acids/bases do not.

The practicality of these reactions extends to various fields including medicine, where it helps in drug design and food chemistry.

Stoichiometry

Stoichiometry is the field of chemistry concerned with the proportions of reactants and products in chemical reactions. It enables chemists to determine how much of each substance is needed or produced in a reaction.
To use stoichiometry effectively, one needs a balanced chemical equation, which serves as a guide to find the mole ratio of reactants and products.
Consider the reaction of hydrofluoric acid with sodium hydroxide:

• Balanced equation: HF + NaOH 鈫� NaF + H鈧侽
• The mole ratio indicates that one mole of HF reacts with one mole of NaOH to produce one mole each of NaF and H鈧侽.

Understanding stoichiometry is crucial for calculating yields and reactant amounts, playing a fundamental role in chemical production and experimentation.