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Chapter 4: Problem 81

What volume of 0.0200 M calcium hydroxide is required to neutralize 35.00 mL of 0.0500 M nitric acid?

Short Answer

Expert verified
The volume of 0.0200 M calcium hydroxide required to neutralize 35.00 mL of 0.0500 M nitric acid is 43.75 mL.

Step by step solution

01

Write the balanced chemical equation

The balanced chemical equation for the neutralization reaction between calcium hydroxide (Ca(OH)₂) and nitric acid (HNO₃) is: Ca(OH)₂ + 2HNO₃ → Ca(NO₃)₂ + 2H₂O This equation shows that 1 mole of calcium hydroxide is needed to neutralize 2 moles of nitric acid.
02

Find moles of nitric acid

To find the moles of nitric acid, we can use the formula: Moles = Molarity × Volume Given that the molarity of nitric acid is 0.0500 M and the volume is 35.00 mL, we can convert the volume to liters and find the moles: Moles of nitric acid = 0.0500 M × 0.035 L = 0.00175 moles
03

Determine moles of calcium hydroxide required

From the balanced chemical equation, we know that one mole of calcium hydroxide is needed to neutralize two moles of nitric acid, so we can determine the moles of calcium hydroxide required: Moles of Ca(OH)₂ = (0.00175 moles of HNO₃) × (1 mol Ca(OH)₂ / 2 moles HNO₃) = 0.000875 moles
04

Calculate the volume of calcium hydroxide solution

Now, we know the moles of calcium hydroxide needed and the molarity of the calcium hydroxide solution. We can use these values to find the volume required using the formula: Volume = Moles / Molarity Volume of Ca(OH)₂ = 0.000875 moles / 0.0200 M = 0.04375 L = 43.75 mL So, the volume of 0.0200 M calcium hydroxide required to neutralize 35.00 mL of 0.0500 M nitric acid is 43.75 mL.

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Key Concepts

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

Neutralization Reaction
A neutralization reaction occurs when an acid and a base react to form water and a salt. This type of chemical reaction is crucial in understanding many everyday processes, such as digestion and cleaning.

In the context of our problem, a neutralization reaction is taking place between nitric acid (HNO₃), an acid, and calcium hydroxide (Ca(OH)₂), a base. When these two substances react, they form calcium nitrate (Ca(NO₃)₂), which is a salt, and water. The general equation for a neutralization reaction is:
  • Acid + Base → Salt + Water
This type of reaction is important because it allows us to make predictions about the quantities of reactants needed, as well as the products formed during the reaction.

Moreover, this balanced reaction reveals a key aspect: stoichiometry. We see that one mole of calcium hydroxide is required for every two moles of nitric acid. This stoichiometric relationship helps us understand how much base is needed to neutralize a given amount of acid. Using this relationship, we can effectively manage and predict the outcomes of chemical reactions.
Molarity Calculations
Molarity is a measure of the concentration of a solution, defined as the number of moles of solute per liter of solution. Understanding and calculating molarity is essential for solving problems involving solutions, such as determining the volume needed to neutralize acids or bases.

When dealing with the given problem, we start by calculating the moles of nitric acid present. The molarity formula, given by \[\text{Moles} = \text{Molarity} \times \text{Volume} \]allows us to determine the molar amount of the acid or base. Since the problem provides the molarity (0.0500 M) and volume (35.00 mL) of the nitric acid, we must first convert the volume to liters. This is because molarity is based on liters, and we have: \[35.00 \text{ mL} = 0.035 \text{ L}\]Plugging these values into the formula, we get: \[\text{Moles of } HNO_3 = 0.0500 \text{ M} \times 0.035 \text{ L} = 0.00175\text{ moles}\]

Therefore, knowing the moles of acid present allows us to proceed to determine the needed amount of base through the stoichiometric relationships obtained from the balanced chemical equation.
Chemical Equation Balancing
Balancing chemical equations is fundamental in any chemical reaction problem because it allows for the correct application of stoichiometry. This ensures that the number of atoms for each element is conserved throughout the reaction.

