Textbook Question
For each strong base solution, determine [OH–], [H3O+], pH, and pOH. c. 1.9×10–4 M KOH
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Ch.16 - Acids and Bases
Chapter 16, Problem 84
Determine the pH of a solution that is 1.55% NaOH by mass. Assume that the solution has a density of 1.01 g/mL.
Verified step by step guidance1
<Calculate the mass of NaOH in 100 g of solution: Since the solution is 1.55% NaOH by mass, there are 1.55 g of NaOH in 100 g of solution.>
<Determine the volume of the solution: Use the density to find the volume. Since the density is 1.01 g/mL, the volume of 100 g of solution is 100 g / 1.01 g/mL.>
<Calculate the molarity of the NaOH solution: First, find the number of moles of NaOH using its molar mass (approximately 40.00 g/mol). Then, divide the moles of NaOH by the volume of the solution in liters to find the molarity.>
<Determine the concentration of OH⁻ ions: Since NaOH is a strong base, it dissociates completely in water. Therefore, the concentration of OH⁻ ions is equal to the molarity of the NaOH solution.>
<Calculate the pH of the solution: Use the concentration of OH⁻ ions to find the pOH of the solution. Then, use the relationship pH + pOH = 14 to find the pH.>
Related Practice
Textbook Question
For each strong base solution, determine [OH–], [H3O+], pH, and pOH. d. 5.0×10–4 M Ca(OH)2
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Textbook Question
Determine the pH of a solution that is 3.85% KOH by mass. Assume that the solution has density of 1.01 g/mL.
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Open Question
What volume of 0.855 M KOH solution is required to make 3.55 L of a solution with a pH of 12.4?
Open Question
What volume of a 15.0% by mass NaOH solution, which has a density of 1.116 g/mL, should be used to make 5.00 L of an NaOH solution with a pH of 10.8?
Textbook Question
Write equations showing how each weak base ionizes water to form OH–. Also write the corresponding expression for Kb. a. NH3 b. HCO3– c. CH3NH2