Multiple Choice
Calculate the concentration of a NaOH solution that has a pH of 11.3.
17. Acid and Base Equilibrium
pH of Strong Acids and Bases
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Given the following solutions at 25°C, determine the pH and classify each as acidic, basic, or neutral: Solution 1: [H3O+] = 3.5×10^-3 M Solution 2: [OH−] = 3.8×10^-7 M Solution 3: [H3O+] = 1.8×10^-7 M Which of the following correctly describes the pH and classification for Solution 1?
A
pH = 7.00, neutral
B
pH = 4.46, acidic
C
pH = 2.46, acidic
D
pH = 11.54, basic
Verified step by step guidance1
To determine the pH of a solution, use the formula: . For Solution 1, substitute the given concentration of hydronium ions, = 3.5×10-3 M, into the formula.
Calculate the pH using the formula: . This will give you the pH value for Solution 1.
Once you have the pH value, compare it to the neutral pH of 7. If the pH is less than 7, the solution is acidic; if it is greater than 7, the solution is basic; if it is equal to 7, the solution is neutral.
For Solution 2, use the formula for pOH: . Substitute the given concentration of hydroxide ions, = 3.8×10-7 M, into the formula to find the pOH.
Convert the pOH to pH using the relationship: . Then classify the solution as acidic, basic, or neutral based on the pH value.
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