In this problem, the balanced equation for the neutralization reaction between calcium hydroxide and nitric acid is:
\[\text{Ca(OH)}_2 + 2\text{HNO}_3 \rightarrow \text{Ca(NO}_3)_2 + 2\text{H}_2\text{O}\] The importance of balancing the equation comes from recognizing the ratio of reactants to each other. For example, the equation shows that one mole of calcium hydroxide reacts with two moles of nitric acid.

Balanced chemical equations are the backbone of accurate stoichiometric calculations. They help in determining the proportionate amounts of reactants required or products formed in reaction scenarios. Without balancing, any further calculations or predictions about reaction outputs would be inaccurate. Balancing also helps ensure adherence to the conservation of mass principle, a key foundation of chemistry.

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Most popular questions from this chapter

Carminic acid, a naturally occurring red pigment extracted from the cochineal insect, contains only carbon, hydrogen, and oxygen. It was commonly used as a dye in the first half of the nineteenth century. It is 53.66% C and 4.09% H by mass. A titration required 18.02 mL of 0.0406 M NaOH to neutralize 0.3602 g carminic acid. Assuming that there is only one acidic hydrogen per molecule, what is the molecular formula of carminic acid?

The unknown acid \(\mathrm{H}_{2} \mathrm{X}\) can be neutralized completely by \(\mathrm{OH}^{-}\) according to the following (unbalanced) equation: $$\mathrm{H}_{2} \mathrm{X}(a q)+\mathrm{OH}^{-}(a q) \longrightarrow \mathrm{X}^{2-}(a q)+\mathrm{H}_{2} \mathrm{O}(i) $$ The ion formed as a product, \(X^{2-},\) was shown to have 36 total electrons. What is element X? Propose a name for \(\mathrm{H}_{2} \mathrm{X}\) . To completely neutralize a sample of \(\mathrm{H}_{2} \mathrm{X}, 35.6 \mathrm{mL}\) of 0.175 \(\mathrm{M}\) \(\mathrm{OH}^{-}\) solution was required. What was the mass of the \(\mathrm{H}_{2} \mathrm{X}\) sample used?

Some of the substances commonly used in stomach antacids are \(\mathrm{MgO}, \mathrm{Mg}(\mathrm{OH})_{2},\) and \(\mathrm{Al}(\mathrm{OH})_{3.}\) a. Write a balanced equation for the neutralization of hydrochloric acid by each of these substances. b. Which of these substances will neutralize the greatest amount of 0.10 M HCl per gram?

Many over-the-counter antacid tablets are now formulated using calcium carbonate as the active ingredient, which enables such tablets to also be used as dietary calcium supplements. As an antacid for gastric hyperacidity, calcium carbonate reacts by combining with hydrochloric acid found in the stomach, producing a solution of calcium chloride, converting the stomach acid to water, and releasing carbon dioxide gas (which the person suffering from stomach problems may feel as a “burp”). Write the balanced chemical equation for this process.

The blood alcohol \(\left(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\right)\) level can be determined by tirrating a sample of blood plasma with an acidic potassium dichromate solution, resulting in the production of \(\mathrm{Cr}^{3+}(a q)\) and carbon dioxide. The reaction can be monitored because the dichromate ion \(\left(\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}\right)\) is orange in solution, and the \(\mathrm{Cr}^{3+}\) ion is green. The unbalanced redox equation is $$\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}(a q)+\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}(a q) \rightarrow \mathrm{Cr}^{3+}(a q)+\mathrm{CO}_{2}(g)$$ If 31.05 \(\mathrm{mL}\) of 0.0600\(M\) potassium dichromate solution is required to titrate 30.0 \(\mathrm{g}\) of blood plasma, determine the mass percent of alcohol in the blood.
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