Multiple Choice
What is the percent ionization of 0.0550 M solution of HC2H3O2?
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17. Acid and Base Equilibrium
The pH Scale
Multiple Choice
Calculate [OH−] of a lemon juice solution at 25°C with a [H+] = 5.7 × 10−4 M.
A
5.7 × 1010 M
B
4.7 × 10−11 M
C
2.7 × 10−18 M
D
1.7 × 10−11 M
Verified step by step guidance1
Identify the relationship between the concentration of hydrogen ions [H\^+] and hydroxide ions [OH\^-] in aqueous solution at 25°C, which is given by the ion-product constant of water: \(K_w = [H\^+][OH\^-]\).
Recall that at 25°C, the value of \(K_w\) is \(1.0 \times 10^{-14}\) M\^2.
Rearrange the equation to solve for the hydroxide ion concentration: \([OH\^-] = \frac{K_w}{[H\^+]}\).
Substitute the given hydrogen ion concentration \([H\^+] = 5.7 \times 10^{-4}\) M and the known \(K_w\) value into the equation.
Perform the division to find \([OH\^-]\), which will give the hydroxide ion concentration in the lemon juice solution.
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