Multiple Choice
Determine the pH of a solution made by dissolving 6.1 g of sodium cyanide, NaCN, in enough water to make a 500.0 mL of solution. (MW of NaCN = 49.01 g/mol). The Ka value of HCN is 4.9 x 10-10.
17. Acid and Base Equilibrium
The pH Scale
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What is the percent ionization of 0.0550 M solution of HC2H3O2?
A
0.017%
B
1.7%
C
98%
D
0.11%
Verified step by step guidance1
Identify the chemical species involved: HC2H3O2 (acetic acid) is a weak acid that partially ionizes in water to form H+ and C2H3O2- ions.
Write the ionization equation for acetic acid: HC2H3O2 ⇌ H+ + C2H3O2-.
Use the expression for percent ionization: \( \text{Percent Ionization} = \left( \frac{[\text{H}^+]}{[\text{HC}_2\text{H}_3\text{O}_2]_{\text{initial}}} \right) \times 100 \).
Determine the concentration of H+ ions at equilibrium. This can be found using the acid dissociation constant (Ka) for acetic acid and the initial concentration of the acid.
Substitute the values into the percent ionization formula to calculate the percent ionization of the solution.
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