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Chapter 15: Problem 191

How many moles of nitric acid do you need to prepare \(200 \mathrm{~mL}\) of an aqueous solution that has a pH of \(2.0\) ?

Short Answer

Expert verified
To prepare \(200 \mathrm{~mL}\) of an aqueous solution with a pH of 2.0, you'll need \(0.002\) moles of nitric acid (HNO₃).

Step by step solution

01

Calculate [H⁺] from pH

Using the pH formula, we can find the concentration of H⁺ ions in the solution. The formula to find [H⁺] is: \[ [H⁺] = 10^{-pH} \] Given the pH value as 2.0, plug in the value into the equation: \[ [H⁺] = 10^{-2} \]
02

Determine the concentration of HNO₃

Since nitric acid, HNO₃, is a strong acid, it will dissociate completely in water, producing equal concentrations of H⁺ and NO₃⁻ ions. The dissociation of nitric acid is as follows: \[ HNO₃ (aq) \rightarrow H⁺ (aq) + NO₃⁻ (aq) \] Therefore, the concentration of HNO₃ in the solution is equal to the concentration of H⁺ ions, which we calculated in Step 1.
03

Calculate the moles of HNO₃ required

Now, we can find the moles of HNO₃ needed for the 200 mL aqueous solution. We will apply the formula: \[moles= Molarity * Volume \] First, let's convert the volume from mL to L: \[Volume (L) = \frac{Volume (mL)}{1000} = \frac{200}{1000} = 0.2 L\] Now plug the values into the equation: \[moles = [H⁺] * Volume \] \[moles = 10^{-2} * 0.2 \]
04

Calculate the final answer

Multiply the values from Step 3: \[moles = 0.01 * 0.2 = 0.002 \] So, to prepare 200 mL of an aqueous solution with a pH of 2.0, 0.002 moles of nitric acid (HNO₃) are needed.

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Most popular questions from this chapter

Pyridine, \(\mathrm{C}_{5} \mathrm{H}_{5} \mathrm{~N}\), is a weak base. (a) Write the chemical equation for the reaction between pyridine and water. (b) List all species present in an aqueous solution of pyridine in order of concentration, highest to lowest. (c) In a 0.100 M pyridine solution, \(3.2 \%\) of the pyridine has reacted with water to form products. Calculate the concentration of all species present (except water) in \(1 \mathrm{~L}\) of a \(0.100\) M pyridine solution. (d) What is the pH of this solution?

What is the molar concentration of hydronium ion and hydroxide ion in pure water at \(25{ }^{\circ} \mathrm{C}\) ?

Why is the conjugate base of a weak acid like acetic acid often referred to as a salt of the acid?

A solution is prepared by dissolving \(2.50\) moles of \(\mathrm{LiOH}\) in enough water to get \(4.00 \mathrm{~L}\) of solution. What are the \(\mathrm{OH}^{-}\) and the \(\mathrm{H}_{3} \mathrm{O}^{+}\) molar concentrations?

Suppose \(2.0\) moles of sodium acetate, \(\mathrm{NaO}_{2} \mathrm{CCH}_{3}\), are dissolved in some water and then \(1.0 \mathrm{~L}\) of a \(1.0 \mathrm{M} \mathrm{HCl}\) solution is added. (a) Write the chemical reaction that occurs. (b) After the reaction, what are the predominant species in solution? How many moles of each species are there? (c) Is the resulting solution a buffer? If yes, explain why.
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