Ionic Equilibria
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See all →- The pH of 0.1 M acetic acid (\(K_a=1.8\times10^{-5}\)) is approximately Answer: B. 2.87 [H^+]=√(K_aC)=sqrt1.8×10⁻⁶=1.34×10⁻³ M; pH ≈2.87 . 1
- The solubility of Ag2CrO4 in water is \(1\times10^{-4}\) mol L-1. Its solubility product is Answer: A. 4×10⁻¹² K_sp=(2s)²s=4s³=4×10⁻¹² . 1
- A buffer contains 0.02 M acetic acid and 0.2 M sodium acetate. If p\(K_a\) of acetic acid is 4.74, the pH of the buffer is Answer: B. 5.74 pH =pK_a+log[salt]/[acid]=4.74+log10=5.74 . 1