Textbook Question
Determine if each salt will form a solution that is acidic, basic, or pH-neutral. b. C2H5NH3NO3 c. K2CO3 d. RbI e. NH4ClO
Ch.16 - Acids and Bases
Chapter 16, Problem 7
A 0.115 M solution of a weak acid (HA) has a pH of 3.29. Calculate the acid ionization constant (Ka) for the acid.
Verified step by step guidance1
<Step 1: Understand the problem. We are given the concentration of a weak acid (HA) and the pH of the solution. We need to find the acid ionization constant (K_a).>
<Step 2: Convert the pH to the concentration of hydrogen ions [H^+]. Use the formula: [H^+] = 10^{-pH}.>
<Step 3: Write the expression for the ionization of the weak acid: HA \rightleftharpoons H^+ + A^-.>
<Step 4: Set up the expression for the acid ionization constant (K_a): K_a = \frac{[H^+][A^-]}{[HA]}.>
<Step 5: Assume that [H^+] = [A^-] and that the initial concentration of HA decreases by [H^+]. Substitute these values into the K_a expression and solve for K_a.>
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Open Question
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