A sample of 7.75 g of Mg(OH)2 is added to 25.0 mL of 0.200 𝑀 HNO3. c. How many moles of Mg(OH)2,HNO3, and Mg(NO3)2 are present after the reaction is complete?

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Determine the balanced chemical equation for the reaction: Mg(OH)_2 + 2HNO_3 \(\rightarrow\) Mg(NO_3)_2 + 2H_2O.

Calculate the moles of Mg(OH)_2 using its molar mass: \(\text{moles of Mg(OH)_2}\) = \(\frac{7.75 \text{ g}\)}{\(\text{molar mass of Mg(OH)_2}\)}.

Calculate the moles of HNO_3 using its concentration and volume: \(\text{moles of HNO_3}\) = 0.200 \(\text{ M}\) \(\times\) 0.0250 \(\text{ L}\).

Determine the limiting reactant by comparing the mole ratio from the balanced equation with the calculated moles of each reactant.

Calculate the moles of Mg(NO_3)_2 formed using the stoichiometry of the balanced equation and the limiting reactant.

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주요 개념

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Stoichiometry

Stoichiometry is the branch of chemistry that deals with the quantitative relationships between the reactants and products in a chemical reaction. It allows us to calculate the amounts of substances consumed and produced in a reaction based on balanced chemical equations. Understanding stoichiometry is essential for determining how many moles of each substance are present after a reaction, as it provides the ratios needed to relate the quantities of reactants and products.

Molarity

Molarity is a measure of concentration defined as the number of moles of solute per liter of solution. It is expressed in units of moles per liter (M). In this question, the molarity of HNO3 is given as 0.200 M, which indicates how many moles of HNO3 are present in the 25.0 mL solution. Calculating the moles of HNO3 is crucial for determining how much of the reactant is available to react with Mg(OH)2.

Neutralization Reaction

A neutralization reaction occurs when an acid reacts with a base to produce water and a salt. In this case, Mg(OH)2, a base, reacts with HNO3, an acid, to form Mg(NO3)2 and water. Understanding the products of this reaction is important for calculating the final amounts of each substance after the reaction is complete, as it helps identify the stoichiometric relationships and the limiting reactant.