Ch.16 - Acid-Base Equilibria

Problem 43b

Chapter 16, Problem 43b

Calculate the pH of each of the following strong acid solutions: (b) 1.52 g of HNO3 in 575 mL of solution

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Calculate the number of moles of HNO_3 using its molar mass. The molar mass of HNO_3 is approximately 63.01 g/mol.

Convert the mass of HNO_3 (1.52 g) to moles by dividing by the molar mass.

Determine the concentration of HNO_3 in the solution by dividing the number of moles by the volume of the solution in liters (575 mL = 0.575 L).

Since HNO_3 is a strong acid, it dissociates completely in water. Therefore, the concentration of HNO_3 is equal to the concentration of H^+ ions.

Calculate the pH of the solution using the formula pH = -\log[H^+].

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Strong Acids

Strong acids, such as nitric acid (HNO3), completely dissociate in water, meaning that all the acid molecules break apart into their constituent ions. This complete ionization is crucial for calculating the concentration of hydrogen ions (H+) in solution, which directly affects the pH.

pH Scale

The pH scale is a logarithmic scale used to measure the acidity or basicity of a solution, ranging from 0 to 14. A pH of 7 is neutral, while values below 7 indicate acidic solutions and values above 7 indicate basic solutions. The pH is calculated using the formula pH = -log[H+], where [H+] is the concentration of hydrogen ions in moles per liter.

Concentration Calculation

To calculate the concentration of H+ ions in a solution, one must first determine the number of moles of the solute (in this case, HNO3) and then divide by the volume of the solution in liters. The formula used is: concentration (M) = moles of solute / volume of solution (L). This concentration is essential for determining the pH of the solution.

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Addition of phenolphthalein to an unknown colorless solution does not cause a color change. The addition of bromthymol blue to the same solution leads to a yellow color. (c) What other indicator or indicators would you want to use to determine the pH of the solution more precisely?

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Open Question

Is each of the following statements true or false? (a) All strong acids contain one or more H atoms. (b) A strong acid is a strong electrolyte. (c) A 1.0-M solution of a strong acid will have pH = 1.0.

Open Question

Determine whether each of the following is true or false: (a) All strong bases are salts of the hydroxide ion. (b) The addition of a strong base to water produces a solution of pH > 7.0. (c) Because Mg(OH)2 is not very soluble, it cannot be a strong base.

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Calculate the pH of each of the following strong acid solutions: (b) 0.225 g of HClO3 in 2.00 L of solution

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Open Question

Calculate [OH-] and pH for (a) 1.5 × 10^-3 M Sr(OH)_2 (b) 2.250 g of LiOH in 250.0 mL of solution (c) 1.00 mL of 0.175 M NaOH diluted to 2.00 L (d) a solution formed by adding 5.00 mL of 0.105 M KOH to 15.0 mL of 9.5 × 10^-2 M Ca(OH)_2.

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Calculate 3OH-4 and pH for each of the following strong base solutions: (c) 10.0 mL of 0.0105 M Ca1OH22 diluted to 500.0 mL

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