Question #194668

Calculate the pH of an aqueous ammonia solution that has an OH-concentration of 3.9 × 103M. Is the solution more basic or acidic

Expert's answer

**Solution.**

"\\begin{bmatrix}\n OH^- \\\\\n\n\\end{bmatrix}=3.9\\sdot 10^3M;"

"\\begin{bmatrix}\nH^+ \\\\\n\n\\end{bmatrix}\\begin{bmatrix}\nOH^- \\\\\n\n\\end{bmatrix}=1\\sdot10^{-14}\\implies \\begin{bmatrix}\nH^+ \\\\\n\n\\end{bmatrix}=\\dfrac{1\\sdot10^{-14}}{\\begin{bmatrix}\n OH^- \\\\\n \n\\end{bmatrix}};"

"\\begin{bmatrix}\nH^+ \\\\\n\n\\end{bmatrix}=\\dfrac{1\\sdot10^{-14}}{\n 3.9\\sdot10^3 }=2.56\\sdot10^{-18};"

"pH=-log\\begin{bmatrix}\nH^+ \\\\\n\n\\end{bmatrix}" ;

"pH=-log(2.56\\sdot10^{-18})=17.59;"

The solution is basic.

**Answer: **"pH=17.59," the solution is basic.

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